Question 1

If a reaction  0, then when the reaction is at equilibrium there will be ________ A) absolutely no B that is formed. B) smaller quantities of B and larger quantities of A. C) equal quantities of A and B. D) large quantities of B and smaller quantities of A. E) absolutely no A remaining." class="answers-bank-image d-inline" rel="preload" > has  0, then when the reaction is at equilibrium there will be ________ A) absolutely no B that is formed. B) smaller quantities of B and larger quantities of A. C) equal quantities of A and B. D) large quantities of B and smaller quantities of A. E) absolutely no A remaining." class="answers-bank-image d-inline" rel="preload" >  0, then when the reaction is at equilibrium there will be ________

Accepted Answer

A)  absolutely no B that is formed.
B)  smaller quantities of B and larger quantities of A.
C)  equal quantities of A and B.
D)  large quantities of B and smaller quantities of A.
E)  absolutely no A remaining.

Question 2

Indicate which of the following has the highest entropy at 298 K.

Accepted Answer

A)  0.5 g of HCN
B)  1 mol of HCN
C)  2 kg of HCN
D)  2 mol of HCN
E)  All of the above have the same entropy at 298 K.

Question 3

The standard molar entropy of lead(II)  bromide (PbBr2)  is 161 J/(mol  K) . What is the entropy of 2.45 g of PbBr2?

Accepted Answer

A)  (1.07 J/K) 
B)  (1.07 J/K) 
C)  (161 J/K) 
D)  (161 J/K) 
E)  0 J/K

Question 4

What is the standard entropy change when 10.0 g of methane reacts with 10.0 g of oxygen?

Accepted Answer

<font face="symbol">F...

Question 5

When plotting ln K vs. 1/T, a linear relationship is obtained ________

Accepted Answer

A)  with a slope of H /R and an intercept of S/R.
B)  with a slope of H /R and an intercept of S/R.
C)  with a slope of H /R and an intercept of S/R.
D)  with a slope of H /R and an intercept of S/R.
E)  never, because logarithmic relationships are intrinsically nonlinear.

Question 6

The symbol     (CH3OH, l)  refers to which of the following reactions? A)    B)        C)        D)    E)   " class="answers-bank-image d-inline" rel="preload" > (CH3OH, l)  refers to which of the following reactions?

Accepted Answer

A)      (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)      (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >    (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >    (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)      (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >    (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >    (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)      (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)      (CH3OH, l)  refers to which of the following reactions? 
A)     
B)         
C)         
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >

Question 7

Noxious NO gas can form from N2 and O2 gases in automobile engines at high temperatures. If the value of the equilibrium constant, Kc, for this reaction at 25C is 1.95  1031, what is the value at 2,000C? 2 and O2 gases in automobile engines at high temperatures. If the value of the equilibrium constant, Kc, for this reaction at 25C is 1.95  1031, what is the value at 2,000C?       Thermodynamic Properties of Nitrogen Monoxide     S87.6 kJ/mol 90.3 kJ/mol 211 J/(mol  K)  A) 2.8  103 B) 3.7  102 C) 6.9  102 D) 6.2  104 E) 1.7  106" class="answers-bank-image d-inline" rel="preload" > 2 and O2 gases in automobile engines at high temperatures. If the value of the equilibrium constant, Kc, for this reaction at 25C is 1.95  1031, what is the value at 2,000C?       Thermodynamic Properties of Nitrogen Monoxide     S87.6 kJ/mol 90.3 kJ/mol 211 J/(mol  K)  A) 2.8  103 B) 3.7  102 C) 6.9  102 D) 6.2  104 E) 1.7  106" class="answers-bank-image d-inline" rel="preload" > 2 and O2 gases in automobile engines at high temperatures. If the value of the equilibrium constant, Kc, for this reaction at 25C is 1.95  1031, what is the value at 2,000C?       Thermodynamic Properties of Nitrogen Monoxide     S87.6 kJ/mol 90.3 kJ/mol 211 J/(mol  K)  A) 2.8  103 B) 3.7  102 C) 6.9  102 D) 6.2  104 E) 1.7  106" class="answers-bank-image d-inline" rel="preload" > Thermodynamic Properties of Nitrogen Monoxide 2 and O2 gases in automobile engines at high temperatures. If the value of the equilibrium constant, Kc, for this reaction at 25C is 1.95  1031, what is the value at 2,000C?       Thermodynamic Properties of Nitrogen Monoxide     S87.6 kJ/mol 90.3 kJ/mol 211 J/(mol  K)  A) 2.8  103 B) 3.7  102 C) 6.9  102 D) 6.2  104 E) 1.7  106" class="answers-bank-image d-inline" rel="preload" > 2 and O2 gases in automobile engines at high temperatures. If the value of the equilibrium constant, Kc, for this reaction at 25C is 1.95  1031, what is the value at 2,000C?       Thermodynamic Properties of Nitrogen Monoxide     S87.6 kJ/mol 90.3 kJ/mol 211 J/(mol  K)  A) 2.8  103 B) 3.7  102 C) 6.9  102 D) 6.2  104 E) 1.7  106" class="answers-bank-image d-inline" rel="preload" > S87.6 kJ/mol 90.3 kJ/mol
211 J/(mol  K)

Accepted Answer

A)  2.8  103
B)  3.7  102
C)  6.9  102
D)  6.2  104
E)  1.7  106

Question 8

If for a given chemical reaction at 298 K, the change in free energy, G, is positive and the change in the standard free energy, G , is negative, then ________

Accepted Answer

A)  Q  K and product is turning back into reactant.
B)  Q  K and more product is being produced.
C)  Q  K and product is turning back into reactant.
D)  Q  K and more product is being produced.
E)  Q  K and the reaction has stopped.

Question 9

Of the three modes of molecular motion-vibration, rotation, and translation-which requires the greatest amount of energy to cause an excitation from the ground state to the first excited state?

Accepted Answer

A)  vibration
B)  rotation
C)  translation
D)  They all require the same amount of energy.
E)  None, because quantized energy states do not apply to these motions.

Question 10

Determine     for       given the following information:   A) (41.10 J/K)  B) (165.29 J/K)  C) (398.75 J/K)  D) (165.29 J/K)  E) (41.10 J/K) " class="answers-bank-image d-inline" rel="preload" > for    for       given the following information:   A) (41.10 J/K)  B) (165.29 J/K)  C) (398.75 J/K)  D) (165.29 J/K)  E) (41.10 J/K) " class="answers-bank-image d-inline" rel="preload" >    for       given the following information:   A) (41.10 J/K)  B) (165.29 J/K)  C) (398.75 J/K)  D) (165.29 J/K)  E) (41.10 J/K) " class="answers-bank-image d-inline" rel="preload" >    for       given the following information:   A) (41.10 J/K)  B) (165.29 J/K)  C) (398.75 J/K)  D) (165.29 J/K)  E) (41.10 J/K) " class="answers-bank-image d-inline" rel="preload" > given the following information:    for       given the following information:   A) (41.10 J/K)  B) (165.29 J/K)  C) (398.75 J/K)  D) (165.29 J/K)  E) (41.10 J/K) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  (41.10 J/K) 
B)  (165.29 J/K) 
C)  (398.75 J/K) 
D)  (165.29 J/K) 
E)  (41.10 J/K)

Question 11

Which of the following must be true for the microstates of a system?
I.The energy of each microstate equals the energy of the system.
II.The entropy of each microstate equals the entropy of the system.
III.The number of microstates equals the entropy of the system.

Accepted Answer

A)  I only
B)  II only
C)  III only
D)  I and III only
E)  I, II, and III are all true.

Question 12

A chemist is planning to study a chemical equilibrium for which no measured explicit thermodynamic values are available. However, the reaction involves common chemical species. What information could a chemist use to make predictions about the equilibrium?

Accepted Answer

A)  equilibrium constants for the equilibrium reactions that can be combined to make the new equilibrium
B)   (Hf and S values for the reactants and products of the new reaction)  
D)  all of the above" class="answers-bank-image d-inline" rel="preload" > values for the reactants and products of the new reaction) 
C)  (Hf and S values for the reactants and products of the new reaction) 
D)  all of the above

Question 13

Before class, students were distributed throughout a classroom. When the bell rang, all the students sat down at three tables in the center of the room. The entropy of the class ________

Accepted Answer

A)  increased.
B)  decreased.
C)  remained the same.
D)  cannot be determined.
E)  is irrelevant.

Question 14

Jane can accept that G  RT ln K, but she cannot reconcile the relationship between S and ln K. Please explain it to her.

Accepted Answer

A)  (S  R ln K  H /T) 
B)  (S  ln (K/R)   H /T) 
C)  (S  R ln (K/T)   H ) 
D)  (S  R ln (K)   H /T) 
E)  (S  R ln (K)   H /T)

Question 15

The standard entropy of N2(g) is 191.5 J/mol F1F1F1S1F1F1F10 K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

Accepted Answer

S_molecule  191.5 J/mol ...

Question 16

For the following exothermic reaction, predict under which conditions the reaction will be spontaneous.

Accepted Answer

A)  The reaction is always spontaneous.
B)  The reaction is never spontaneous.
C)  The reaction is spontaneous at high temperatures.
D)  The reaction is spontaneous at low temperatures.
E)  Insufficient data is provided to answer this question.

Question 17

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2,000 K. Substance  (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6       A) 2.04  107 B) 5.44  1014 C) 2.67  108 D) 2.91  109 E) 3.65  1012" class="answers-bank-image d-inline" rel="preload" > (kJ/mol)   (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6       A) 2.04  107 B) 5.44  1014 C) 2.67  108 D) 2.91  109 E) 3.65  1012" class="answers-bank-image d-inline" rel="preload" > (kJ/mol)  S (J/mol · K) 
O2(g)  0 0 205.0
O3(g)  142.3 163.4 237.6  (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6       A) 2.04  107 B) 5.44  1014 C) 2.67  108 D) 2.91  109 E) 3.65  1012" class="answers-bank-image d-inline" rel="preload" >  (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6       A) 2.04  107 B) 5.44  1014 C) 2.67  108 D) 2.91  109 E) 3.65  1012" class="answers-bank-image d-inline" rel="preload" >  (J/mol · K)  O2(g)  0 0 205.0 O3(g)  142.3 163.4 237.6       A) 2.04  107 B) 5.44  1014 C) 2.67  108 D) 2.91  109 E) 3.65  1012" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  2.04  107
B)  5.44  1014
C)  2.67  108
D)  2.91  109
E)  3.65  1012

Question 18

Values for F1F1F1S1F1F1F10HF1F1F1S1F1F1F10 and F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 for a reaction can be determined experimentally by fitting a linear equation to a plot of ________ on the x-axis and ________ on the y-axis. The slope of this equation is equal to ________ and the intercept allows us to calculate ________.

Accepted Answer

1/T; ln K; <font face="symbol">...

Question 19

Determine      given the following information:   A) (2,705 kJ)  B) (608.0 kJ)  C) (1,791 kJ)  D) (3,457 kJ)  E) (608.0 kJ) " class="answers-bank-image d-inline" rel="preload" >       given the following information:   A) (2,705 kJ)  B) (608.0 kJ)  C) (1,791 kJ)  D) (3,457 kJ)  E) (608.0 kJ) " class="answers-bank-image d-inline" rel="preload" >      given the following information:   A) (2,705 kJ)  B) (608.0 kJ)  C) (1,791 kJ)  D) (3,457 kJ)  E) (608.0 kJ) " class="answers-bank-image d-inline" rel="preload" > given the following information:      given the following information:   A) (2,705 kJ)  B) (608.0 kJ)  C) (1,791 kJ)  D) (3,457 kJ)  E) (608.0 kJ) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  (2,705 kJ) 
B)  (608.0 kJ) 
C)  (1,791 kJ) 
D)  (3,457 kJ) 
E)  (608.0 kJ)

Question 20

When you increase the volume of a gas, the energy separation between microstates ________

Accepted Answer

A)  increases.
B)  decreases.
C)  remains unchanged.
D)  becomes infinite.
E)  disappears.

Exam 17: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Values for H and S for a reaction can be determined experimentally by fitting a linear equation to a plot of on the x-axis and on the y-axis. The slope of this equation is equal to and the intercept allows us to calculate .

Correct Answer
verified
1/T; ln K; ...
View Answer

Determine given the following information:

Correct Answer
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Correct Answer
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When you increase the volume of a gas, the energy separation between microstates ________

Correct Answer
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Of the three modes of molecular motion-vibration, rotation, and translation-which requires the greatest amount of energy to cause an excitation from the ground state to the first excited state?

Correct Answer
verified

Indicate which of the following has the highest entropy at 298 K.

Correct Answer
verified

Which of the following must be true for the microstates of a system? I.The energy of each microstate equals the energy of the system. II.The entropy of each microstate equals the entropy of the system. III.The number of microstates equals the entropy of the system.

Correct Answer
verified

What is the standard entropy change when 10.0 g of methane reacts with 10.0 g of oxygen?

Correct Answer
verified
F...
View Answer

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2,000 K. Substance (kJ/mol) (kJ/mol) S (J/mol · K) O₂(g) 0 0 205.0 O₃(g) 142.3 163.4 237.6

Correct Answer
verified

If a reaction has  0, then when the reaction is at equilibrium there will be ________

Correct Answer
verified

Determine  for given the following information:

Correct Answer
verified

A chemist is planning to study a chemical equilibrium for which no measured explicit thermodynamic values are available. However, the reaction involves common chemical species. What information could a chemist use to make predictions about the equilibrium?

Correct Answer
verified

The standard entropy of N₂(g) is 191.5 J/mol  K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

Correct Answer
verified
S_molecule  191.5 J/mol ...
View Answer

For the following exothermic reaction, predict under which conditions the reaction will be spontaneous.

Correct Answer
verified

Jane can accept that G  RT ln K, but she cannot reconcile the relationship between S and ln K. Please explain it to her.

Correct Answer
verified

If for a given chemical reaction at 298 K, the change in free energy, G, is positive and the change in the standard free energy, G , is negative, then ________

Correct Answer
verified

Before class, students were distributed throughout a classroom. When the bell rang, all the students sat down at three tables in the center of the room. The entropy of the class ________

Correct Answer
verified

The standard molar entropy of lead(II) bromide (PbBr₂) is 161 J/(mol  K) . What is the entropy of 2.45 g of PbBr₂?

Correct Answer
verified

When plotting ln K vs. 1/T, a linear relationship is obtained ________

Correct Answer
verified

The symbol  (CH₃OH, l) refers to which of the following reactions?

Correct Answer
verified

Exam 17: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Values for H and S for a reaction can be determined experimentally by fitting a linear equation to a plot of ________ on the x-axis and ________ on the y-axis. The slope of this equation is equal to ________ and the intercept allows us to calculate ________.

Correct Answerverified1/T; ln K; ...View AnswerShow Answer

Determine given the following information:

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

When you increase the volume of a gas, the energy separation between microstates ________

Correct AnswerverifiedShow Answer

Of the three modes of molecular motion-vibration, rotation, and translation-which requires the greatest amount of energy to cause an excitation from the ground state to the first excited state?

Correct AnswerverifiedShow Answer

Indicate which of the following has the highest entropy at 298 K.

Correct AnswerverifiedShow Answer

Which of the following must be true for the microstates of a system? I.The energy of each microstate equals the energy of the system. II.The entropy of each microstate equals the entropy of the system. III.The number of microstates equals the entropy of the system.

Correct AnswerverifiedShow Answer

What is the standard entropy change when 10.0 g of methane reacts with 10.0 g of oxygen?

Correct AnswerverifiedF...View AnswerShow Answer

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2,000 K. Substance (kJ/mol) (kJ/mol) S (J/mol · K) O2(g) 0 0 205.0 O3(g) 142.3 163.4 237.6

Correct AnswerverifiedShow Answer

If a reaction has  0, then when the reaction is at equilibrium there will be ________

Correct AnswerverifiedShow Answer

Determine  for given the following information:

Correct AnswerverifiedShow Answer

A chemist is planning to study a chemical equilibrium for which no measured explicit thermodynamic values are available. However, the reaction involves common chemical species. What information could a chemist use to make predictions about the equilibrium?

Correct AnswerverifiedShow Answer

The standard entropy of N2(g) is 191.5 J/mol  K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

Correct AnswerverifiedSmolecule  191.5 J/mol ...View AnswerShow Answer

For the following exothermic reaction, predict under which conditions the reaction will be spontaneous.

Correct AnswerverifiedShow Answer

Jane can accept that G  RT ln K, but she cannot reconcile the relationship between S and ln K. Please explain it to her.

Correct AnswerverifiedShow Answer

If for a given chemical reaction at 298 K, the change in free energy, G, is positive and the change in the standard free energy, G , is negative, then ________

Correct AnswerverifiedShow Answer

Before class, students were distributed throughout a classroom. When the bell rang, all the students sat down at three tables in the center of the room. The entropy of the class ________

Correct AnswerverifiedShow Answer

The standard molar entropy of lead(II) bromide (PbBr2) is 161 J/(mol  K) . What is the entropy of 2.45 g of PbBr2?

Correct AnswerverifiedShow Answer

When plotting ln K vs. 1/T, a linear relationship is obtained ________

Correct AnswerverifiedShow Answer

The symbol  (CH3OH, l) refers to which of the following reactions?

Correct AnswerverifiedShow Answer

Values for H and S for a reaction can be determined experimentally by fitting a linear equation to a plot of on the x-axis and on the y-axis. The slope of this equation is equal to and the intercept allows us to calculate .

Correct Answer
verified
1/T; ln K; ...
View Answer

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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F...
View Answer

Using the thermodynamic data below, determine the equilibrium constant for the conversion of oxygen to ozone at 2,000 K. Substance (kJ/mol) (kJ/mol) S (J/mol · K) O₂(g) 0 0 205.0 O₃(g) 142.3 163.4 237.6

Correct Answer
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Correct Answer
verified

Correct Answer
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Correct Answer
verified

The standard entropy of N₂(g) is 191.5 J/mol  K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

Correct Answer
verified
S_molecule  191.5 J/mol ...
View Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The standard molar entropy of lead(II) bromide (PbBr₂) is 161 J/(mol  K) . What is the entropy of 2.45 g of PbBr₂?

Correct Answer
verified

Correct Answer
verified

The symbol  (CH₃OH, l) refers to which of the following reactions?

Correct Answer
verified