The standard enthalpy change for the combustion of C3H6(g) + H2(g) → C3H8(g) at 25°C is -219.4 kJ/mol.
Explanation:The standard enthalpy change for the reaction is obtained by calculating the difference between the enthalpy of the products and the enthalpy of the reactants. In this case, the enthalpy change can be determined using the enthalpy of formation values for the compounds involved. The balanced equation for the combustion of propane is:
C3H6(g) + H2(g) → C3H8(g)
The enthalpy change can be calculated as follows:
∆H° = ∑∆H°f(products) - ∑∆H°f(reactants)
∆H° = [2*(∆H°f(CO2(g))) + ∆H°f(H2O(l))] - [∆H°f(C3H6(g)) + ∆H°f(H2(g))]
Substitute the given values for the enthalpies of formation:
∆H° = [2*(-393.5 kJ/mol) + (-285.8 kJ/mol)] - [(-2058.3 kJ/mol) + 0 kJ/mol]
Simplify the equation:
∆H° = -219.4 kJ/mol
Therefore, the standard enthalpy change for the combustion of C3H6(g) + H2(g) → C3H8(g) at 25°C is -219.4 kJ/mol.
Part A Describe the electrodes in this nickel-copper galvanic cell. Drag the appropriate items to their respective bins. View Available Hint(s) ResetHelp Nickel Copper Standard reduction potentials for nickel(II) and copper(II) The standard reduction potential for a substance indicates how readily that substance gains electrons relative to other substances at standard conditions. The more positive the reduction potential, the more easily the substance gains electrons. Consider the following: Ni2+(aq)+2e−→Ni(s),Cu2+(aq)+2e−→Cu(s), E∘red=−0.230 V E∘red=+0.337 V Part B What is the standard potential, E∘cell, for this galvanic cell? Use the given standard reduction potentials in your calculation as appropriate.
Answer:
Part-A:
Anode is Nickel and Cathode is copper.
Part -B:
[tex]E^{0}_{cell}[/tex] of the reaction is 0.567V.
Explanation:
Nickel-Copper cell electrodes are "Ni" and "Cu" rod.
Nickel electrode is dipped in [tex]Ni^{+2}[/tex] solution.
Copper electrode dipped in [tex]Cu^{+2}[/tex] solution.
Part -A:
Anode:
At anode oxidation takes place
[tex]Ni(s) \rightarrow Ni^{+2}(aq)+2e^{-}[/tex]
Hence, anode is Nickel.
Cathode:
At cathode reduction takes place.
[tex]Cu^{+2}+2e^{-} \rightarrow Cu(s)[/tex]
Hence, Cathode is copper.
Part-B:
[tex]E^{0}_{cell}=E^{0}_{cathode}-E^{0}_{anode}[/tex]
[tex]=0.337-(-0.230)=0.567V[/tex]
Hence, [tex]E^{0}_{cell}[/tex] of the reaction is 0.567V.
Anodes and cathodes are the electrodes where oxidation and reduction take place.
What are the electrodes in galvanic cell?Electrochemical cells have two electrodes which is called anode and cathode. The anode is the electrode where oxidation occurs while the other hand, cathode is the electrode where reduction takes place so we can conclude that anodes and cathodes are the electrodes where oxidation and reduction take place.
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A coal-burning power plant produces 500 megawatts of electricity while burning 225,000 kg of coal per hour (almost 250 tons each hour!). If the coal has an average energy content of 20 million Joules per kg, determine the efficiency of the power plant.
Answer:
40%
Explanation:
The efficiency of a plant is determined by
[tex]eff=\frac{E_{produced}}{E_{in}}[/tex]
Our produced energy is
[tex]500 \ MW[/tex]
While the input energy can be calculated
[tex]E_{in}=number\ of \ coal \ in \ * energy\ per\ coal\ unit\\ =\frac{225000}{3600}coal/ s\ *20\ MJ/coal\\ = 1250\ MW[/tex]
So, the efficiency of plant is
[tex]eff=\frac{500}{1250}}\\ 0.4[/tex]
or 40% efficient
Final answer:
The efficiency of the coal-burning power plant in question is 40%, calculated by comparing the electrical energy output to the energy input from burning coal.
Explanation:
To determine the efficiency of the coal-burning power plant, we compare the energy output in the form of electricity to the energy input from burning coal. First, calculate the total energy input per hour by multiplying the amount of coal burned by the average energy content of the coal. Then, convert the electrical energy output from megawatts to joules per hour. Finally, calculate efficiency using the formula: Efficiency (%) = (Energy output / Energy input) × 100.
Here are the calculations:
Energy input per hour = 225,000 kg/hour × 20× 106 J/kg = 4.5× 1012 J/hourEnergy output per hour = 500 MW × 3.6× 106 J/MWs = 1.8× 1012 J/hourEfficiency = (1.8× 1012 J/hour / 4.5× 1012 J/hour) × 100 = 40%Thus, the efficiency of the power plant is 40%.
The equilibrium: 2 NO2(g) \Longleftrightarrow⇔ N2O4(g) has Kc = 4.7 at 100ºC. What is true about the rates of the forward (ratefor) and reverse (raterev) reactions initially and at equilibrium if an empty container is filled with just NO2?
Initial: forward rate < reverse rate Equilibrium: forward rate > reverse rate
Initial: forward rate > reverse rate Equilibrium: forward rate > reverse rate
Initial: forward rate > reverse rate Equilibrium: forward rate = reverse rate
Initial: forward rate = reverse rate Equilibrium: forward rate = reverse rate
Answer:
Initial: forward rate > reverse rate Equilibrium: forward rate = reverse rateExplanation:
2NO₂(g) → N₂O₄(g) Kc=4.7
The definition of equilibrium is when the forward rate and the reverse rate are equal.
Because in the initial state there's only NO₂, there's no possibility for the reverse reaction (from N₂O₄ to NO₂). Thus the forward rate will be larger than the reverse rate.
The most common method for the synthesis of unsymmetrical ethers is the Williamson synthesis, a reaction (SN2) of an alkoxide ion with an alkyl halide. Two pathways are possible, but often one is preferred. Construct the preferred pathway for the synthesis of 2-propoxypropane from propene, with propene-derived alkyl halide and alkoxide intermediates, by dragging the appropriate intermediates and reagents into their bins. Not every given reagent or intermediate will be used.
Answer:
2- propanol treated with metal base NaH followed by hydrogen bromide to form 2- propoxypropane.
Explanation:
Formation of secondary halide:
Firstly propene reacts with sulfuric acid or water to form 2- Propanol.
Formation of primary halide:
Also, according to the Anti markovinikov rule propene undergoes addition to the hydrogen bromide in the presence of peroxide to form 1- bromopropane.
The secondary halide i.e, 2- propanol treated with metal base NaH to form sodium isopropoxide. Further treated with hydrogen bromide to form 2- Propoxypropane. This reaction follows [tex]S_{N}2[/tex] mechanism.
The overall reaction is as follows.
The preferred pathway for the synthesis of 2-propoxypropane from propene in the Williamson synthesis involves the reaction of propene with an alkyl halide and an alkoxide ion.
Explanation:The preferred pathway for the synthesis of 2-propoxypropane from propene in the Williamson synthesis involves the reaction of propene with an alkyl halide and an alkoxide ion. The alkoxide ion is formed by treating an alcohol with a strong base, such as sodium hydride (NaH). The alkyl halide is then added to the alkoxide ion, resulting in the formation of the desired product, 2-propoxypropane.
Alcohol + Strong Base (NaH) → Alkoxide Ion
Alkoxide Ion + Alkyl Halide → 2-Propoxypropane
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Write balanced half-reactions for the following redox reaction: 5Cl2(g)+2Mn+2(aq)+8H2O(l)→ 10Cl−(aq)+2MnO−4(aq)+16H+(aq)a. reduction: __.b. oxidation: ___.
Answer:
a. 5Cl₂ + 10e⁻ → 10Cl⁻
b. 4H₂O + Mn²⁺ → MnO₄⁻ + 5e⁻ + 8H⁺
Explanation:
5Cl2(g)+2Mn+2(aq)+8H2O(l)→ 10Cl−(aq)+2MnO4-(aq)+16H+(aq)
First of all, think in all the oxidation numbers for each compound. That's the way, you can notice the half reaction.
When the oxidation number, decrease, you have reduction. Compound is wining electrons.
When the oxidation number increase, you have oxidation. Compound is losing electrons.
Cl2(g) - Atoms in ground state, has 0 as oxidation number. In products side, you have the anion chloride which act with -1, so chlorine has been reduced.
Mn2+ - The manganese ion is already telling you with 2, that is its oxidation number. On the side products, the element was transformed into the permanganate anion; how oxygen acts with -2 and there are 4 atoms, it has -8 as oxidation state but since the general charge is -1 the Mn is acting with +7. From + 2 it went to +7, which means that it increased, so it has oxidized.
5Cl₂ + 10e⁻ → 10Cl⁻ - REDUCTION
The chlorine had to gain 1 electron to go from 0 to -1, but being a diatomic molecule were 2 electrons, but finally so that the charges are balanced and because there are 5 moles, it ends up gaining 10 electrons.
Mn²⁺ → MnO₄⁻ - OXIDATION
Look that in main reaction we have H⁺, that is the clue to notice us, that we are in acidic medium. So if we have 4 O, in MnO₄⁻, we have to complete with 4H₂O in the other side of O. And to ballance the protons, we have to add 8H⁺ in product side
4H₂O + Mn²⁺ → MnO₄⁻ + 5e⁻ + 8H⁺ OXIDATION
How do u finish this?. You have to multipply .2, the oxidation one to balance the e⁻ so, they can be cancelled.
5Cl₂ + 10e⁻ → 10Cl⁻
(4H₂O + Mn²⁺ → MnO₄⁻ + 5e⁻ + 8H⁺ ).2
8H₂O + 2Mn²⁺ → 2MnO₄⁻ + 10e⁻ + 16H⁺
5Cl₂ + 10e⁻ + 8H₂O + 2Mn²⁺ → 10Cl⁻ + 2MnO₄⁻ + 10e⁻ + 16H⁺
5Cl₂ + 8H₂O + 2Mn²⁺ → 10Cl⁻ + 2MnO₄⁻ + 16H⁺
The half-reactions for the given redox reaction includes the reduction of Mn2+(aq) to MnO4-(aq) with the addition of 5 electrons and 8 hydrogen ions and the oxidation of Cl2(g) to 10 Cl-(aq), losing 10 electrons in the process.
Explanation:The redox reaction is related to the process of reduction and oxidation which often takes place in electrochemical cells. This process includes half-reactions, which separately represent the oxidation and reduction in the redox reaction. For the given equation, the oxidation and reduction half-reactions are as follows:
a. Reduction: Mn2+(aq) + 5e- + 8H+(aq) → MnO4-(aq) + 4H2O(l).
b. Oxidation: Cl2(g) → 10e- + 10Cl-(aq).
These equations represent the transformation of Mn2+ and Cl2 in the given redox reaction where Mn2+ is being reduced and Cl2 is being oxidized.
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A buffer is prepared by mixing hypochlorous acid ( HClO ) and sodium hypochlorite ( NaClO ) . If a strong base, such as NaOH , is added to this buffer, which buffer component neutralizes the additional hydroxide ions ( OH − ) ? ClO − HClO Write a balanced chemical equation for the reaction of the selected buffer component and the hydroxide ion ( OH − ) . Do not include physical states.
The chemical equation for the neutralization of hydroxide ion by HClO is:
HClO + OH ---> H2O + ClO-What a buffer?A buffer is a solution which resists changes to its pH when a small quantity of strong acid or base is added to it.
A solution of weak acid such as hypochlorous acid (HClO) and its basic salt that is sodium hypochlorite (NaClO) forms a buffer solution
When a strong base is added to the buffer, the excess hydroxide ion will be neutralized by hydrogen ions from the acid, HClO.
The chemical equation for the neutralization of hydroxide ion with acid follows:
HClO + OH ---> H2O + ClO-Therefore, the balanced chemical equation is such that the excess OH- is neutralized.
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Which statements are true?
a. The evaporation of water is an exothermic process.
b. A combustion reaction is exothermic.
c. When energy is transferred as heat from the surroundings to the system, Deta H is negative.
d. When energy is transferred as heat from the system to the surroundings, Deta H is negative.
e. for an exothermic reaction Deta H is positive.
f. for an endothermic reaction Deta H is positive.
Explanation:
Evaporation is defined as a process in which liquid state of water is changing into vapor state.So, we need to break the bonds of liquid substance in order to convert it into vapor state. And, energy is absorbed for breaking of bonds which means that evaporation is an endothermic process.
Hence, the statement evaporation of water is an exothermic process is false.
When a hydrocarbon reacts with oxygen and leads to the formation of carbon dioxide and water then this type of reaction is known as combustion reaction.A combustion reaction will always release heat energy. Hence, combustion reaction is exothermic in nature.
When energy is transferred as heat from the surroundings to the system then it means energy is being absorbed by the system. And, absorption of heat is an endothermic process for which [tex]\Delta H[/tex] is positive.Whereas when energy is transferred from system to the surrounding then it means energy is released by the system which is an exothermic process.Hence, for an exothermic process value of [tex]\Delta H[/tex] is negative.
Thus, we can conclude that statements which are true are as follows.
A combustion reaction is exothermic.When energy is transferred as heat from the system to the surroundings, [tex]\Delta H[/tex] is negative.For an endothermic reaction Deta H is positive.Consider the following generic chemical equation. 2A+4B→3C What is the limiting reactant when each of the following amounts of A and B are allowed to react? Part A 2 molA; 5 molB 2 ; 5 B A SubmitRequest Answer Part B 1.8 molA; 4 molB 1.8 ; 4 B A SubmitRequest Answer Part C 3 molA; 4 molB 3 ; 4 B A SubmitRequest Answer Part D 22 molA; 40 molB 22 ; 40 B A
Answer:
A. Limiting reactant is A.
B. Limiting reactant is A.
C. Limiting reactant is B.
D. Limiting reactant is B.
Explanation:
It is possible to find the limiting reactant for a reaction taking the moles of a reactant that will react and using the chemical equation find the moles of the other reactant you will need.
For the reaction:
2A + 4B → 3C
A. 2 moles A requires:
2molA×[tex]\frac{4molB}{2molA}[/tex]= 4moles of B
As you have 5 moles of B, limiting reactant is A.
B. 1,8 moles A requires:
1,8 molA×[tex]\frac{4molB}{2molA}[/tex]= 3,6 moles of B
As you have 4 moles of B, limiting reactant is A.
C. 3 moles A requires:
3 molA×[tex]\frac{4molB}{2molA}[/tex]= 6 moles of B
As you have just 4 moles of B, limiting reactant is B.
D. 22 moles A requires:
22 molA×[tex]\frac{4molB}{2molA}[/tex]= 44moles of B
As you have just 40 moles of B, limiting reactant is B.
I hope it helps!
For each scenario, the limiting reactant is determined by comparing the moles used according to the stoichiometry of the reaction. In Parts A, B, and D, A is the limiting reactant; in Part C, B is limiting.
To determine the limiting reactant, compare the moles of each reactant to the stoichiometric coefficients in the balanced equation (2A + 4B → 3C).
1. Part A (2 mol A; 5 mol B):
- Moles of A used = 2 (coefficient in front of A)
- Moles of B used = [tex]\frac{5}{2}[/tex] (coefficient in front of B divided by 2)
- Since Moles of B used > Moles of A used, A is the limiting reactant.
2. Part B (1.8 mol A; 4 mol B):
- Moles of A used = 1.8 (coefficient in front of A)
- Moles of B used = [tex]\frac{4}{4}[/tex] (coefficient in front of B divided by 4)
- Since Moles of A used < Moles of B used, A is the limiting reactant.
3. Part C (3 mol A; 4 mol B):
- Moles of A used = 3 (coefficient in front of A)
- Moles of B used = [tex]\frac{4}{2}[/tex] (coefficient in front of B divided by 2)
- Since Moles of B used < Moles of A used, B is the limiting reactant.
4. Part D (22 mol A; 40 mol B):
- [tex]\( \text{Moles of A used} = \frac{22}{2} \)[/tex] (coefficient in front of A divided by 2)
- Moles of B used = 40 (coefficient in front of B)
- Since Moles of A used < Moles of B used, A is the limiting reactant.
In summary:
- Part A: Limiting reactant is A.
- Part B: Limiting reactant is A.
- Part C: Limiting reactant is B.
- Part D: Limiting reactant is A.
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What is/are the product(s) of a neutralization reaction of a carboxylic acid? View Available Hint(s) What is/are the product(s) of a neutralization reaction of a carboxylic acid? a neutral compound and water a carboxylate salt and water a carboxylate salt a base and water g
Answer:
A carboxylate salt and water
Explanation:
A carboxylic acid is an organic compound that has general formula RCOOH, where R is a carbon chain. Because it's an acid, the neutralization will happen when it reacts with a base, such as NaOH.
When this reaction occurs, the base will dissociate in Na⁺ and OH⁻, and the acid will ionize in RCOO⁻ and H⁺, so the products will be RCOO⁻Na⁺ (a carboxylate salt) and H₂O (water).
Using a 300 MHz NMR instrument:
a. How many Hz downfield from TMS is a signal at 2.5 ppm?
b. If a signal comes at 1200 Hz downfield from TMS, at what ppm does it occur?
c. If two peaks are separated by 2 ppm, how many I-AZ does this correspond to?
Answer:
a. 750Hz, b. 4.0ppm, c. 600Hz
Explanation:
The Downfield Shift (Hz) is given by the formula
Downfield Shift (Hz) = Chemical Shift (ppm) x Spectrometer Frequency (Hz)
Using the above formula we can solve all three parts easily
a. fspec = 300 MHz, Chem. Shift = 2.5ppm, 1MHz = 10⁶ Hz, 1ppm (parts per million) = 10⁻⁶
Downfield Shift (Hz) = 2.5ppm x 300MHz x (1Hz/10⁶MHz) x (10⁻⁶/1ppm)
Downfield Shift = 750 Hz
The signal is at 750Hz Downfield from TMS
b. Downfield Shift = 1200 Hz, Chemical Shift = ?
Chemical Shift = Downfield shift/Spectrometer Frequency
Chemical Shift = (1200Hz/300MHz) x (1ppm/10⁻⁶) = 4.0 ppm
The signal comes at 4.0 ppm
c. Separation of 2ppm, Downfield Shift = ?
Downfield Shift (Hz) = 2(ppm) x 300 (MHz) x (1Hz/10⁶MHz) x (10⁻⁶/1ppm) = 600 Hz
The two peaks are separated by 600Hz
Two solutions, initially at 24.60 °C, are mixed in a coffee cup calorimeter (Ccal = 15.5 J/°C). When a 100.0 mL volume of 0.100 M AgNO3 solution is mixed with a 100.0 mL sample of 0.200 M NaCl solution, the temperature in the calorimeter rises to 25.30 °C. Determine the ∆H°rxn in kJ/mol AgCl for the reaction as written below. The density of the final solution is 1.00 g/mL and heat capacity of the final solution is 4.18 J/goC.
Answer:
∆H°rxn in kJ/mol AgCl = - 59.61 kJ/mol
Explanation:
To solve this question we need to calculate the heat absorbed by the cup calorimeter and by the water in the solutions. We will also need to calculate the amount in moles produced by the reaction since we want to know the ∆H°rxn in kJ/mol AgCl .
mol AgNO₃ = 100 mL x 1L/1000 mL x 0.100 mol/L = 0.01 mol
mol NaCl = 100 mL x 1L/1000 mL x 0.200 mol/L = 0.02 mol
Therefore our limiting reagent is the 0.01 mol AgNO₃ and 0.01 mol AgCl will be produced according to the stoichiometry of the reaction:
AgNO₃ + NaCl ⇒ AgCl + NaNO₃
Heat absorbed by the water:
qw = m(H₂O) x c x ΔT where m (H₂O) = 200 g ( the density of final solution is 1 g/ml)
c = specific heat of water = 4.18 J/gºC
ΔT = change in temperature = (25.30 - 24.60 ) ºC = 0.7ºC
qw = 200 g x 4.18 J/gºC x 0.7 ºC = 585.20 J
Heat Absorbed by the calorimeter :
q cal = C cal x ΔT = 15.5 J/ºC x 0.7ºC = 10.85 J
Total Heat released by the combustion = qw + qcal = 585.20 J +10.85 J
= 596.05 J
We have to change the sign to this quantity since it is an exotermic reaction ( ΔT is positive ) and have the ∆Hrxn
∆H rxn = -596.05 J
but this is not what we are being asked since this heat was released by the formation of 0.0100 mol of AgCl so finally
∆H°rxn = -596.05 J /0.01 mol = -59,605 J/mol x 1 kJ/1000J = -59.61 kJ/mol
The four sets of lines in the hydrogen emission spectrum are known as Balmer, Brackett, Paschen, and Lyman. For each series, assign the energy (infrared, ultraviolet, or visible), the nr value, and all possible n, values up to 7 Series Balmer Brackett Paschen Lyman Energy nf ni visible) infrared ultraviolet 1 2 3 6 7
Answer:
Hydrogen spectrum
Explanation:
Balmer series - Observed in the visible region
Brackett series - Observed in the infrared region
Paschen series - Observed in the infrared region
Lyman series - Observe in the Ultraviolet region.
There are four sets of lines seen in the hydrogen emission spectra are Lyman series in the UV region, Balmer in the visible region and bracket and paschen in the IR region.
What is emission spectra?Emission spectrum is set of radiations emitted by an atom in the order of increasing frequency or decreasing wavelengths. Electrons in atoms transit between various energy levels.
Electrons excites from the lower energy level to the higher energy level by the absorption of light and return back to the ground state by emitting a complementary light.
The lyman series in the hydrogen emission spectrum is starting from the energy level n= 1. It is seen in the UV-region. Balmer series is found in visible region and their n value starts from n = 2.
Similarly Bracket starts from n= 3 and paschen series starts from n= 4. Both are overlapping lines together and they are seen in IR region.
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When the following oxidation–reduction reaction in acidic solution is balanced, what is the lowest whole-number coefficient for H2O, and on which side of the balanced equation should it appear?
MnO4–(aq)+Br–(aq)→Mn2+(aq)+Br2(l)
Select one:
a. 1, reactant side
b. 2, product side
c. 8, product side
d. 16, reactant side
e. 4, product side
Answer:
c. 8, product side
Explanation:
In order to balance a redox reaction we use the ion-electron method, which has the following steps:
Step 1: identify oxidation and reduction half-reaction.
Oxidation: MnO₄⁻(aq) → Mn²⁺(aq)
Reduction: Br⁻(aq) → Br₂(l)
Step 2: perform the mass balance adding H⁺ and H₂O where necessary
8 H⁺(aq) + MnO₄⁻(aq) → Mn²⁺(aq) + 4 H₂O(l)
2 Br⁻(aq) → Br₂(l)
Step 3: perform the electrical balance adding electrons where necessary.
8 H⁺(aq) + MnO₄⁻(aq) + 5 e⁻ → Mn²⁺(aq) + 4 H₂O(l)
2 Br⁻(aq) → Br₂(l) + 2 e⁻
Step 4: multiply both half-reactions by numbers that secure that the number of electrons gained and lost are the same.
2 × (8 H⁺(aq) + MnO₄⁻(aq) + 5 e⁻ → Mn²⁺(aq) + 4 H₂O(l))
5 × (2 Br⁻(aq) → Br₂(l) + 2 e⁻)
Step 5: add both half-reactions side to side.
16 H⁺(aq) + 2 MnO₄⁻(aq) + 10 e⁻ + 10 Br⁻(aq) → 2 Mn²⁺(aq) + 8 H₂O(l) + 5 Br₂(l) + 10 e⁻
16 H⁺(aq) + 2 MnO₄⁻(aq) + 10 Br⁻(aq) → 2 Mn²⁺(aq) + 8 H₂O(l) + 5 Br₂(l)
Calculate the percentage by mass of water in magnesium sulfate heptahydrate, MgSO4•7H2O
Enter your answer with 3 significant figures
Answer:
The percentage by mass of water in magnesium sulfate heptahydrate is 51.2 %
Explanation:
Step 1: Data given
Molar mass of MgSO4*7H2O = 246.5 g/mol
Molar mass of H2O = 18.02 g/mol
Molar massof MgSO4 = 120.37 g/mol
Step 2: Calculate % water in magnesium sulfate heptahydrate
Since we have 7 molecules of water in the heptahydrate, we will divide the molar mass of 7 molecules water by the molar mass of the heptahydrate.
m%(H2O) = (7*18.02)/ 246.5
m%(H2O) = (126.14 /246.5)*100%
m%(H2O) = 51.2 %
To controle this we will calculate the mass % of MgSO4
m%(MgSO4) = (120.37/ 246.50)*100%
m%(MgSO4) = 48.8%
51.2 + 48.8 = 100%
The percentage by mass of water in magnesium sulfate heptahydrate is 51.2 %
Answer:from reffered dfn of %by mass
%by M=mass of component particular/total mass
But mass directly proportional to Molar mass
% by M=molar mass of H2O cpn/total M
%by M=7((1×2)+16)/(7((1×2)+16)+(24+(16×4)+32))
=0.573
Metals with ________ electron configurations characteristically form diamagnetic, square planar complexes.
a. d6
b. d8
c. d10
d. d0
e. d9
Answer:
B
Explanation:
Diamagnetism , paramagnetism and ferromagnetism are terms which are used to describe the magnetic activity of transition metals. These terms helps to know the response the metal will have when placed in a magnetic field. These activities can be discerned from the d-block electronic configuration. If the number of electrons are even, this means they all form a pair and the metal is diamagnetic. If otherwise, there is an unpaired electron which causes the paramagnetic activity of the metal in magnetic field.
To the question, options A-D are diamagnetic but configurations with d8 are the ones that form square planar complexes
Write a balanced chemical equation describing the oxidation of Cl2 gas by Cu3+ to form chlorate ion (ClO3-) and Cu2+ in an acidic aqueous solution. Use the smallest whole-number coefficients possible and indicate states of matter in your balanced reaction.
The detailed answer provides the balanced chemical equation for the oxidation of Cl2 by Cu3+ in an acidic solution, with states of matter indicated.
The balanced chemical equation describing the oxidation of Cl2 gas by Cu3+ to form chlorate ion (ClO3-) and Cu2+ in an acidic aqueous solution is:
3Cu^3+(aq) + 6Cl¯(aq) + 18H^+(aq) + Cl2(g) → 3Cu^2+(aq) + ClO3^-(aq) + 9H2O(l)
States of matter: (s) solid, (l) liquid, (g) gas, (aq) aqueous solution.
The oxidation of [tex]Cl_2[/tex] gas by [tex]Cu^{3+}[/tex] to form chlorate ion and [tex]Cu^{2+}[/tex] in an acidic aqueous solution is represented by the balanced chemical equation provided.
The given question concerns the concept of balancing chemical equations in chemistry and deriving correct chemical reactions for the mentioned reactants and products. Also, oxidation is mentioned which refers to addition of oxygen to an entity or removal of hydrogen from entity. The balanced chemical equation for the oxidation of [tex]Cl_2[/tex] gas by [tex]Cu^{3+}[/tex] in an acidic aqueous solution is:
[tex]2Cl_2(g) + 2Cu^{3+} (aq) + 4H^+ (aq) \rightarrow 2ClO^{3-} (aq) + 2Cu^{2+} (aq) + 2H_2O (l)[/tex]
This reaction results in the formation of chlorate ion ([tex]ClO^{3-}[/tex]) and [tex]Cu^{2+}[/tex] in the solution. The states of matter as gas, aqueous, and liquid are indicated in the equation.
Identify the group of elements that corresponds to each of the following generalized electron configurations and indicate the number of unpaired electrons for each: (a) [Noble gas] ns^2 np^5 (b) [noble gas] ns^2 (n-1)d^2 (c) [noble gas] ns^2 (n-1)d^10 np^1 (d)[noble gas] ns^2 (n-2)f^6
Answer:
(a) [Noble gas] ns² np⁵: Number of unpaired electron is 1 and belongs to group 17 i.e. halogen group of the periodic table.
(b) [noble gas] ns² (n-1)d²: Number of unpaired electron is 2 and belongs to group 4 of the periodic table.
(c) [noble gas] ns² (n-1)d¹⁰ np¹: Number of unpaired electron is 1 and belongs to group 13 of the periodic table.
(d)[noble gas] ns² (n-2)f⁶ : Number of unpaired electron is 6 and belongs to group 8 of the periodic table.
Explanation:
In the Periodic table, the chemical elements are arranged in 7 rows, called periods and 18 columns, called groups. They are organized in increasing order of atomic numbers.
(a) [Noble gas] ns² np⁵
As the total number of electrons in the p-orbital is 5. Therefore, the number of unpaired electron is 1.
This element has 2 electrons in ns orbital and 5 electrons in np orbital. So there are 7 valence electrons.
Therefore, this element belongs to the group 17 i.e. halogen group of the periodic table.
(b) [noble gas] ns² (n-1)d²
As the total number of electrons in the d-orbital is 2. Therefore, the number of unpaired electrons is 2.
This element has 2 electrons in ns orbital and 2 electrons in (n-1)d orbital. So there are 4 valence electrons.
Therefore, this element belongs to the group 4 of the periodic table.
(c) [noble gas] ns² (n-1)d¹⁰ np¹
As the total number of electrons in the p-orbital is 1. Therefore, the number of unpaired electron is 1.
This element has 2 electrons in ns orbital and 1 electron in np orbital. So there are 3 valence electrons.
Therefore, this element belongs to the group 13 of the periodic table.
(d)[noble gas] ns² (n-2)f⁶
As the total number of electrons in the f-orbital is 6. Therefore, the number of unpaired electron is 6.
This element has 2 electrons in ns orbital and 6 electrons in (n-2)f orbital. So there are 8 valence electrons.
Therefore, this element belongs to the group 8 of the periodic table.
The group of elements that corresponds to each of the following are:
(a) [Noble gas] ns² np⁵: Number of unpaired electron is 1 and belongs to group 17.
(b) [noble gas] ns² (n-1)d²: Number of unpaired electron is 2 and belongs to group 4.
(c) [noble gas] ns² (n-1)d¹⁰ np¹:Number of unpaired electron is 1 and belongs to group 13.
(d) [noble gas] ns² (n-2)f⁶ : Number of unpaired electron is 6 and belongs to group 8.
Periodic Table:Periods are horizontal rows (across) the periodic table, while groups are vertical columns (down) the table. The elements are arranged in increasing order of their atomic number.
Group 17 is known as Halogen group, it has only on unpaired electron that means it needs one electron more to complete its octet or attain noble gas configuration. Group 4 is the second group of transition metals in the periodic table. Group 13, is also known as Boron group and it lies in p block elements. Group 8, is also known as Iron family.
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GenAlex Medical, a leading manufacturer of medical laboratory equipment, is designing a new automated system that can detect therapeutic levels of dissolved acetaminophen (10. to 30./μgmL), using a blood sample that is as small as 2.0mL. Calculate the minimum mass in milligrams of acetaminophen that the new system must be able to detect. Round your answer to 2 significant digits.
Answer:
The minimum mass of acetaminophen that the new system must be able to detect is 0.02 milligrams.
Explanation:
Range of the equipment to detect acetaminophen in blood = 10.0 to 30.0 μg/mL
Minimum amount of acetaminophen that can be detected= 10.0 μg/mL
Volume of blood sample = 2 mL
Amount of acetaminophen in 2 ml sample of blood =
[tex]2 mL\times 10.0 \mu g/mL=20.0 \mu g[/tex]
20.0 μg = 0.02 mg (1 μg = 0.001 mg)
The minimum mass of acetaminophen that the new system must be able to detect is 0.02 milligrams.
Gaseous methane (CH4) reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide (CO2) and gaseous water (H20). What is the theoretical yield of carbon dioxide formed from the reaction of 1.28 g of methane and 10.1 g of oxygen gas? Be sure your answer has the correct number of significant digits in it. 02
Answer:
Theoretical yield = 3.51 g
Explanation:
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
For [tex]CH_4[/tex] :-
Mass of [tex]CH_4[/tex] = 1.28 g
Molar mass of [tex]CH_4[/tex] = 16.04 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus,
[tex]Moles= \frac{1.28\ g}{16.04\ g/mol}[/tex]
[tex]Moles_{CH_4}= 0.0798\ mol[/tex]
For [tex]O_2[/tex] :-
Mass of [tex]O_2[/tex] = 10.1 g
Molar mass of [tex]O_2[/tex] = 31.998 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus,
[tex]Moles= \frac{10.1\ g}{31.998\ g/mol}[/tex]
[tex]Moles_{O_2}= 0.3156\ mol[/tex]
According to the given reaction:
[tex]CH_4+2O_2\rightarrow CO_2+2H_2O[/tex]
1 mole of methane gas reacts with 2 moles of oxygen gas
0.0798 mole of methane gas reacts with 2*0.0798 moles of oxygen gas
Moles of oxygen gas = 0.1596 moles
Available moles of oxygen gas = 0.3156 moles
Limiting reagent is the one which is present in small amount. Thus, [tex]CH_4[/tex] is limiting reagent.
The formation of the product is governed by the limiting reagent. So,
1 mole of methane gas on reaction produces 1 mole of carbon dioxide.
0.0798 mole of methane gas on reaction produces 0.0798 mole of carbon dioxide.
Mole of carbon dioxide = 0.0798 mole
Molar mass of carbon dioxide = 44.01 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus,
[tex]0.0798\ moles= \frac{Mass}{44.01\ g/mol}[/tex]
Mass of [tex]CO_2[/tex] = 3.51 g
Theoretical yield = 3.51 g
The theoretical yield of carbon dioxide formed from the reaction of 1.28 g of methane and 10.1 g of oxygen gas is 3.51 g.
The balanced equation for the reaction between methane (CH4) and oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O) is:
CH4 + 2O2 → CO2 + 2H2O
To find the theoretical yield of carbon dioxide, we need to calculate the moles of methane and oxygen and use the stoichiometry of the balanced equation.
Given: Mass of methane (CH4) = 1.28 g
Mass of oxygen gas (O2) = 10.1 g
Step 1: Calculate the moles of methane and oxygen using their molar masses:
Moles of CH4 = mass / molar mass = 1.28 g / 16.04 g/mol = 0.0798 mol
Moles of O2 = mass / molar mass = 10.1 g / 32.00 g/mol = 0.3156 mol
Step 2: Determine the limiting reactant (the reactant that is completely consumed first) by comparing the mole ratios of CH4 and O2 in the balanced equation. From the equation, for every 1 mol of CH4 there are 2 moles of O2 needed. Therefore, the mole ratio of CH4 to O2 is 1:2.
Since the mole ratio of CH4 to O2 is 1:2, and there are fewer moles of CH4 (0.0798 mol) compared to the moles of O2 (0.3156 mol), CH4 is the limiting reactant.
Step 3: Calculate the moles of CO2 produced using the mole ratio from the balanced equation:
Moles of CO2 = moles of CH4 x (1 mol of CO2 / 1 mol of CH4) = 0.0798 mol x (1 mol / 1 mol) = 0.0798 mol
Step 4: Convert the moles of CO2 to grams using the molar mass of CO2:
Mass of CO2 = moles x molar mass = 0.0798 mol x 44.01 g/mol = 3.51 g
Therefore, the theoretical yield of carbon dioxide formed from the reaction of 1.28 g of methane and 10.1 g of oxygen gas is 3.51 g (to the correct number of significant digits).
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Calculate the change internal energy (ΔE) for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings. Calculate the change internal energy (ΔE) for a system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings. 9.00 x 102 kJ 64.1 kJ -9.00 x 102 kJ -64.1 kJ -65.9 kJ
A system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings has a change in the internal energy of -65.9 kJ.
The system is giving off 65.0 kJ of heat (Q). By convention, when a system is releasing heat, Q < 0. Then, Q = -65.0 kJ.The system is also performing 855 J of work (W) on the surroundings. By convention, when a system performs work on the surroundings, W < 0. Then, W = -855 J (-0.855 kJ)According to the First Law of Thermodynamics, we can calculate the change in the internal energy (ΔE) of the system using the following expression.
[tex]\Delta E = Q + W = (-65.0 kJ) + (-0.855 kJ) = -65.9 kJ[/tex]
A system that is giving off 65.0 kJ of heat and is performing 855 J of work on the surroundings has a change in the internal energy of -65.9 kJ.
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100 POINTS!!! WILL MARK BRAINIEST!!! What is the maximum number of grams of SO2 that can be fromed when 10.0 g of H2S reacts with 8.5 of oxygen? Given the equation 2H2S + 3O2 --> 2SO2 + 2H2O. PLS SHOW WORK!!
Answer:
Mass = 12.82 g
Explanation:
Given data:
Mass of oxygen = 8.5 g
Mass of H₂S = 10.0 g
Mass of SO₂ = ?
Solution:
Chemical equation;
2H₂S + 3O₂ → 2SO₂ + 2H₂O
Number of moles of H₂S:
Number of moles = mass/ molar mass
Number of moles = 10.0 g / 34 g/mol
Number of moles =0.3 mol
Number of moles of oxygen:
Number of moles = mass/ molar mass
Number of moles = 8.5 g / 32 g/mol
Number of moles = 0.3 mol
Now we will compare the moles of SO2 with oxygen and hydrogen sulfide.
O₂ : SO₂
3 : 2
0.3 : 2/3×0.3=0.2 mol
H₂S : SO₂
2 : 2
0.3 : 0.3
The number of moles of SO₂ produced by oxygen are less so it will limiting reactant.
Mass of SO₂:
Mass = number of moles × molar mass
Mass = 0.2 mol × 64.1 g/mol
Mass = 12.82 g
Chemistry: An oxygen gas container has a volume of 20.0 L. How many grams of oxygen are in the container, if the gas has a pressure of the 845mmHg at 22degrees Celsius?
Answer:
There are 29.4 grams of oxygen in the container
Explanation:
Step 1: Data given
Volume = 20.0 L
Pressure = 845 mmHg
Temperature = 22.0 °C
Molar mass of O2 = 32 g/mol
Step 2: Ideal gas law
p*V = n*R*T
⇒ p = the pressure of the gas = 845 mmHg = 1.11184
⇒ V = the volume of the gas = 20.0 L
⇒ n = the number of moles = TO BE DETERMINED
⇒R = the gasconstant = 0.08206 L*atm/K*mol
⇒ T = the temperature = 22°C + 273 = 295 Kelvin
n = (p*V)/(R*T)
n = (1.11184*20.0)/(0.08206*295)
n = 0.9186 moles
Step 3: Calculate mass of NO2
Mass of O2 = Moles O2 * Molar mass O2
Mass of O2 = 0.9186 moles * 32 g/mol
Mass of O2 = 29.4 grams
There are 29.4 grams of oxygen in the container
What is the value for the reaction: N2(g) + 2 O2(g) --> N2O4(g) in terms of K values from the reactions:
½ N2(g) + ½ O2(g) ---> NO(g)
K1
2 NO(g) + O2(g) ---> N2O4(g)
K2
K1^2 + K2
2 K1 x K2
K1^2 x K2
K1 + K2
Answer : The correct expression will be:
[tex]K=(K_1)^2\times K_2[/tex]
Explanation :
The chemical reactions are :
(1) [tex]\frac{1}{2}N_2(g)+\frac{1}{2}O_2(g)\rightleftharpoons NO(g)[/tex] [tex]K_1[/tex]
(2) [tex]2NO(g)+O_2(g)\rightleftharpoons N_2O_4(g)[/tex] [tex]K_2[/tex]
The final chemical reaction is :
[tex]N_2(g)+2O_2(g)\rightleftharpoons N_2O_4[/tex] [tex]K=?[/tex]
Now we have to calculate the value of [tex]K[/tex] for the final reaction.
Now equation 1 is multiply by 2 and then add both the reaction we get the value of 'K'.
If the equation is multiplied by a factor of '2', the equilibrium constant will be the square of the equilibrium constant of initial reaction.
If the two equations are added then equilibrium constant will be multiplied.
Thus, the value of 'K' will be:
[tex]K=(K_1)^2\times K_2[/tex]
The change in entropy, Δ S ∘ rxn , is related to the the change in the number of moles of gas molecules, Δ n gas . Determine the change in the moles of gas for each of the reactions and decide if the entropy increases, decreases, or has little or no change. A. 2 H 2 ( g ) + O 2 ( g ) ⟶ 2 H 2 O ( l )
Answer:
The entropy decreases.
Explanation:
The change in the standard entropy of a reaction (ΔS°rxn) is related to the change in the number of gaseous moles (Δngas), where
Δngas = n(gaseous products) - n(gaseous reactants)
If Δngas > 0, the entropy increasesIf Δngas < 0, the entropy decreases.If Δngas = 0, there is little or no change in the entropy.Let's consider the following reaction.
2 H₂(g) + O₂(g) ⟶ 2 H₂O(l)
Δngas = 0 - 3 = -3, so the entropy decreases.
An unknown quantity of sugar was completely dissolved in water at 75 degrees Celsius to form a clear and colorless solution. The temperature of the solution was then lowered to 25 degrees Celsius while being mixed.
Question 1: Was the solution at 75 degrees Celsius saturated, unsaturated or supersaturated?
Question 2: Explain your reason for choosing the answer in question 1.
Answer:
67
Explanation:
Question 1: The solution at 75 degrees Celsius was likely saturated.
Question 2: The reason for choosing "saturated" is that the sugar was completely dissolved in water at 75 degrees Celsius, forming a clear and colorless solution.
What happens in such solutionsIn a saturated solution, the maximum amount of solute (sugar, in this case) that can dissolve at that temperature has already dissolved. When the solution is clear and colorless at that temperature, it suggests that the solution contains as much sugar as it can hold under those conditions.
If it were unsaturated, there would still be room for more sugar to dissolve, and if it were supersaturated, it would become unstable and potentially precipitate out excess solute when the temperature was lowered.
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A piston system absorbs 50.5 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.491 atm. The final volume of the system is 56.2 L. What was the initial volume of the system if the internal energy of the system decreased by 106.0 J? (To convert between L∙atm and J, use 1 L∙atm = 101.3 J.)
Answer:
The initial volume of the system: V₁ = 53.06 L
Explanation:
Given: heat absorbed by system: q = 50.5 J, Pressure: P = 0.491 atm, Final volume: V₂ = 56.2 L, The change in the internal energy: ΔE = -106.0 J
Initial volume: V₁ = ? L
According to the First Law of Thermodynamics:
ΔE = q - PΔV
⇒ PΔV = q - ΔE = 50.5 J - (-106.0 J) = 156.5 J
As, 1 L∙atm = 101.3 J ⇒ 1 J = (1 ÷ 101.3) L∙atm
⇒ PΔV = 156.5 J = (156.5 ÷ 101.3) L∙atm = 1.54 L∙atm
So,
ΔV = 1.54 L∙atm ÷ P = 1.54 L∙atm ÷ 0.491 atm = 3.14 L
∵ ΔV = V₂ - V₁ = 3.14 L
⇒ V₁ = V₂ - 3.14 L = 56.2 L - 3.14 L = 53.06 L
Therefore, the initial volume of the system: V₁ = 53.06 L
In Ontario, some electricity comes from coal-burning generators. Coal is a natural form of carbon that has a large amount of sulphur mixed in with it. Answer the following questions based on the burning of coal to produce energy.
a) Write the word equations and balanced chemical equations for the burning of carbon and the burning of sulphur. (4 marks)
b) Which of these products is harmful to the environment? How is it harmful? (2 marks)
c) Write the word equation and balanced chemical equation for the reaction that produces this harmful environmental effect. (2 marks)
d)Explain why it is important to make sure your furnace is tuned up and in proper working order before the winter
Answer:
a)
[tex]C(s)+O_{2}(g) \rightarrow CO_{2}(g)[/tex]
[tex]S(s)+O_{2}(g) \rightarrow SO_{2}(g)[/tex]
b)
Sulphurdioxide
c)
[tex]SO_{2}(g) + H_{2}O(l) \rightarrow H_{2}SO_{3}(l)[/tex]
[tex]SO_{2}(g) + \frac{1}{2}O_{2} \rightarrow SO_{3}(g)[/tex]
d)
Incomplete combustion produce harmful gases.
Explanation:
a)
Carbon reacts with atmospheric oxygen to form carbondioxide as well as sulphur dioxide.
The chemical equations are as follows.
[tex]C(s)+O_{2}(g) \rightarrow CO_{2}(g)[/tex]
[tex]S(s)+O_{2}(g) \rightarrow SO_{2}(g)[/tex]
b)
Sulfur dioxide is very harmful to the environment to cause acid rains.
This harmful gas mix with rain water to form sulphuric acid.
c)
The balanced chemical equation for the reaction that produces harmful environmental effects is as follows.
[tex]SO_{2}(g) + H_{2}O(l) \rightarrow H_{2}SO_{3}(l)[/tex]
[tex]SO_{2}(g) + \frac{1}{2}O_{2} \rightarrow SO_{3}(g)[/tex]
[tex]SO_{3}(g) +H_{2}O(l) \rightarrow H_{2}SO_{4}(l)[/tex]
d)
In the absence of proper amount of oxygen required for combustion, incomplete combustion will take place which will result in formation of more carbondioxide an other harmful gases.
how many grams are in 0.5 moles of C10H16?
Please show your work for marked brainliest!
Answer:
68 g
Explanation:
Molar mass (C10H16) = 10*12.0 g/mol + 16*1.0 g/mol = (120+16)g/mol =
= 136 g/mol
m (C10H16) = n(C10H16)*M(C10H16) = 0.5 mol*136 g/mol = 68 g
n(C10H16) - number of moles of C10H16
M(C10H16) - molar mass of C10H16
what is the molarity of the solution formed when 7.88 grams of NaCl is mixed with enough water to make 350. mL of solution?
Answer:
The molarity of the solution is 0.386 M
Explanation:
Step 1: Data given
Mass of NaCl = 7.88 grams
Volume of the solution = 350 mL
Molar mass of NaCl = 58.5 g/mol
Step 2: Calculate number of moles
Number of moles NaCl = mass of NaCl / molar mass of NaCl
Number of moles NaCl = 7.88 grams / 58.5 g/mol
Number of moles = 0.135 moles
Step 3: Calculate molarity of the solution
Molarity = Number of moles NaCl / volume
Molarity = 0.135 moles / 0.350 L
Molarity = 0.386 M
The molarity of the solution is 0.386M
Consider the following data for air trapped in a flask: Pressure = 0.988 atm Room Temperature = 23.5°C Volume of the flask = 1.042 L For this calculation, assume air is 78.5% nitrogen and 21.5% oxygen (by number of moles). R = 0.0821 L•atm•mol-1•K-1 N = 14.01 g/mol O = 16.00 g/mol What is the mass of air in the flask
Answer:
total mass will be = = 1.207g
Explanation:
First what is given
Pressure P= 0.988 atm Room TemperatureT = 23.5°C= 296.5 K
Volume V= 1.042 L
Nitrogen in air is 80 % (moles number) = 0.8
Ideal gas constant R = 0.0821 L atmmol-1K-1
Given mass of N = 14.01 g/mol
Given mass of oxygen O = 16.00 g/mol
Total number of moles = ?
So first we have to find the total number of moles by using formula
Total number of moles
n = PV/ RT
adding the values
moles n= 0.988atm x 1.042L / (0.0821L-atm/mole-K x 296.6K)
= 1.0294 / 24.35
= 0.042 moles (total number of moles)
So by using Nitrogen percentage
Moles of nitrogen = total moles x 80/100
= 0.042moles x 0.8
So moles of O2= Total moles – moles of N2
= 0.042moles - 0.034moles
Moles of O2 = 0.008moles
Now for finding the mass of the N2 and oxygen
Mass of Nitrogen N2 = no of moles x molar mass
= 0.034 x 28
= 0.952 g
Mass of oxygen O2 = no of moles x molar mass
= 0.008 x 32
= 0.256 g
total mass will be = Mass of Nitrogen N2 + Mass of oxygen O2
=0.952 g + 0.256 g
=1.207g
The mass of air in the flask = 1.207g
Given:
Pressure, P= 0.988 atm
Room Temperature, T = 23.5°C= 296.5 K
Volume, V= 1.042 L
Nitrogen in air is 80 % (moles number) = 0.8
Ideal gas constant R = 0.0821 L atm [tex]mol^{-1}K^{-1}[/tex]
Molar mass of N = 14.01 g/mol
Molar mass of oxygen O = 16.00 g/mol
To find:
Total number of moles = ?
Calculation for number of moles:From ideal gas law:
n = PV/ RT
n= 0.988atm * 1.042L / (0.0821 L atm [tex]mol^{-1}K^{-1}[/tex] * 296.6K)
n = 1.0294 / 24.35
n= 0.042 moles
Using mol fraction we will calculate moles for nitrogen and oxygen:
Moles of nitrogen = total moles * 80/100
Moles of nitrogen = 0.042moles * 0.8 = 0.034 moles
So, Moles of O₂ = Total moles – moles of N₂
Moles of O₂ = 0.042 moles - 0.034 moles
Moles of O₂ = 0.008 moles
Calculation for mass:
Mass of Nitrogen N₂ = no of moles x molar mass
= 0.034 x 28
= 0.952 g
Mass of oxygen O₂ = no of moles x molar mass
= 0.008 * 32
= 0.256 g
Total mass will be = Mass of Nitrogen N₂ + Mass of oxygen O₂
=0.952 g + 0.256 g
Total mass = 1.207g
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