Answer:
The ratio of effusion rates for [tex]^{238}UF_6[/tex] and [tex]^{235}UF_6[/tex] is 0.995734.
Explanation:
Effusion rate of the [tex]^{235}UF_6 [/tex]gas = [tex]R[/tex]
Effusion rate of the [tex]^{238}UF_6 [/tex]gas = [tex]r[/tex]
Molar mass of [tex]^{235}UF_6=235.054+6\times 19.00 amu=349.054 amu[/tex]
Molar mass of [tex]^{238}UF_6=238.051+6\times 19.00 amu=352.051 amu[/tex]
Graham's law states that the rate of effusion or diffusion of gas is inversely proportional to the square root of the molar mass of the gas. The equation given by this law follows the equation:
[tex]\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}[/tex]
[tex]\frac{r}{R}=\sqrt{\frac{349.054 amu}{352.051 amu}}=0.995734[/tex]
The ratio of effusion rates for [tex]^{238}UF_6[/tex] and [tex]^{235}UF_6[/tex] is 0.995734.
Final answer:
The ratio of effusion rates for 238UF6 and 235UF6 can be calculated using Graham's law, which states that the ratio of effusion rates is equal to the square root of the ratio of the molar masses of the gases.
Explanation:
The ratio of effusion rates for 238UF6 and 235UF6 can be calculated using Graham's law, which states that the ratio of effusion rates is equal to the square root of the ratio of the molar masses of the gases.
So, the ratio of effusion rates for 238UF6 and 235UF6 is:
(352.04 g/mol) / (349.03 g/mol) = 1.008
This means that the effusion rate of 238UF6 is approximately 1.008 times higher than the effusion rate of 235UF6.
A concentrated binary solution containing mostly species 2 (but x2 ≠ 1) is in equilib- rium with a vapor phase containing both species 1 and 2. The pressure of this two- phase system is 1 bar; the temperature is 25°C. At this temperature, 1 = 200 bar and P2sat = 0.10 bar. Determine good estimates of x1 and y1. State and justify all assumptions.
Answer:
x1= 4.5 × 10^-3, y1= 0.9
Explanation:
A binary solution having two species is in equilibrium in a vapor phase comprising of species 1 and 2
Take the basis as the pressure of the 2 phase system is 1 bar. The assumption are as follows:
1. The vapor phase is ideal at pressure of 1 bar
2. Henry's law apply to dilute solution only.
3. Raoult's law apply to concentrated solution only.
Where,
Henry's constant for species 1 H= 200bar
Saturation vapor pressure of species 2, P2sat= 0.10bar
Temperature = 25°C= 298.15k
Apply Henry's law for species 1
y1P= H1x1...... equation 1
y1= mole fraction of species 1 in vapor phase.
P= Total pressure of the system
x1= mole fraction of species 1 in liquid phase.
Apply Raoult's law for species 2
y2P= P2satx2...... equation 2
From the 2 equations above
P=H1x1 + P2satx2
200bar= H1
0.10= P2sat
1 bar= P
Hence,
P=H1x1 + (1 - x1) P2sat
1bar= 200bar × x1 + (1 - x1) 0.10bar
x1= 4.5 × 10^-3
The mole fraction of species 1 in liquid phase is 4.5 × 10^-3
To get y, substitute x1=4.5 × 10^-3 in equation 1
y × 1 bar = 200bar × 4.5 × 10^-3
y1= 0.9
The mole fraction of species 1 in vapor phase is 0.9
What is Binary solution?
A binary solution having two species is in equilibrium in a vapor phase comprising of species 1 and 2
If we consider the pressure of the 2 phase system is 1 bar.
The assumption are as follows:
The vapor phase is ideal at pressure of 1 bar. Henry's law apply to dilute solution only. Raoult's law apply to concentrated solution only.Where, these values are given:
Henry's constant for species 1 H= 200bar
Temperature = 25°C= 298.15K
P₂sat= 0.10 bar
Apply Henry's law for species 1
y₁P= H₁x₁.......... (i)
where y₁= mole fraction of species 1 in vapor phase, P= Total pressure of the system ,x₁= mole fraction of species 1 in liquid phase.
Apply Raoult's law for species 2
y₂P= P₂sat. x₂...........(ii)
From (i) and (ii)
P=H₁x₁ + P₂sat. x₂
200bar= H₁
0.10= P₂sat
1 bar= P
Hence,
P=H₁x₁ + (1 - x₁) P₂sat
1bar= 200bar × x₁ + (1 - x₁) 0.10bar
x₁= [tex]4.5 * 10^{-3}[/tex]
The mole fraction of species 1 in liquid phase is [tex]4.5 * 10^{-3}[/tex]
To get y, substitute x₁=[tex]4.5 * 10^{-3}[/tex] in (i)
y × 1 bar = 200bar × [tex]4.5 * 10^{-3}[/tex]
y₁= 0.9
The mole fraction of species 1 in vapor phase is 0.9.
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Draw the mechanism of the slow step that occurs in both first-order substitution and first-order elimination reactions for (R)-3-bromo-2,3-dimethylpentane in methanol with heat applied. Provide curved arrows in Box 1 to depict the flow of electrons and draw the intermediate in Box 2.
Answer:
see explaination
Explanation:
We are given the (R)-3-bromo-2,3-dimethylpentane and asking to draw the curved arrow which is the showing the mechanism for first-order substitution and first-order elimination reactions. We know the formation of carbocation is the rate determining step in the first-order substitution and first-order elimination reactions.
So in the (R)-3-bromo-2,3-dimethylpentane there is –Br gets removed and formed the tertiary carbocation which is more stable, so the curved arrows in Box 1 to depict the flow of electrons and intermediate in Box 2.
Check attachment
Analyze and solve this partially completed galvanic cell puzzle. There are 4 electrodes each identified by a letter of the alphabet, A through D. The values in the partially completed grid are measured cell potentials for a cell consisting of electrode #1 and electrode #2. You may assume that each galvanic cell was properly constructed with the appropriate metals and solutions and that all the measured values in the grid are accurate.
electrode #1 ?
C
B
D
A
electrode #2?
Ecell(volts)
Ecell(volts)
Ecell(volts)
Ecell(volts)
C
0
0.91
0.62
0.26
B
0.91
0
1.53
D
0.62
1.53
0
0.36
0 volts
0.10 volts
0.26 volts
0.36 volts
0.55 volts
0.62 volts
0.65 volts
0.88 volts
0.98 volts
1.17 volts
1.27 volts
1.79 volts
1.89 volts
Complete Question
The complete question is shown on the first uploaded image
Answer:
The correct option is [tex]E_{cell}__{AC}} = 0.94[/tex]
Explanation:
From the question we are told that
the cell voltage for AD is [tex]E_{cell}__{AD}} = 1.56V[/tex]
From the data give we can see that
[tex]E_{cell}__{AD}} - E_{cell}__{BD}} = E_{cell}__{AB}}[/tex]
i.e [tex]1.56 - 1.53 = 0.03[/tex]
In the same way we can say that
[tex]E_{cell}__{AD}}-E_{cell}__{CD}} = E_{cell}__{AC}}[/tex]
=> [tex]E_{cell}__{AC}}=1.56- 0.62[/tex]
[tex]E_{cell}__{AC}} = 0.94[/tex]
Galvanic cells are the voltaic cells that generate an electric current from redox reactions. The cell potential of cells A and C will be 0.94 volts.
What are the cell potentials?The cell potential is the estimation of the gained or lost electrons by the species on the electrode of the electrochemical cell.
Given, the cell voltage for cells A and D is 1.56 V.
Cell potential between A and B cells is calculated as:
[tex]\begin{aligned} \rm E_{cell}_{(AB)} &= \rm E_{cell}_{(AD)} - \rm E_{cell}_{(BD)}\\\\&= 1.56 - 1.53\\\\&= 0.03 \end{aligned}[/tex]
Similarly, cell potential between A and C cells is calculated as:
[tex]\begin{aligned} \rm E_{cell}_{(AC)} &= \rm E_{cell}_{(AD)} - \rm E_{cell}_{(CD)}\\\\&= 1.56 - 0.62\\\\&= 0.94 \end{aligned}[/tex]
Therefore, the cell potential between A and C cell is 0.94 volts.
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You mix sodium metal with nitric acid. What salt is produced?
Answer:
By mixing 2 Moles of Sodium Metal with 2 Moles of nitric acid, Sodium Nitrate is formed.
Explanation:
2Na+ + HNO3 produces 2NaNO3 + H2
Hydrogen peroxide can act as either an oxidizing agent or a reducing agent depending on the species present in solution. Write the balanced half-reaction equations for each situation. Write the balanced half-reaction equation for when H2O2(aq) acts as an oxidizing agent in an acidic solution. Phases are optional. half-reaction equation: Write the balanced half-reaction equation for when H2O2(aq) acts as a reducing agent in an acidic solution. Phases are optional. half-reaction equation: A disproportionation reaction is one in which a single species oxidizes and reduces itself. Write the complete balanced equation for the disproportionation reaction of H2O2(aq) . Phases are optional. disproportionation reaction:
Answer:
1) H₂O₂ + 2H⁺ + 2e⁻ → 2H₂O
2) H₂O₂ → 2H⁺ + 2e⁻ O₂
3) 2H₂O₂ → 2H₂O + O₂
Explanation:
Half-reaction equation for when H₂O₂(aq) acts as an oxidizing agent in an acidic solution (this means H₂O₂ is reduced):
H₂O₂ + 2H⁺ + 2e⁻ → 2H₂OIt is a reduction because the oxidation number of O changes from -1 to -2.
Half-reaction equation for when H₂O₂(aq) acts as a reducing agent in an acidic solution (this means H₂O₂ is oxidized):
H₂O₂ → 2H⁺ + 2e⁻ O₂
It is an oxidation because the oxidation number of O changes from -1 to 0.
Disproportionation reaction of H₂O₂(aq):
2H₂O₂ → 2H₂O + O₂
Hydrogen peroxide can act as both an oxidizing and a reducing agent in an acidic solution. It becomes oxidized when acting as a reducing agent and gets reduced when it acts as an oxidizing agent. In a disproportionation reaction, it can both oxidize and reduce itself.
Explanation:Hydrogen peroxide (H2O2) can indeed act as either an oxidizing or reducing agent depending on the species present in solution. When
H2O2
acts as an oxidizing agent in an acidic solution, the balanced half-reaction is:
H2O2 + 2H+ + 2e- → 2H2O
This reaction shows H2O2 being reduced, thus it is acting as an oxidizer because it causes the oxidation of other substances by accepting electrons. In contrast, when
H2O2 acts as a reducing agent in an acidic solution, the balanced half-reaction is:
H2O2 → O2 + 2H+ + 2e-
In this case, H2O2 is being oxidized to O2 so it acts as a reducer because it donates electrons which allows the reduction of other substances.
Finally, in a disproportionation reaction, H2O2 can act as both the oxidizing and reducing agent, showing the same substance functioning as an oxidant and a reductant. The complete balanced equation for this disproportionation reaction of H2O2 is:
2H2O2 → 2H2O + O2
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Consider the reaction: NO2(g) + CO(g) ⇌ NO(g) + CO2(g) Kc = 0.30 at some temperature. If the initial mixture has the concentrations below, the system is_______.
This is an incomplete question, here is a complete question.
Consider the reaction: [tex]NO_2(g)+CO(g)\rightleftharpoons NO(g)+CO_2(g)[/tex]
Kc = 0.30 at some temperature.
If the initial mixture has the concentrations below, the system is_______.
Chemicals Concentration (mol/L)
- NO₂ 0.024
- CO 0.360
- NO 0.180
- CO₂ 0.120
Possible answers:
1) not at equilibrium and will remain in an unequilibrated state.
2) not at equilibrium and will shift to the left to achieve an equilibrium state.
3) not at equilibrium and will shift to the right to achieve an equilibrium state.
4) at equilibrium
Answer : The correct option is, (2) not at equilibrium and will shift to the left to achieve an equilibrium state.
Explanation:
Reaction quotient (Qc) : It is defined as the measurement of the relative amounts of products and reactants present during a reaction at a particular time.
First we have to determine the value of reaction quotient (Qc).
The given balanced chemical reaction is,
[tex]NO_2(g)+CO(g)\rightleftharpoons NO(g)+CO_2(g)[/tex]
The expression for reaction quotient will be :
[tex]Q_c=\frac{[NO][CO_2]}{[NO_2][CO]}[/tex]
In this expression, only gaseous or aqueous states are includes and pure liquid or solid states are omitted.
Now put all the given values in this expression, we get
[tex]Q_c=\frac{(0.180)\times (0.120)}{(0.024)\times (0.360)}=2.5[/tex]
Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.
There are 3 conditions:
When [tex]Q>K[/tex] that means product > reactant. So, the reaction is reactant favored.
When [tex]Q<K[/tex] that means reactant > product. So, the reaction is product favored.
When [tex]Q=K[/tex] that means product = reactant. So, the reaction is in equilibrium.
The given equilibrium constant value is, [tex]K_c=0.30[/tex]
From the above we conclude that, the [tex]Q>K[/tex] that means reactant < product. So, the reaction is reactant favored that means reaction must shift to the reactant or left to be in equilibrium.
Hence, the correct option is, (2) not at equilibrium and will shift to the left to achieve an equilibrium state.
Mark each of the following statements as either True or False: The rate law is deduced directly from the coefficients of the overall reaction. The rate equation for this mechanism is rate = k [O][ClO]. ClO(g) is an intermediate formed in this reaction mechanism. Step 2 of the mechanism is a bimolecular. The sum of the two steps is equal to the overall reaction: O(g) + O3(g) → 2O2(g). Cl(g) is a catalyst in this reaction mechanism.
Answer:
Details of true/false statements are given below.
Explanation:
The rate law is deduced directly from the coefficients of the overall reaction. False
The rate equation for this mechanism is rate = k [O][ClO]. ClO(g) is an intermediate formed in this reaction mechanism. True
Step 2 of the mechanism is a bimolecular. True
The sum of the two steps is equal to the overall reaction: O(g) + O3(g) → 2O2(g). True
Cl(g) is a catalyst in this reaction mechanism. True
Measurements show that the enthalpy of a mixture of gaseous reactants increases by 215. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -155. kJ of work is done on the mixture during the reaction.Calculate the change in energy of the gas mixture during the reaction. Round your answer to 2 significant digits.Is the reaction exothermic or endothermic?
Answer: The change in energy of the gas mixture during the reaction is 60 kJ. The reaction is endothermic.
Explanation:
According to first law of thermodynamics:
[tex]\Delta E=q+w[/tex]
[tex]\Delta E[/tex]=Change in internal energy
q = heat absorbed or released
w = work done or by the system
w = work done on the system
w = -155 kJ
q = +215kJ {Heat absorbed by the system is positive}
[tex]\Delta E=+215+(-155)kJ=60kJ[/tex]
As the heat is absorbed and enthalpy increases, the reaction is endothermic.
uestion 174 Which sequence of reactions is expected to produce the product below as the final, and major, organic product? I 1. HC≡CH, NaNH2; 2. (CH3)2CHCH2Br 3. Aqueous H2SO4, HgSO4 II 1. CH3C≡CH, NaNH2; 2. (CH3)2CHBr; 3. Disisamylborane; 4. H2O2, NaOH III 1. (CH3)2CHBr, NaNH2; 2. CH3C≡CH; 3. O3; 4. H2O IV 1. CH3C≡CH, NaNH2: 2. (CH3)2CHCH2Br; 3. BH3·THF; 4. H2O2, NaOH V 1. (CH3)2CHCH2Br, NaNH2; 2. HC≡CH; 3. 9-BBN; 4. H2O2, NaOH I II III IV V
Complete Question
The complete question is shown on the first uploaded image
Answer:
The correction option is is [tex]I[/tex]
Explanation:
The mechanism of the reaction is show on the second uploaded image
The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic interaction between the ions and thus the strength of the lattice energy of the ionic compound. Arrange the compounds according to the magnitudes of their lattice energies based on the relative ion charges and sizes.- MgS
- NaCl
- MgCl_2
- KBr
The charges and sizes of ions in an ionic compound determine the strength of its lattice energy.
Explanation:The strength of the lattice energy in an ionic compound is determined by the charges and sizes of the ions. The larger the charges and the smaller the ion sizes, the stronger the electrostatic interaction and the higher the lattice energy. Based on this, the compounds can be arranged in order of their magnitudes of lattice energies:
MgSKBrNaClMgCl2MgS has the highest lattice energy because of the high charge and small size of both the Mg2+ and S2- ions.
So the order of lattice energies would be: MgS > MgCl_2 > NaCl > KBr
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: If a 250. mL sample of the above buffer solution initially has 0.0800 mol H2C6H5O7 - and 0.0600 mol HC6H5O7 2- , what would be the new concentration of HC6H5O7 2- after 25.0 mL of 0.125 M NaOH is added to the buffer?
Answer: New concentration of [tex]HC_{6}H_{5}O^{2-}_{7}[/tex] is 0.23 M.
Explanation:
The given data is as follows.
Moles of [tex]HC_{6}H_{5}O^{2-}_{7}[/tex] = 0.06 mol
Moles of [tex]H_{2}C_{6}H_{5}O_{7}[/tex] = 0.08 mol
Therefore, moles of [tex]OH^{-}[/tex] added are as follows.
Moles of [tex]OH^{-}[/tex] = [tex]0.125 \times \frac{25}{1000}[/tex]
= 0.003125 mol
Now, new moles of [tex]HC_{6}H_{5}O^{2-}_{7}[/tex] = 0.06 + 0.003125
= 0.063125
Therefore, new concentration of [tex]HC_{6}H_{5}O^{2-}_{7}[/tex] will be calculated as follows.
Concentration = [tex]\frac{0.063125}{0.275}[/tex]
= 0.23 M
Thus, we can conclude that new concentration of [tex]HC_{6}H_{5}O^{2-}_{7}[/tex] is 0.23 M.
The absorbance features observed in the visible spectrum for curcumin is a result of an allowed optical excitation of an electron from the π-HOMO to the π*-LUMO. What is the energy change for this electronic excitation based on the spectrum? (Hint: Energy and wavelength are related by the equation E = hc/λ.) h = 4.136 × 10-15 eV⋅ s c = 2.998 × 108 m/s
Answer:
2.3 ev or 3.68 ×10^-19J
Explanation:
The spectrum is shown in the image attached
h= 4.136 × 10-15 eV⋅ s
c = 2.998 × 108 m/s
λmax= 550×10^-9 (from the spectrum attached)
E=hc/λmax
E= 4.136 × 10^-15 × 2.998 × 10^8/550×10^-9
E= 2.3 ev or 3.68 ×10^-19J
The energy change for the electronic excitation is : 3.68 * 10⁻¹⁹J
Given data :
h = 4.136 * 10⁻¹⁵ eV⋅ s
c = 2.998 * 108 m/s
λmax = 550 * 10⁻⁹ ( Obtained from image attached below )
Applying the energy and wavelength relationship equation
E = hc / λmax
= ( 4.136 * 10⁻¹⁵ * 2.998 * 108 ) / 550 * 10⁻⁹
= 2.3 ev ≈ 3.68 * 10⁻¹⁹J.
Hence we can conclude that the energy change for the electronic excitation is 2.3 ev ≈ 3.68 * 10⁻¹⁹J.
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Missing data related to your question is attached below
Question 3After creating a Beer's Law plot using standard solutions of Q, you determined the slope of Beer's Law to be 0.515 M-1. Your unknown solution of Q tested in Part B of the experiment had an absorbance of 0.145. Determine the concentration (in molarity) of the unknown solution Q from Part B.Question 4Refer to the procedure stated in the manual pages for Part A to answer the following question.Using the equation editor embedded in this question, show a sample calculation determining the original concentration of the provided unknown Q in Part A from the diluted concentration calculated in question 3 above.Lab ManualYou have been provided with a solution of unknown Q, the actual molar concentration is listed as the unknown number. Dilute 15.00 mL of the provided solution to a final volume of 50.00 mL. You may only use the equipment and reagents listed above. Be sure to record your unknown number in your notebook. After making your dilution, calculate the concentration of your diluted solution.
The concentration of the unknown solution 'Q' from Part B is determined to be 0.282 M using Beer's Law. The original concentration of the unknown 'Q' from Part A, before dilution, is calculated to be 0.94 M.
Explanation:The concentration of the unknown solution Q can be determined using the Beer's Law plot. Beer's Law or the Beer-Lambert law connects the absorbance of a solution to its concentration through the following equation: A = εcl, where 'A' is the absorbance, 'ε' is the molar absorptivity, 'c' is the concentration and 'l' is the path length. The slope of the Beer's Law plot corresponds to the product, 'εl'. So, the concentration can be calculated as: c=A/(εl), which gives c= 0.145/0.515 M-1 = 0.282 M
Regarding the dilution of the solution in Part A, we are given that 15.00 mL of the solution was diluted to a final volume of 50.00 mL. This can be used to calculate the original concentration. The formula used in this case is C1V1 = C2V2, where C1 is the original concentration, V1 is the original volume, C2 is the diluted concentration, and V2 is the final volume. Substituting C2 with the concentration we just calculated, the original concentration C1 can be calculated as: C1 = (C2V2)/V1 = (0.282 M × 50.00 mL)/ 15.00 mL = 0.94 M.
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Consider the dissociation of strong versus weak acids: HCl(aq)+H2O(l)→H3O+(aq)+Cl−(aq)HF(aq)+H2O(l)⇌H3O+(aq)+F−(aq) The first reaction is not reversible, but the second one is. So, only the conjugate of the weak acid, F−, can react with H3O+. Now consider the solubility of insoluble salts: AgCl(s)⇌Ag+(aq)+Cl−(aq)AgF(s)⇌Ag+(aq)+F−(aq) The addition of acid has no effect on silver chloride. But for the second reaction, H3O+ will react with F−, decreasing its concentration and driving the equilibrium to the right. Thus, salts that contain the conjugate of a weak acid become more soluble as the acidity of the solution increases.
Answer:
The solubility of those salts increases which contains conjugate of weak acid. Conjugate of weak acid refers to strong base such as sodium hydroxide and potassium hydroxide etc.
Explanation:
The solubility of salts in strong acidic solution increases due to the presence of conjugate of weak acid which is actually a strong base. So if the salts contain strong base, it readily react with strong acid that is present in the solution.
If 1 mol of gas is placed into a balloon under standard temperature and pressure (273 K and 1 atm), what volume would the balloon be?
Answer:
[tex]V=22.4L[/tex]
Explanation:
Hello,
In this case, considering the ideal gas equation:
[tex]PV=nRT[/tex]
It is possible to compute the volume the gas would have for the given STP conditions as:
[tex]V=\frac{nRT}{P}[/tex]
[tex]V=\frac{1mol*0.082\frac{atm*L}{mol*K}*273K}{1atm}\\\\V=22.4L[/tex]
Which correspond to the standard volume as well.
Best regards.
Answer:
The volume of the balloon would be 22.386 L
Explanation:
An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:
P * V = n * R * T
In this case:
P= 1 atmV= ?n= 1 molR= 0.082 [tex]\frac{atm*L}{mol*K}[/tex]T= 273 KReplacing:
1 atm* V= 1 mol* 0.082 [tex]\frac{atm*L}{mol*K}[/tex]*273 K
Solving:
[tex]V=\frac{1 mol*0.082\frac{atm*L}{mol*K} *273 K}{1 atm}[/tex]
V=22.386 L
The volume of the balloon would be 22.386 L
Consider a 125 mL buffer solution at 25°C that contains 0.500 mol of hypochlorous acid (HOCl) and 0.500 mol of sodium hypochlorite (NaOCl). What will be the pH of this buffer solution after adding 0.341 mol of HCl? The Ka of hypochlorous acid is 2.9 x 10-8 . Assume the change in volume of the buffer solution is negligible
Answer:
pH = 6.82
Explanation:
To solve this problem we can use the Henderson-Hasselbach equation:
pH = pKa + log[tex]\frac{[NaOCl]}{[HOCl]}[/tex]We're given all the required data to calculate the original pH of the buffer before 0.341 mol of HCl are added:
pKa = -log(Ka) = -log(2.9x10⁻⁸) = 7.54[HOCl] = [NaOCl] = 0.500 mol / 0.125 L = 4 MpH = 7.54 + log [tex]\frac{4}{4}[/tex]pH = 7.54By adding HCl, we simultaneously increase the number of HOCl and decrease NaOCl:
pH = 7.54 + log[tex]\frac{[NaOCl-HCl]}{[HOCl+HCl]}[/tex]pH = 7.54 + log [tex]\frac{(0.500mol-0.341mol)/0.125L}{(0.500mol+0.341mol)/0.125L}[/tex]pH = 6.82If the standard reduction potential of a half-cell is positive, which redox reaction is spontaneous when paired with a hydrogen electrode?
A. oxidation
B. both reduction and oxidation
C. reduction
D. neither reduction nor oxidation
If the standard reduction potential of a half-cell is positive, the reduction reaction is spontaneous when paired with a hydrogen electrode
Explanation:
The relative standard reduction potential of the half-cell in which reduction occurs; more positive than the other half-cell.If the standard reduction potential of a half-cell is positive, the reduction reaction is spontaneous when paired with a hydrogen electrode.The reduction is a chemical process in which electrons are added to an atom or an ion; it always occurs accompanied by oxidation of the reducing agent.The reduction to happen the electrons gained by the material that is being decreased must be transported from the atoms of ions of a different material.Answer:
Reduction
Explanation:
Using the complex based titration system: 50.00 mL 0.00250 M Ca2+ titrated with 0.0050 M EDTA, buffered at pH 11.0 determine (i) first pCa first before initiating the titration process and then (ii) at equivalence when all the Ca2+ is titrated to CaY2-. Please, use your text books and/or lecture notes to find potentially missing information about constants needed to solve the problem.
Answer:
i) The pCa before initiating the titration is 2.6
ii) The pCa is 6.67
Explanation:
please look at the solution in the attached Word file
What is the correct formula for the compound formed by CA2+ and NO2-
Answer:
Ca(NO2)2
Explanation:
A flammable gas made up of only carbon and hydrogen is found to effuse through a porous barrier in 1.50 min. Under the same conditions of temperature and pressure, it takes an equal volume of bromine vapor 4.73 min to effuse through the same barrier. Calculate the molar mass of the unknown gas, and suggest what this gas might be.
Answer:
A. The molar mass of the unknown gas is 16g/mol
B. Compound is CH4 i.e methane
Explanation:
A. Step 1:
Representation:
Let t1 be time for unknown gas
Let t2 be the time for bromine vapor
Let M1 be molar mass of the unknown gas
Let M2 be the molar mass of bromine vapor
A. Step 2 :
Data obtained from the question.
Time for the unknown gas (t1) = 1.50 min
Time for Br2 (t2) = 4.73 min
Molar Mass of unknown gas (M1) =?
Molar Mass of Br2 (M2) = 80 x 2 = 160g/mol
A. Step 3:
Determination of the molar mass of the unknown gas.
Applying the equation:
t2/t1 = √(M2/M1)
The molar mass of can be obtained as follow:
t2/t1 = √(M2/M1)
4.73/1.5 = √(160/M1)
Take the square of both side
(4.73/1.5)^2 = 160/M1
9.94 = 160/M1
Cross multiply to express in linear form.
9.94 x M1 = 160
Divide both side by 9.94
M1 = 160/9.94
M1 = 16g/mol
Therefore, the molar mass of the unknown gas is 16g/mol
B. Identification of the gas.
The gas contains C and H only. From the calculations made above, the molar mass of the unknown gas is 16g/mol.
We know also that the molar mass of carbon is 12g/mol and that of Hydrogen is 1g/mol
Therefore,
C + H = 16
There would be only 1 atom of C in the compound since the molar mass of the compound is 16g/mol. With these understanding, let us determine the number of H atom in the compound. This is illustrated below :
C + H = 16
12 + H = 16
H = 16 - 12
H = 4
Divide by the molar mass of H i.e 1
H = 4/1 = 4
There are 4 atoms of H in the compound. Therefore, the compound is CH4 i.e methane
The molar mass of the unknown gas is 16 g/mol hence the unknown gas is methane.
We must note that the time taken for a gas to diffuse is directly proportional to the molar mass of the gas.
Hence;
t1/t2 = √M1/M2
Let t1 = time taken for the flammable gas to diffuse = 1.50 min
Let t2 = time taken for the bromine vapor to diffuse = 4.73 min
M1 = molar mass of the flammable gas = ?
M2 = molar mass of the bromine vapor = 160 g/mol
Substituting values;
1.50/4.73 = √M1/160
(1.50/4.73)^2 = M1/160
0.1006 = M1/160
M1 = 0.1006 × 160
M1 = 16 g/mol
The unknown gas is methane.
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Calcium hydride reacts with water to form hydrogen gas according to the unbalanced equation below: CaH2(s) + H2O(l) --> Ca(OH)2(aq) + H2(g) This reaction is sometimes used to inflate life rafts, weather balloons, and the like, where a simple, compact means of generating H2 is desired. How many grams of calcium hydride are needed to generate 15.0 L of hydrogen gas at 25 degrees C and 825 torr of pressure?
Answer:
28 grams CaH₂(s) is required for production of 15L H₂(g) at 25°C and 825Torr.
Explanation:
CaH₂(s) + H₂O(l) => Ca(OH)₂(s) + H₂(g)
Using ideal gas law, PV = nRT
=> moles H₂(g) = PV/RT = [(825/760)Atm](15L)/(0.08206L·Atm·mol⁻¹·K⁻¹)(298K) = 0.6659 mol H₂(g)
From stoichiometry of given equation,
=> 0.6659 mol H₂(g) requires 0.6659 mole CaH₂(s)
Converting moles to grams, multiply by formula weight,
=> 0.6659 mole CaH₂(s) = 0.6659 mole CaH₂(s) x 42g/mole = 27.966 grams CaH₂(s) ≅ 28 grams CaH₂(s) (2 sig. figs.)
At 5000 K and 1.000 atm, 83.00% of the oxygen molecules in a sample have dissociated to atomic oxygen. At what pressure will 95.0% of the molecules dissociate at this temperature
Answer:
At [tex]P_{total} = 0.240\ atm[/tex]; 95.0% of the molecules will dissociate at this temperature
Explanation:
The chemical reaction of this dissociation is:
[tex]O_2 \leftrightarrow 2O_g[/tex]
The ICE table is as follows:
[tex]O_2 \ \ \ \ \ \ \ \leftrightarrow \ \ \ \ \ \ \ \ 2O_g[/tex]
Initial 100 0
Change -83 +166
Equilibrium 17 166
The mole fractions of each constituent is now calculated as:
[tex]Mole \ fraction \ of \ O(X_o) = \frac{166}{183}[/tex] = 0.9071
[tex]Mole \ fraction \ of \ O_2(X_o_2_}}) = \frac{17}{183}[/tex] = 0.0929
Given that the total pressure [tex]P_{total}[/tex] = 1.000 atm ; the partial pressure of each gas is calculated by using Raoult's Law.
[tex]Partial \ Pressure \ of \ O (P_o) = X_oP_{total}\\\\ = 0.9071 \ atm[/tex]
[tex]Partial \ Pressure \ of \ O_2 (P_o_2) = X_oP_{total}\\\\ = 0.0929 \ atm[/tex]
Now; we proceed to determine the equilibrium constant [tex]K_c[/tex]; which is illustrated as:
[tex]K_c = \frac{Po^2}{Po_2} \\ \\ K_c = \frac{(0.9072)^2}{0.0929} \\ \\ =8.86 \ atm[/tex]
Let assume that the partial pressure of [tex]O_2[/tex] be x ;&
the change in pressure of [tex]O_2[/tex] be y ; then
we can write that the following as the changes in concentration of species :
[tex]O_2 \ \ \ \ \ \ \ \leftrightarrow \ \ \ \ \ \ \ \ 2O_g[/tex]
Initial x 0
Change -y +2 y
Equilibrium x - y 2 y
From above; we can rewrite our equilibrium constant as:
[tex]K_c = \frac{(2y)^2}{x-y} \\ \\ 8.86 = \frac{(2y)^2}{x-y} ----- equation (1)[/tex]
From the question; we are told that provided that 95% of the molecules dissociate at this temperature. Therefore, we have:
[tex]\frac{y}{x}*100 = 95[/tex]% -------- equation (2)
Solving and equating equation 1 and 2 ;
x = 0.123 atm
y = 0.117 atm
Thus, the pressure required can be calculated as :
[tex]P_{total} = (x-y) +2y \\ \\ P_{total} = (0.123- 0.117)+ 2(0.123) \\ \\ \\ P_{total} = 0.240 \ atm[/tex]
To a flask, 15.0 mL of 1.25 M hydrofluoric acid is added. Then, 3.05 M KOH is used to titrate the acid sample. Write the balanced net ionic equation for the acid-base reaction.
Answer:
HF + OH- = F- + H2O
Explanation:
Since hydrofluoric acid does not ionize in aqueous solution, the fluoride ion is still present as part of the product
Answer:
H+ (aq) + OH-(aq) → H2O(l)
Explanation:
Step 1: Data given
Volume of hydrofluoric acid = 15.0 mL = 0.015 L
Molarity = 1.25 M
Molarity of KOH = 3.05 M
Step 2: The unbalanced equation
HF(aq) + KOH(aq) → KF(aq) + H2O(l)
This equation is already balanced
Step 3: The net ionic equation
The net ionic equation shows only those elements, compounds, and ions that are directly involved in the chemical reaction.
The elements, compounds, and ions that do not take part in the chemical reaction are called spector ions.
H+ (aq) + F-(aq) + K+(aq) + OH-(aq)→ K+(aq) +F-(aq) + H2O(l)
We'll remove all the spector ions.
H+ (aq) + OH-(aq) → H2O(l)
An object at 20∘C absorbs 25.0 J of heat. What is the change in entropy ΔS of the object? Express your answer numerically in joules per kelvin. ΔS = nothing J/K Request Answer Part E An object at 500 K dissipates 25.0 kJ of heat into the surroundings. What is the change in entropy ΔS of the object? Assume that the temperature of the object does not change appreciably in the process. Express your answer numerically in joules per kelvin. ΔS = nothing J/K Request Answer Part F An object at 400 K absorbs 25.0 kJ of heat from the surroundings. What is the change in entropy ΔS of the object? Assume that the temperature of the object does not change appreciably in the process. Express your answer numerically in joules per kelvin. ΔS = nothing J/K Request Answer Part G Two objects form a closed system. One object, which is at 400 K, absorbs 25.0 kJ of heat from the other object,which is at 500 K. What is the net change in entropy ΔSsys of the system? Assume that the temperatures of the objects do not change appreciably in the process. Express your answer numerically in joules per kelvin.
Question:
Part D) An object at 20∘C absorbs 25.0 J of heat. What is the change in entropy ΔS of the object? Express your answer numerically in joules per kelvin.
Part E) An object at 500 K dissipates 25.0 kJ of heat into the surroundings. What is the change in entropy ΔS of the object? Assume that the temperature of the object does not change appreciably in the process. Express your answer numerically in joules per kelvin.
Part F) An object at 400 K absorbs 25.0 kJ of heat from the surroundings. What is the change in entropy ΔS of the object? Assume that the temperature of the object does not change appreciably in the process. Express your answer numerically in joules per kelvin.
Part G) Two objects form a closed system. One object, which is at 400 K, absorbs 25.0 kJ of heat from the other object,which is at 500 K. What is the net change in entropy ΔSsys of the system? Assume that the temperatures of the objects do not change appreciably in the process. Express your answer numerically in joules per kelvin.
Answer:
D) 85 J/K
E) - 50 J/K
F) 62.5 J/K
G) 12.5 J/K
Explanation:
Let's make use of the entropy equation: ΔS = [tex] \frac{Q}{T} [/tex]
Part D)
Given:
T = 20°C = 20 +273 = 293K
Q = 25.0 kJ
Entropy change will be:
ΔS = [tex] \frac{25*1000}{293} [/tex]
= 85 J/K
Part E)
Given:
T = 500K
Q = -25.0 kJ
Entropy change will be:
ΔS = [tex] \frac{-25*1000}{500} [/tex]
= - 50 J/K
Part F)
Given:
T = 400K
Q = 25.0 kJ
Entropy change will be:
ΔS = [tex] \frac{25*1000}{400} [/tex]
= 62.5 J/K
Part G:
Given:
T1 = 400K
T2 = 500K
Q = 25.0 kJ
The net entropy change will be:
ΔS = [tex] (\frac{25*1000}{400}) + (\frac{-25*1000}{500}[/tex]
= 12.5 J/K
Answer:
A) The change in entropy [tex]\delta S = 0.085J/K[/tex]
B) The change in entropy [tex]\delta S = -50J/K[/tex]
C) The change in entropy [tex]\delta S = 62.5J/K[/tex]
D) The net change in entropy [tex]\delta S = 12.5J/K[/tex]
Explanation:
A)
[tex]T = 20^oC + 273k\\\\T = 293k[/tex]
expression for change in entropy,
[tex]\delta S = \frac{\delta Q}{T}\\\\\delta S = \frac{25}{293}\\\\\delta S = 0.085J/K[/tex]
B) [tex]\delta S = \frac{\delta Q}{T}\\\\\delta S = \frac{-25*10^3}{500}\\\\\delta S = -50J/K[/tex]
The negative sign indicates the heat lost into the surrounding
C)
[tex]\delta S = \frac{\delta Q}{T}\\\\\delta S = \frac{25*10^3}{400}\\\\\delta S = 62.5J/K[/tex]
The entropy remains constant in the adiabatic process because no heat is given to the system in this process.
D)
[tex]\delta S_1 = \frac{\delta Q_1}{T_1}\\\\\delta S_1 = \frac{25*10^3}{400}\\\\\delta S_1 = 62.5J/K[/tex]
similarly,
[tex]\delta S_2 = \frac{\delta Q_2}{T_2}\\\\\delta S_2 = \frac{25*10^3}{500}\\\\\delta S_2 = 50J/K[/tex]
Therefore the net change in entropy is,
[tex]\delta S = \delta S_1 - \delta S_2\\\\\delta S = 62.5 - 50\\\\\delta S = 12.5J/K[/tex]
Entropy is not a conserved quantity because it can be created but cannot be destroyed.
The net change in entropy is calculated by difference of the change in entropy at two different temperatures.
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A certain half-reaction has a standard reduction potential +0.80 V . An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.9 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell.
a. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have?
b. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have?
Answer:
a. Minimum 1.70 V
b. There is no maximum.
Explanation:
We can solve this question by remembering that the cell potential is given by the formula
ε⁰ cell = ε⁰ reduction - ε⁰ oxidation
Now the problem states the cell must provide at least 0.9 V and that the reduction potential of the oxidized species 0.80 V, thus
ε⁰ reduction - ε⁰ oxidation ≥ ε⁰ cell
Since ε⁰ oxidation is by definition the negative of ε⁰ reduction , we have
ε⁰ reduction - ( 0.80 V ) ≥ 0.90 V
⇒ ε⁰ reduction ≥ 1.70 V
Therefore,
(a) The minimum standard reduction potential is 1.70 V
(b) There is no maximum standard reduction potential since it is stated in the question that we want to have a cell that provides at leat 0.9 V
If the vapor pressure of an aqueous solution containing 6.00 moles of a nonvolatile solute has a vapor pressure of 19.8 torr, and given that the vapor pressure of water at room temperature is 23.7 torr, how many total moles are present in solution? Your answer should have three significant figures.
Answer:
36.5 mol
Explanation:
The vapor pressure of a solution of a non volatile solute in water is given by Raoult´s law:
P H₂O = χ H₂O x P⁰ H₂O
where χ H₂O is the mole fraction of water in the solution and P⁰ H₂O
In the turn the mole fraction is given by
χ H₂O = mol H₂O / total # moles = mol H₂O /ntot
Thus
P H₂O = mole H₂O / n tot x P⁰ H₂0
now the mol of H₂O is equal n tot - 6 mol solute
Plugging the values given in the question and solving the resultant equation
19.8 torr = ( ntot - 6 ) x 23.7 torr / n tot
19.8 ntot = 23.7 ntot - 142.2
ntot = 36.5 ( rounded to 3 significant figures )
There are three competing factors at play here: 1. The effective nuclear charge 2. The size of the atom and the force of attraction according to Coulomb's law 3. A pair of electrons in an orbital The first ionization energy is the energy required to completely remove the first electron from the atom. The higher in energy an electron is to start with, the less additinal energy will be required to remove it, which translates to a lower ionization energy. By the same token, an electron arrangement which is lower in energy will require more energy to remove an electron.
Answer:
These three factors are required for ionization potential or ionization energy.
Explanation:
Ionization potential refers to the amount of energy which is required for the removal of outermost electron of the atom. If the atom size is big so the outermost electron is far from the nucleus and low energy is required for its removal due to lower force of attraction between nucleus and outermost electron. If the nuclear charge is higher, so the electron is tightly held by the nucleus and require more energy for its removal. Nuclear charge means number of protons present in the nucleus.
Consider the perbromate anion. What is the central atom? Enter its chemical symbol. How many lone pairs are around the central atom? What is the ideal angle between the bromine-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the bromine-oxygen bonds to be ...
Answer:
See explanation
Explanation:
The central atom in the perbromate ion is bromine. The chemical symbol of bromine is Br. There are no lone pairs around the central bromine atom. The ion is tetrahedral in shape hence we expect a bond angle of 109°. 27 which is the ideal tetrahedral bond angle. The actual bond angle of the prebromate ion is 109.5°. The perbromate ion is BrO4^-
The observed bond angle is very close to the ideal value because of the absence of lone pairs of electrons from the central atom in the ion.
The perbromate anion, BrO4-, has Bromine (Br) as its central atom and two lone pairs of electrons. This configuration results in a square planar molecular structure, presenting ideal Bromine-Oxygen bond angles of 90° and 180°. These angles are expected to be virtually accurate due to minimization of lone pair-bonding pair repulsions.
Explanation:The perbromate anion, represented by the chemical formula BrO4-, has bromine (Br) as its central atom. Based on the octet rule, the central bromine atom is surrounded by four oxygen atoms and has two lone pairs of electrons. Given this arrangement, the perbromate anion exhibits an octahedral electron-pair geometry, but due to the presence of the two lone pairs, its molecular structure is square planar. The ideal angle between the Bromine-Oxygen bonds in a square planar structure is 90° or 180°. Since the lone pairs occupy the positions minimizing their interactions with the bonded oxygen atoms, the actual angle in the perbromate anion is expected to closely match this ideal angle.
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Three elements have the electron configurations 1s22s22p63s1, 1s22s22p63s2, and 1s22s22p5. The first ionization energies of these elements (not in the same order) are 1.681, 0.738, and 0.496 MJ/mol. The atomic radii are 160, 186, and 64 pm. Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration.
Answer:
Explanation:
1s²2s²2p⁶3s² = magnesium ionization energy, 0.738 MJ/mol atomic radius 160 pm
1s²2s²2p⁶3s¹ = Sodium, ionization energy, 0.496 MJ/mol, atomic radius 186 pm
1s²2s²2p⁵ = Florine ionization energy, 1.681 MJ/mol, atomic radius 64 pm
Ionization energy is the minimum amount of energy needed to remove an electron from its orbital around the atom from the influence of the atom while atomic radius is one-half the distance between the nuclei of identical atoms that are bonded together.
It is difficult to prepare an amide from a carboxylic acid and an amine directly, since an acid-base reaction occurs which renders the amine nitrogen non-nucleophilic. Typically, in such an amide synthesis, the carboxylic acid OH group is first transformed into a better, nonacidic leaving group. In practice, amides are often prepared by treating the carboxylic acid with dicyclohexylcarbodiimide (DCC). The amine is then added and nucleophilic acyl substitution occurs easily because dicyclohexylurea is a good leaving group. This method of amide bond formation is a key step in the laboratory synthesis of peptide bonds (amide bonds) between protected amino acids. Draw curved arrows to show the movement of electrons in this step of the mechanism.
Answer:
See explaination
Explanation:
Please kindly check attachment for the step by step solution.