Answer:
2-hexanone
Explanation:
First, we'll begin by:
1. Locating the longest continuous chain i.e haxane
2. Determine the functional group in the compound. The functional group in ketone (C=O). This changes the name from hexane to hexanone i.e replacing the -e in at the end in hexane with -one to make it hexanone.
3. Give the functional group the lowest low count. In doing this, we'll start counting from the left. The functional group is at carbon 2.
Note: no substitute group is attached.
Now, in naming the compound, we must indicate the position of functional group as illustrated below:
The name of the compound is:
2-hexanone
The compound is called 2-hexanone. This is because there is a six carbon chain with a ketone functional group attached to the second carbon.
Explanation:You are dealing with an organic compound formula. Let's identify the compound based on its structure. The compound you have given is CH3 - C - CH2 - CH2 - CH2 - CH3. This is a 6 carbon chain and there is double bond between Oxygen and the second carbon. Now, when naming compounds in chemistry we firstly count the length of the chain, it is hexane. Then, we look for any functional group and where it is attached in the chain. A ketone functional group is CO, so this would make it a hexanone. As the CO is attached at the second carbon, it is 2-hexanone. So the correct answer for the name of the compound would be 2-hexanone.
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Four gases were combined in a gas cylinder with these partial pressures: 3.5 atm N2, 2.8 atm O2, 0.25 atm Ar, and 0.15 atm He.
What is the total pressure inside the cylinder?
6.7
atm
What is the mole fraction of N2 in the mixture?
0.52
atm
2 equations: First, P subscript T equals P subscript 1 plus P subscript 2 plus P subscript 3 plus ellipses plus P subscript n. Second: StartFraction P subscript a over P subscript T EndFraction equals StartFraction n subscript a over N subscript T EndFraction.
What is the mole fraction of O2 in the mixture?
atm
What is the mole fraction of Ar in the mixture?
atm
Answer:
Mole Fraction of O2 --> 0.42
Mole Fraction of Ar --> 0.037
Explanation:
Answer:
Mole Fraction of O2 --> 0.42
Mole Fraction of Ar --> 0.037
Explanation:
The decomposition of nitramide, O 2 NNH 2 , O2NNH2, in water has the chemical equation and rate law O 2 NNH 2 ( aq ) ⟶ N 2 O ( g ) + H 2 O ( l ) rate = k [ O 2 NNH 2 ] [ H + ] O2NNH2(aq)⟶N2O(g)+H2O(l)rate=k[O2NNH2][H+] A proposed mechanism for this reaction is O 2 NNH 2 ( aq ) k 1 ⇌ k − 1 O 2 NNH − ( aq ) + H + ( aq ) ( fast equilibrium ) O2NNH2(aq)⇌k−1k1O2NNH−(aq)+H+(aq)(fast equilibrium) O 2 NNH − ( aq ) k 2 −→ N 2 O ( g ) + OH − ( aq ) ( slow ) O2NNH−(aq)→k2N2O(g)+OH−(aq)(slow) H + ( aq ) + OH − ( aq ) k 3 −→ H 2 O ( l ) ( fast ) H+(aq)+OH−(aq)→k3H2O(l)(fast) What is the relationship between the observed value of k k and the rate constants for the individual steps of the mechaanism?
Answer:
Explanation:
The given overall reaction is as follows:
O 2 N N H ₂( a q ) k → N ₂O ( g ) + H ₂ O( l )
The reaction mechanism for this reaction is as follows:
O ₂ N N H ₂ ⇌ k 1 k − 1 O ₂N N H ⁻ + H ⁺ ( f a s t e q u i l i b r i u m )
O ₂ N N H − k ₂→ N ₂ O + O H ⁻ ( s l ow )
H ⁺ + O H − k ₃→ H ₂ O ( f a s t )
The rate law of the reaction is given as follows:
k = [ O ₂ N N H ₂ ] / [ H ⁺ ]
The rate law can be determined by the slow step of the mechanism.
r a t e = k ₂ [ O ₂ N N H ⁻ ] . . . ( 1 )
Since, from the equilibrium reaction
k e q = [ O ₂ N N H ⁻ ] [ H ⁺ ] /[ O ₂ N N H ₂ ] = k ₁ /k − 1
[ O ₂ N N H ⁻] = k ₁ /k − 1 × [ O ₂ N N H ₂ ] /[ H ⁺ ]. . . . ( 2 )
Substitituting the value of equation (2) in equation (1) we get.
r a t e = k ₂ k ₁/ k − 1 × [ O ₂ N N H ₂ ] /[ H ⁺ ]
Therefore, the overall rate constant is
k = k₂k₁/k-1
The observed rate constant k is related to the individual rate constants of the mechanism by the equation k = k2 (k1/k-1), where k2 is the rate constant of the rate-determining slow step and k1/k-1 is the equilibrium constant of the first fast equilibrium step.
Explanation:The relationship between the observed rate constant k (in the rate law) and the rate constants for the individual steps (k1, k-1, k2, k3) in the proposed mechanism for the decomposition of nitramide can be determined by examining the rate-determining step (RDS). In a reaction mechanism, the slowest step controls the overall reaction rate. For the given mechanism:
O2NNH2(aq) ⇌k1⇌k−1 O2NNH−(aq) + H+(aq) (fast equilibrium)O2NNH−(aq) →k2 N2O(g) + OH−(aq) (slow)H+(aq) + OH−(aq) →k3 H2O(l) (fast)the observed rate law is rate = k [O2NNH2] [H+]. Because the second step is slow, it is the RDS. The equilibrium of the first step means that the concentration of the intermediate O2NNH−(aq) can be expressed in terms of the concentrations of the reactants O2NNH2 and H+. Therefore, the observed rate constant k is a function of the rate constants of the individual steps, particularly k2 and the equilibrium constant (K = k1/k−1) from the first step. Hence, we can conclude that k is equal to k2 multiplied by the equilibrium constant of the first step, where k = k2 (k1/k−1)
Use the reaction data in the table below to select the answer choice that best describes this reaction.
Reaction Enthalpy Change
345.7 kJ/mol
Reaction Entropy Change
-25. 3 J/molK
This reaction is never spontaneous.
This reaction is spontaneous at all temperatures.
This reaction is spontaneous at low temperatures.
This reaction is spontaneous at high temperatures
Answer: This reaction is never spontaneous
Explanation:
According to Gibbs equation:
[tex]\Delta G=\Delta H-T\Delta S[/tex]
[tex]\Delta G[/tex] = Gibb's free energy change
[tex]\Delta H[/tex] = enthalpy change
T = temperature
[tex]\Delta S[/tex] = entropy change
A reaction becomes spontaneous when [tex]\Delta G[/tex] = Gibb's free energy change is negative.
[tex]\Delta G=+ve-T(-ve)[/tex]
[tex]\Delta G=+ve+ve[/tex]
[tex]\Delta G=+ve[/tex]
Thus this reaction is never spontaneous
A student dissolves 11.1 g of potassium hydroxide (KOH) in 250. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 23.0 °C to 34.0 °C over the course of 4.6 minutes.
Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction:
KOH(s) â K (aq) + OH (aq)
You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits.
Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction.
Is this reaction exothermic, endothermic, or neither?
The dissolution of potassium hydroxide (KOH) in water is an exothermic process, as indicated by the increase in temperature when KOH is dissolved in water.
Explanation:The dissolution of potassium hydroxide (KOH) in water is an exothermic process. This can be determined based on the observation that the temperature of the water increased from 23.0°C to 34.0°C when 11.1 g of KOH was dissolved in 250.0 g of water. The positive change in temperature indicates that heat was released by the KOH dissolving in water, resulting in an increase in temperature.
The reaction is exothermic as the temperature of the water rises from 23.0°C to 34.0°C, indicating the release of heat.
To determine if the reaction is exothermic or endothermic, we need to look at the temperature change during the dissolution of potassium hydroxide (KOH).
Since the temperature of the water rises from 23.0 °C to 34.0 °C, which is an increase of 11.0 °C, this indicates that the solution absorbs heat.
This increase in temperature demonstrates that the reaction releases heat into the surroundings, thus it is an exothermic reaction. In an exothermic reaction, the temperature of the surroundings rises because energy is released.
Example Calculation:
Mass of water (m): 250 g
Specific heat capacity (C) of water: 4.184 J/g°C
Temperature change (ΔT): 34.0 °C - 23.0 °C = 11.0 °C
Heat (q) absorbed by the solution: q = m × C × ΔT = 250 g × 4.184 J/g°C × 11.0 °C = 11, 506 J or 11.506 kJ
Since the heat is released by the dissolution of KOH, the reaction is said to be exothermic.
The scientist finds fossilized remains of other species in the same rock layer as the trilobite. What can the scientist conclude about
these other fossils?
The Organisms that formed them likely lived during the Paleozoic era.
Final answer:
When trilobite fossils are found alongside other species in the same rock layer, a scientist can infer that these organisms lived during the same time period and may have had similar environmental conditions. Trilobites are used as index fossils which can determine the age of the rocks they are in due to their distinct presence in the geological record from 500 to 600 million years ago.
Explanation:
When a scientist discovers fossilized remains of other species in the same rock layer as a trilobite, they can draw some important conclusions. Since trilobites were widespread marine animals that lived between 500 and 600 million years ago, any other fossils found within the same stratum are likely from the same geological period. This is due to the principle of superposition, which states that in any undisturbed sequence of rocks deposited in layers, the youngest layer is on top and the oldest on bottom, each layer being younger than the one beneath it and older than the one above it.
Furthermore, trilobites are known as index fossils because they were widespread, rapidly evolving, and limited in geological time. Therefore, they serve as indicators of the age of the rock layer in which they are found. Discovering other species in conjunction with trilobite fossils suggests that these organisms also lived during the same time period and may have shared similar environments. This can be used to infer that these species are from the same age and geological period as the trilobites.
The study of these fossils can provide invaluable insight into the biodiversity and ecological conditions of prehistoric marine environments. Moreover, these findings contribute to our understanding of evolutionary history and may help to identify patterns of mass extinction or other significant pale ontological events.
The formation of ClF (chlorine monofluoride) from its elements has an equilibrium constant of 22.3 at room temperature. Which of the following statements is correct if chlorine gas and fluorine gas are mixed at room temperature?
The reaction will form products until equilibrium is established
Products are quickly formed
A negligible amound of ClF is formed
Products are slowly formed
Answer:
A the reaction will form
Explanation:
Between HClO3 and HIO3, which is stronger and why? Question 16 options: 1) HClO3 is stronger because chlorine is in a higher oxidation state than iodine. 2) HClO3 is stronger because chlorine is more electronegative than iodine. 3) HIO3 is stronger because iodine is in a higher oxidation state than chlorine. 4) HIO3 is stronger because iodine is less electronegative than chlorine.
Answer:
2) HClO3 is stronger because chlorine is more electronegative than iodine.
Explanation:
The more electronegative the element is the more strong or acidic it becomes.
Chlorine being more electronegative than Iodine makes it easier for it to pull the electron of hydrogen more strongly and hence has a higher tendency to release a H+ unit. Hence that makes it stronger.
HClO3 is stronger than HIO3 because chlorine is more electronegative than iodine.
Chloric acid (HClO3) is more stronger than Iodic acid (HIO3) because chlorine is more electronegative than iodine. As we go from top to bottom in the periodic table, the atomic size increases and electronegativity decreases.
Electronegativity is the ability of an atom to attract electron pair towards itself. Chlorine atom comes on the top whereas iodine is present lower than chlorine in the periodic table so the atomic size of chlorine is smaller and higher value of electronegativity as compared to iodine so we can conclude that Chloric acid (HClO3) is more stronger than Iodic acid (HIO3).
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Which process is an example of a physical change?
burning
rusting
flattening
ripening
Answer:
The answer is flattening
Explanation:
A physical change is generally something that affects the shape of form of the matter and a chemical change results from a chemical reaction. Flames are caused by chemical reactions, as is rust, and the process of a fruit becoming ripe. Thus, the answer is “flattening”.
In the realm of chemistry, only flattening out of the listed options is considered a physical change as it alters the condition of a substance without modifying its underlying chemical structure.
Explanation:In the context of Chemistry, physical changes are processes that change the form or appearance of a substance, but not its chemical composition. Of the processes you listed: burning, rusting, flattening, and ripening, flattening is an example of a physical change. For instance, if you have a piece of aluminum foil and you flatten it, it is still aluminum foil - no new substance is created. On the other hand, burning, rusting, and ripening are chemical changes because they result in new substances being formed.
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Consider the following reaction NaOH (s) --> Na+ (aq) + OH- (aq)
Is the reactant an __________.
Answer:
base and it's in solution
Explanation:
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Which statements describes why ethyl methyl ether (b.p. 7.9°C) and 1-propanol (b.p. 97.2°C) have such different boiling points despite identical molar masses? A) Ethyl methyl ether has more hydrogen bonding than 1-propanol. B) 1-propanol has more hydrogen bonding than ethyl methyl ether. C) Ethyl methyl ether has greater dispersion forces than 1-propanol. D) 1-propanol has greater dispersion forces than ethyl methyl ether. E) Ethyl methyl ether has greater molecular volume than 1-propanol.
Answer:
B) 1-propanol has more hydrogen bonding than ethyl methyl ether.
Explanation:
1-propanol and ethyl methyl ether look very similar but have very different boiling points. They both have three carbon atoms but ethyl methyl ether has an oxygen atom.
Ethyl methyl ether has both London dispersion forces and dipole-dipole interactions.
1-Propanol has London dispersion forces, dipole-dipole interactions and hydrogen bonding.
1-propanol has more hydrogen bonding than ethyl methyl ether which explains why they both have different boiling points.
An aqueous solution is 3.23M in tartaric acid (C4H06). The solution's density is 1.023 g/mL.
Calculate the solution's molality in tartaric acid.
Answer:
Molality = 6.0 m
Explanation:
The molecular weight of tartaric acid = 150.087 g/mol
Given that:
Density of the solution = 1.023 g/mL
Molarity = 3.23M
Density is given as : [tex]Molarity ( \frac{1}{molality } +\frac{mol.wt}{1000} )[/tex]
∴
[tex]1.023 = 3.23 (\frac{1}{molality } +\frac{150.087}{1000} )[/tex]
[tex]\frac{1}{molality } =( \frac{1.023}{3.23} - \frac{150.087}{1000} )[/tex]
[tex]\frac{1}{molality } =0.3167 - 0.1500[/tex]
[tex]\frac{1}{molality } = 0.1667[/tex]
Molality = [tex]\frac{1}{0.1667}[/tex]
Molality = 5.999 m
Molality ≅ 6.0 m
Use scientific reasoning to explain what happens if 0.87 mol NaCl is dissolved in pure water creating 3.00 L of solution, what is its molarity of the resulting solution?
Answer : The molarity of the resulting solution is, 0.29 M
Explanation :
When NaCl dissolved in water then it dissociates to give sodium ions and chloride ions.
Given,
Moles of NaCl = 0.87 mol
Volume of solution = 3.00 L
Molarity : It is defined as the number of moles of solute present in one liter of volume of solution.
Formula used :
[tex]\text{Molarity}=\frac{\text{Moles of }NaCl}{\text{Volume of solution (in L)}}[/tex]
Now put all the given values in this formula, we get:
[tex]\text{Molarity}=\frac{0.87mol}{3.00L}=0.29mole/L=0.29M[/tex]
Therefore, the molarity of the resulting solution is, 0.29 M
H2SO4 is a strong acid because the first proton ionizes 100%. The Ka of the second proton is 1.1x10-2. What would be the pH of a solution that is 0.100 M H2SO4? Account for the ionization of both protons.
Question options:
a) 2.05
b) 0.963
c) 0.955
d) 1.00
Answer:
b) 0.963
Explanation:
H2SO4→ HSO4- + H3O+
HSO4- + H2O ⇌ SO42- + H3O+
Construct ICE table:
HSO4- (aq) + H2O ⇌ SO42- (aq) + H3O+ (aq)
I 0.1 solid & 0 0.1
C -x liquid + x + x
E 0.1 - x are ignored x 0.1 + x
Calculate x
Ka = products/reactants
= [tex]\frac{[SO42-] [H3O+]}{[HSO4-]}[/tex]
0.011 = [tex]\frac{x (0.1 + x)}{0.1 - x}[/tex]
0.011 x (0.1 -x) = o.1x + x^2
0.0011 - 0.011 x - o.1x - x^2 = 0
0.0011 - 0.011 x - x^2 = 0
Use formula to solve for quadratic equation
x = [tex]{ -b +,-\sqrt{b^2 - 4ac[/tex] / 2a
a = -1, b = -0.111, c = 0.001
Solve for x
x = [tex]\sqrt[-(-o.111)]{(-0.111)^2 - 4(-1) (0.0011) }[/tex] / 2(-1)
x = 0.111 +,- [tex]\sqrt{0.012321 + 0.0044}[/tex] / -2
x = 0.111 +,- [tex]\sqrt{0.016721}[/tex] / -2
x = [tex]\frac{0.111 +, - 0.1293}{-2}[/tex]
x = [tex]\frac{0.111 + 0.1293}{-2}[/tex] , x = [tex]\frac{0.111 - 0.1293}{-2}[/tex]
x = [tex]\frac{0.2403}{-2}[/tex] , x = [tex]\frac{0.0183}{-2}[/tex]
x = - 0.12015 , x = 0.00915
x cannot be negative, so
x = 0.00915 M
Calculate [H3O+]
[H3O+] = 0.1 M + x
[H3O+] = 0.1 M + 0.00915 M
[H3O+] = 0.10915 M
Clculate pH
pH = - log [ H3O+]
pH = - log [ 0.10915]
pH = 0.963
Final answer:
The pH of a 0.100 M H2SO4 solution is approximately 1.00, considering the complete ionization of the first proton and the partial ionization of the second proton, which is less significant due to its lower Ka value.
Explanation:
The question asks about the pH of a 0.100 M H2SO4 solution, taking into account the ionization of both protons. Sulfuric acid (H2SO4) is a strong diprotic acid that dissociates completely for the first proton, yielding a concentration of 0.100 M H+ and 0.100 M HSO4-. The second proton dissociation is less extensive, with a given Ka of 1.1x10-2, which we need to include in our calculation of pH.
First step ionization (complete dissociation):
H2SO4 → H+ + HSO4-
Second step ionization (partial dissociation):
HSO4- ↔ H+ + SO42- (Ka = 1.2 x 10-2)
To calculate the pH, we first consider the complete ionization of the first proton, which directly gives us 0.100 M of H+. The pH contribution from this ionization is pH = -log(0.100) = 1.00. Then we consider the second ionization of HSO4-. Given the Ka and the initial HSO4- concentration of 0.100 M, we can set up an equilibrium expression to find the additional contribution of H+ from the second ionization. However, because the ionization is low, the change in concentration of H+ due to the second ionization can be negligible for this approximate calculation. Therefore, we can assume the pH of the solution largely results from the first dissociation.
Therefore, the answer is that the pH of the 0.100 M H2SO4 solution is approximately 1.00.
At 500 K the reaction 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g) has Kp = 51 In an equilibrium mixture at 500 K, the partial pressure of NO is 0.125 atm and Cl2 is 0.165 atm. What is the partial pressure of NOCl in the equilibrium mixture?
Answer:
p3=0.36atm (partial pressure of NOCl)
Explanation:
2 NO(g) + Cl2(g) ⇌ 2 NOCl(g) Kp = 51
lets assume the partial pressure of NO,Cl2 , and NOCl at eequilibrium are P1 , P2,and P3 respectively
[tex]Kp=\frac{[NOCl]^{2} }{[NO]^{2} [Cl_2] }[/tex]
[tex]Kp=\frac{[p3]^{2} }{[p1]^{2} [p2] }[/tex]
p1=0.125atm;
p2=0.165atm;
p3=?
Kp=51;
On solving;
p3=0.36atm (partial pressure of NOCl)
The reaction,
[tex]2 NO(g)+Cl_2(g) \rightleftharpoons 2 NOCl (g)[/tex]Given values,
Pressure,
[tex]P_1 = 0.125 \ atm[/tex][tex]P_2 = 0.165 \ atm[/tex]Value of Kp,
[tex]51[/tex]Now,
→ [tex]K_p = \frac{[NOCl]^2}{[NO]^2[Cl_2]^2}[/tex]
or,
→ [tex]K_p = \frac{[P_3]^2}{[P_1]^2[P_2]}[/tex]
By substituting the values,
[tex]51 = \frac{[P_3]^2}{[0.125]^2[0.165]}[/tex]
[tex]P_3 = 0.36 \ atm[/tex]
Thus the response above is appropriate.
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The mass of the deuterium molecule D2 is twice that of the hydrogen molecule H2. If the vibrational frequency of H2 is 1.29 × 1014 Hz, what is the vibrational frequency of D2, assuming that the "spring constant" of attracting forces is the same for the two species? Answer in units of Hz.
Answer:
9.12x10¹³ Hz
Explanation:
The vibrational frequency (ω) of a molecule is given by:
[tex] \omega = \sqrt{\frac{k}{\mu}} [/tex]
Where:
k: is the spring constant
μ: is the reduced mass
The reduced mass of a diatomic molecule is:
[tex] \frac{1}{\mu} = \frac{1}{m_{a}} + \frac{1}{m_{b}} [/tex]
Where ma and mb are the atomic masses of the atoms a and b, respectively, of the diatomic molecule.
Hence, the vibrational frequency of the hydrogen molecule is:
[tex]\omega_{H_{2}} = \sqrt{\frac{k}{\mu_{H_{2}}}}[/tex] (1)
From equation (1) we can find k:
[tex] k = \omega_{H_{2}}^{2}*\mu_{H_{2}} [/tex] (2)
The vibrational frequency of the deuterium molecule is:
[tex] \omega_{D_{2}} = \sqrt{\frac{k}{\mu_{D_{2}}}} [/tex] (3)
By entering equation (2) into equation (3) we can calculate the vibrational frequency of the deuterium molecule:
[tex] \omega_{D_{2}} = \sqrt{\frac{\omega_{H_{2}}^{2}*\mu_{H_{2}}}{\mu_{D_{2}}}} [/tex]
[tex] \omega_{D_{2}} = \sqrt{\frac{\omega_{H_{2}}^{2}*\mu_{H_{2}}}{2*\mu_{H_{2}}}} [/tex]
[tex] \omega_{D_{2}} = \frac{\omega_{H_{2}}}{\sqrt{2}} = \frac{1.29 \cdot 10^{14} Hz}{\sqrt{2}} = 9.12 \cdot 10^{13} Hz [/tex]
Therefore, the vibrational frequency of the deuterium molecule is 9.12x10¹³ Hz.
I hope it helps you!
The vibrational frequency of D₂ is : 9.12 * 10¹³ Hz
Given that:
Vibrational frequency ( w ) = [tex]\sqrt{\frac{k}{u} }[/tex]
u = reduced mass
The reduced mass of a diatomic molecule is expressed as
[tex]\frac{1}{u} = \frac{1}{m_{a} } + \frac{1}{m_{b} }[/tex]
Where : Ma and Mb are the atomic masses of mass A and mass B
First step : expressing the vibrational frequency of the hydrogen molecule
wH₂ = [tex]\sqrt{\frac{k}{uH_{2} } }[/tex] ----- ( i )
from the equation
k = ( wH₂ )² * uH₂ ---- ( ii )
Next step : expressing the vibrational frequency of the deuterium molecule.
wD₂ = [tex]\sqrt{\frac{k}{uD_{2} } }[/tex] ---- ( iii )
Insert equation ( ii ) into equation ( iii )
wD₂ = [tex]\frac{wH_{2} }{\sqrt{2} }[/tex] = ( 1.29 * 10¹⁴ ) / ( √2 ) = 9.12 * 10¹³ Hz
Hence we can conclude that The vibrational frequency of D₂ is : 9.12 * 10¹³ Hz.
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If you left a block of dry ice in a bowl at room temperature all day, what would happen to it?
Answer:
It would evaporate.
Explanation:
If you left it on room temperature it would evaporate.
Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced and contains state symbols after every reactant and product.
The given question is incomplete. The complete question is :
Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced and contains state symbols after every reactant and product
[tex]HNO_3(aq)+H_2O(l)\rightarrow[/tex]
Answer: The complete equation is [tex]HNO_3(aq)+H_2O(l)\rightarrow NO_3^-(aq)+H_3O^+(aq)[/tex]
Explanation:
According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.
[tex]HNO_3[/tex] being a strong acid dissociates to give [tex]H^+[/tex] ions an [tex]H_2O[/tex] will act as base and accept [tex]H^+[/tex] to form [tex]H_3O^+[/tex]
Thus the complete equation is [tex]HNO_3(aq)+H_2O(l)\rightarrow NO_3^-(aq)+H_3O^+(aq)[/tex]
Relate energy levels to the amount of energy their electrons have
In atoms, electrons exist on specific, discrete energy levels, which correspond to distinct values of the principal quantum number 'n'. Electricity fills these 'shells' from the lowest to the highest energy state. Transitions between energy levels require definite energy changes.
Explanation:The energy levels of electrons in an atom can be understood using the principal quantum number often denoted by 'n'. Electrons exist only on specific, discrete energy levels and not between them. This principle is known as the quantization of energy. Each energy level is associated with a specific value of 'n', with n = 1, 2, 3, and so on. The greater the 'n' value, the higher the energy level.
Each energy level or shell can be visualized as concentric circles radiating from the nucleus of the atom. Electrons fill these shells starting from the one closest to the nucleus (lowest energy state), filling up to the one furthest from the nucleus (highest energy state). This illustrates the principle of energy states in a metal as in Figure 9.13.
Furthermore, the Bohr atom model suggests that each electron orbit around the nucleus corresponds to a distinct energy level, and each transition between these levels involves a definite energy change. Therefore, the energy levels of electrons in an atom are directly related to the amount of energy possessed by the electrons.
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A battery charger used to recharge the NiMH batteries used in a digital camera can deliver as much as 0.35 A of current. If it takes 145 minutes to recharge one battery, how many g Ni(OH)2 are oxidized to NiO(OH)
Answer:
The amount that oxidized to NiO(OH) is = 1.46 gm
Explanation:
Given data
Current I = 0.35 A
Time taken = 145 min
We know that charge
Q = I t
Q = 0.35 × 145 × 60
Q = 3045 C
Faraday's constant = 96500 C
No. of moles of electron
[tex]N = \frac{3045}{96500}[/tex]
N = 0.03155
1 mol of [tex]NI(OH)_{2}[/tex] is oxidized by 2 moles of electrons, so no. of moles can be oxidized is
[tex]\frac{0.03155}{2}[/tex] = 0.015775 moles
Now convert this moles into gm by multiplying 92.708 [tex]\frac{gm}{mol}[/tex]
0.015775 × 92.708 = 1.46 gm
Therefore the amount that oxidized to NiO(OH) is = 1.46 gm
100 mL of a strong acid is completely neutralized by 100 mL of a strong base. The observed products are salt and water. Upon further investigation, the solution has a pH > 7. How is this possible?
A) The concentration of acid is the same as the concentration of the base.
B) The concentration of acid is higher than the concentration of the base.
C) The concentration of base is higher than the concentration of the acid.
D) The water autoionizes to give [OH-] ions.
Answer:
Option C. The concentration of base is higher than the concentration of the acid.
Explanation:
The reaction between a strong acid and a strong base follows the equation:
HA + OH⁻ ⇆ A⁻ + H₂O
The pH is:
[tex] pH = -log [H_3O^{+}] [/tex]
If we have 100 mL of a strong acid and 100 mL of a strong base, for the pH to be more than 7, that means that the concentration of the base is higher than the concentration of the acid. This is because, the number of moles that remains in the solution after the reaction between the acid and the base will be the moles of the base. The number of moles of the reaction above is:
[tex] n_{T} = n_{a} - n_{b} [/tex] (1)
Where na: is the moles of acid, nb: the moles of the base, and nT is the total number of moles.
Case A) If the concentration of acid is the same as the concentration of the base since the volume of the acid and the base are the same, the number of moles of acid is the same as the number of moles of the base, hence, they neutralize, so the pH = 7. This is not the correct option.
Case B) If the concentration of acid is higher than the base since the volume of the acid and the base are the same, the number of moles of acid is also higher than the number of moles of the base and the total moles in equation (1) results in an excess of moles of the acid, so the pH is < 7. This is not the correct option.
Case C) If the concentration of base is higher than the concentration of the acid since the volume of the acid and the base are the same, the number of moles of the base is also higher than the number of moles of the acid and the total moles in equation (1) results in an excess of moles of the base, so the pH is > 7. This is the correct option.
Case D) The water autoionizes to give [OH-] ions. The autoionization of the water produces the same concentration of acid that the base, so this is not the correct option.
From all of the above, the correct option is C. For the pH to be more than 7, the concentration of the base is higher than the concentration of the acid.
I hope it helps you!
Calculate the approximate volume of a 1.50 mol sample gas at 15.0°C and a pressure at 3.75atm.
Answer:
V= 9.45L
Explanation:
P=3.75atm, V=?, n= 1.5, R= 0.082, T= 15+ 273= 288K
Applying
PV= nRT
Substitute and Simplify
3.75*V= 1.5*0.082*288
V= 9.45L
The approximate volume of a 1.50 mol sample of gas at 15.0°C and a pressure of 3.75 atm is calculated using the Ideal Gas Law to be about 9.20 liters.
To calculate the approximate volume of a 1.50 mol sample of gas at 15.0°C and a pressure of 3.75 atm, we can use the Ideal Gas Law, which is PV = nRT. First, we must convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. Then we can solve for V, the volume of the gas.
The conversion from Celsius to Kelvin: T(K) = 15.0 + 273.15 = 288.15 K
Using the Ideal Gas Law constants, R = 0.0821 L·atm/K·mol. Substituting the known values into the Ideal Gas Law equation:
PV = nRT
(3.75 atm) × V = (1.50 mol) × (0.0821 L·atm/K·mol) × (288.15 K)
V = (1.50 mol × 0.0821 L·atm/K·mol × 288.15 K) / 3.75 atm
V = 9.2029 L
Therefore, the approximate volume of the gas sample is about 9.20 liters.
According to VSEPR theory, the molecule PF6- has how many regions of electron density around the central atom (how many electron groups?) (enter a number from 1 to 6) PF6- will have (linear, trigonal planar, tetrahedral, trigonal pyramidal, bent, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal, square planar) electronic geometry, and (linear, trigonal planar, tetrahedral, trigonal pyramidal, bent, trigonal bipyramidal, seesaw, T-shaped, octahedral, square pyramidal, square planar) molecular geometry.
Answer : The electronic geometry and the molecular geometry of the molecule will be octahedral.
Explanation :
Formula used :
[tex]\text{Number of electron pair}=\frac{1}{2}[V+N-C+A][/tex]
where,
V = number of valence electrons present in central atom
N = number of monovalent atoms bonded to central atom
C = charge of cation
A = charge of anion
The given molecule is, [tex]PF_6^-[/tex]
[tex]\text{Number of electrons}=\frac{1}{2}\times [5+6+1]=6[/tex]
The number of electron pair are 6 that means the hybridization will be [tex]sp^3d^2[/tex] and the electronic geometry and the molecular geometry of the molecule will be octahedral.
The correct number of regions of electron density around the central atom in PF₆- is 6. The electronic geometry of PF6- is octahedral, and the molecular geometry is also octahedral.
To determine the number of electron regions around the central phosphorus atom in PF6-, we count the bonded atoms and any lone pairs on the central atom.
The Lewis structure of PF6- shows that the phosphorus atom is bonded to six fluorine atoms and has no lone pairs since it is surrounded by six bonding groups and has a formal charge of -1, which balances the overall charge of the ion.
Each bonded fluorine contributes one region of electron density, and there are no lone pairs on the phosphorus atom.
Therefore, there are six regions of electron density around the central phosphorus atom, which corresponds to an octahedral electronic geometry.
Since there are no lone pairs, the molecular geometry is the same as the electronic geometry, which is octahedral. This means that all six fluorine atoms are arranged around the central phosphorus atom in a way that they are at the vertices of an octahedron.
In summary, the VSEPR theory predicts that PF6- has six regions of electron density, an octahedral electronic geometry, and an octahedral molecular geometry.
Think about what you've learned about how particle motion is related to temperature.
Select all of the statements that are true.
1. The average kinetic energy of the particles in a substance determines the
substance's temperature.
2. If the particles in two pure substances have the same average speed, the
substances can have different temperatures.
3. When two substances have the same temperature, all of the particles in
both substances are moving at the same speed.
4. How fast a substance's particles are moving determines how hot or cold
the substance is.
Final answer:
The true statements about particle motion and temperature are that the average kinetic energy of the particles in a substance determines its temperature and that faster moving particles generally result in a higher temperature of the substance.
Explanation:
The relationship between particle motion and temperature is based on the kinetic-molecular theory. According to this theory, temperature is proportional to the average kinetic energy of the particles, such as molecules or atoms, in a substance. Therefore:
The average kinetic energy of the particles in a substance determines the substance's temperature.
If the particles in two pure substances have the same average speed, it does not necessarily mean they have the same temperature, since heavier particles will have more kinetic energy at the same speed, leading to different temperatures.
When two substances have the same temperature, it indicates that the average kinetic energy of the particles in both substances is the same, not that all of the particles are moving at the same speed, because particles have a range of speeds.
The speed of a substance's particles can give an indication of how hot or cold that substance is. Faster moving particles generally mean a higher temperature.
As such, the true statements are 1 and 4. Understanding that temperature is not simply a measure of particle speed, but rather the average kinetic energy involved, clarifies misconceptions about the nature of thermal energy and its measurement.
Qualitative measurements involve numerical measurements while quantitative measurements record descriptions.
Question 5 options:
True
False
Beyond simple thermal decomposition, an even more effective means of obtaining energy from NH4ClO4(s) \rm NH_4ClO_4(s) is to mix this oxidizer with a fuel. When NH4ClO4(s) is employed in solid-fuel booster rockets, it is packed with powdered aluminum. The powdered aluminum is the fuel, and the ammonium perchlorate is the oxidizer. Two of the reactions occurring on ignition are
6NH4ClO4(s)+10Al(s)2NH4ClO4(s)+2Al(s)??5Al2O3(s)+6HCl(g)+9H2O(g)+3N2(g),?H1=?4392.5 kJ
Al2O3(s)+2HCl(g)+3H2O(g)+2NO(g),?H2=?1172.6 k
Which of the following statements are correct?
Check all that apply.
a.All nitrogen atoms lose three electrons in both reactions.
b.Chlorine is reduced from + +7 to ? -1 in both reactions.
c.Reaction 2 produces more energy per gram of Al \rm Al.
d.The thrust produced by the formation of gaseous products is greater per mole of ammonium perchlorate in Reaction 2.
Final answer:
Only statement b, which says that chlorine is reduced from +7 to -1 in both reactions, is correct. Statements a, c, and d cannot be confirmed as correct based on the given information.
Explanation:
The student has presented two chemical reaction equations involving the thermal decomposition of NH4ClO4 (ammonium perchlorate) and powdered aluminum. Let's address the statements provided:
a. All nitrogen atoms lose three electrons in both reactions. This statement is incorrect. In the provided reactions, nitrogen goes from an oxidation state of -3 in NH4+ to 0 in N2, which means each nitrogen atom gains three electrons.
b. Chlorine is reduced from +7 to -1 in both reactions. This statement is correct. In NH4ClO4, chlorine starts with an oxidation state of +7 and is reduced to -1 in HCl.
c. Reaction 2 produces more energy per gram of Al. Without details of the mass of aluminum involved in Reaction 2, we cannot determine which reaction produces more energy per gram of aluminum. However, if the reactions involve the same mass of aluminum, then Reaction 1 is more energetic since the absolute value of ΔH is greater.
d. The thrust produced by the formation of gaseous products is greater per mole of ammonium perchlorate in Reaction 2. This statement cannot be evaluated without more information about the moles of gaseous products formed in Reaction 2.
Therefore, based on the information provided, the correct statement is b. Chlorine is reduced from +7 to -1 in both reactions.
What is the temperature of CO2 gas if the average speed (actually the root-mean-square speed) of the molecules is 750 m/s?
Answer:
992.302 K
Explanation:
V(rms) = 750 m/s
V(rms) = √(3RT / M)
V = velocity of the gas
R = ideal gas constant = 8.314 J/mol.K
T = temperature of the gas
M = molar mass of the gas
Molar mass of CO₂ = [12 + (16*2)] = 12+32 = 44g/mol
Molar mass = 0.044kg/mol
From
½ M*V² = 3 / 2 RT
MV² = 3RT
K = constant
V² = 3RT / M
V = √(3RT / M)
So, from V = √(3RT / M)
V² = 3RT / M
V² * M = 3RT
T = (V² * M) / 3R
T = (750² * 0.044) / 3 * 8.314
T = 24750000 / 24.942
T = 992.302K
The temperature of the gas is 992.302K
Note : molar mass of the gas was converted from g/mol to kg/mol so the value can change depending on whichever one you use.
The temperature of a gas can be calculated from the root-mean-square speed of its molecules using the kinetic theory of gases. For CO2 gas with the rms speed of 750 m/s, the derived temperature is approximately 485.4 K.
Explanation:The temperature of a gas can be calculated from the root-mean-square (rms) speed of its molecules using the kinetic theory of gases. This theory develops a relationship between the average kinetic energy of the gas molecules and the temperature of the gas through the equation K = 3/2kBT = mv²/2, where kB is Boltzmann’s constant, T is the temperature, m is the mass of a gas molecule, and v is the rms speed. Thus, temperature can be derived as T = mv² / (3kB).
For CO2, the molar mass is 0.044 kg/mol. Knowing that the number of molecules (n) is the number of moles times Avogadro's number (6.022 × 10²³), we derive the molecular mass m = 0.044 kg/mol / (6.022 × 10²³) = 7.3 × 10^-26 kg. Plugging in the values for v (750 m/s), m, and kB (1.38 × 10^-23 J/K), we get an approximate temperature of 485.4 K.
Learn more about rms speed here:https://brainly.com/question/33262591
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you need to prepare 250.0 mL of a 1.50 M HCl solution from a 2.00 M HCl stock solution. assuming that the accuracy of the concentration is important, which type of glassware should you use to make the solution
Answer:
I should use a volumetric flask.
Explanation:
If the accuracy of the concentration is important, we need to use a volumetric flask.
Answer:
The glassware appropriate for dilution preparation is a (250 mL) volumetric flask
Explanation:
We know that molarity or concentration of a solution is the number of moles per litres of solution, the molarity and volume of the solution in question can be used to find out how much of the stock solution to be diluted using the formula;
[tex]c = \frac{n}{v}[/tex]
Once the variables are confirmed, a 250 mL solution of 1.50M HCl can be prepared by measuring determined stock solute into a 250mL volumetric flask and the making it upto the 250mL mark. (a measuring cylinder can be used to check accuracy of volume added).
Nitrogen and hydrogen gases are combined at high temperatures and pressures to produce ammonia, NH3. If 101.7 g of N2 are reacted with excess H2, how many moles of NH3 will be formed
Answer:
7.26 moles of NH₃ are formed in this reaction
Explanation:
This is about the reaction for the production of ammonia
1 mol of nitrogen gas reacts to 3 moles of hydrogen in order to produce 2 moles of ammonia.
The equation is: N₂ + 3H₂ → 2NH₃
In the question, we were informed that the excess is the H₂ so the N₂ is limiting reagent. We determine the moles, that has reacted:
101.7 g / 28 g/mol = 3.63 moles
So, If 1 mol of nitrogen gas can produce 2 moles of ammonia
3.63 moles of N₂ must produce ( 2 . 3.63) / 1 = 7.26 moles of NH₃
Answer:
In this reaction, 7.26 moles of NH3 will be formed.
Explanation:
Step 1: Data given
Mass of N2 = 101.7 grams
Molar mass N2 = 28.0 g/mol
H2 is in excess
Molar mass H2 = 2.02 g/mol
Molar mass of NH3 = 17.03 g/mol
Step 2: The balanced equation
N2(g) + 3H2(g) → 2NH3(g)
Step 3: Calculate moles N2
Moles N2 = mass N2/ molar mass N2
Moles N2 = 101.7 grams / 28.0 g/mol
Moles N2 = 3.63 moles
Step 4: Calculate moles NH3
For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3
For 3.63 moles N2 we'll produce2*3.63 = 7.26 moles NH3
In this reaction, 7.26 moles of NH3 will be formed.
2K + 2HBr → 2 KBr + H2
When 5.5moles of K reacts with 4.04moles of HBr, to produce Hydrogen gas(H₂)
●a). What is the limiting reactant?
●b.)What is the excess reactant?
2K + 2HBr → 2 KBr + H2
When 5.5moles of K reacts with 4.04moles of HBr, to produce Hydrogen gas(H₂)
●a). What is the limiting reactant?
●b.)What is the excess reactant?
2K + 2HBr → 2 KBr + H2
When 5.5moles of K reacts with 4.04moles of HBr, to produce Hydrogen gas(H₂)
●a). What is the limiting reactant?
●b.)What is the excess reactant?
●C.)How much product is produced?
Answer:
[tex]\large \boxed{\text{a) HBr; b) K; c) 0.0503 g}}[/tex]
Explanation:
The limiting reactant is the reactant that gives the smaller amount of product.
Assemble all the data in one place, with molar masses above the formulas and masses below them.
M_r: 39.10 80.41 2.016
2K + 2HBr ⟶ 2KBr + H₂
m/g: 5.5 4.04
a) Limiting reactant
(i) Calculate the moles of each reactant
[tex]\text{Moles of K} = \text{5.5 g} \times \dfrac{\text{1 mol}}{\text{31.10 g}} = \text{0.141 mol K}\\\\\text{Moles of HBr} = \text{4.04 g} \times \dfrac{\text{1 mol}}{\text{80.91 g}} = \text{0.049 93 mol HBr}[/tex]
(ii) Calculate the moles of H₂ we can obtain from each reactant.
From K:
The molar ratio of H₂:K is 1:2.
From HBr:
The molar ratio of H₂:HBr is 3:2.
[tex]\text{Moles of H}_{2} = \text{0.049 93 mol HBr } \times \dfrac{\text{1 mol H}_{2}}{\text{2 mol HBr}} = \text{0.024 97 mol H}_{2}[/tex]
(iii) Identify the limiting reactant
HBr is the limiting reactant because it gives the smaller amount of NH₃.
b) Excess reactant
The excess reactant is K.
c) Mass of H₂
[tex]\text{Mass of H}_{2} = \text{0.024 97 mol H}_{2} \times \dfrac{\text{2.016 g H}_{2}}{\text{1 mol H}_{2}} = \textbf{0.0503 g H}_{2}\\\text{The mass of hydrogen is $\large \boxed{\textbf{0.0503 g}}$}[/tex]
A solution is to be prepared with a sodium ion concentration of 0.513 mol/L. What mass of sodium sulfate (g) is needed to prepare 1.98 liters of such a solution? Do not enter units with your answer.
Answer:
We should weigh 72.1 of sodium sulfate
Explanation:
The solution must be made of sodium sulfate. This salt can be dissociated like this:
Na₂SO₄ → 2Na⁺ + SO₄⁻²
From this dissociation we can say that, 2 moles of sodium cation are obtained from 1 mol of salt.
Therefore 0.513 moles of sodium cation will be obtained from 0.2565 moles of salt (0.513 . 1) / 2. The thing is that this number are the moles contained in 1 L of solution, and we need to prepare such 1.98 L
Molarity = mol / Volume (L) → Molarity . volume (L) = mol
0.2565 mol/L . 1.98L = 0.508 moles
These are the moles we should weigh. Let's convert them to moles:
0.508 mol . 142.06 g / 1 mol = 72.1 g
Answer:
We need 72.1 grams of Na2SO4
Explanation:
Step 1: Data given
sodium ion concentration = 0.513 mol/L
Volume = 1.98 L
Step 2: The balanced equation
Na2SO4 → 2Na+ + SO4^2-
Step 3: Calculate moles Na+
Moles Na+ = molarity Na+ * volume
Moles Na+ = 0.513 * 1.98 L
Moles Na+ = 1.01574 moles
Step 4: Calculate moles Na2SO4
For 1 mol Na2SO4 we need 2 moles Na+ and 1 mol SO4^2-
For 1.01574 moles Na+ we'll need 1.01574/2 = 0.50787 moles Na2SO4
Step 5: Calculate moles Na2SO4
Mass Na2SO4 = moles Na2SO4 * molar mass Na2SO4
Mass Na2SO4 = 0.50787 moles * 142.04 g/mol
Mass Na2SO4 = 72.1 grams
We need 72.1 grams of Na2SO4