Question 1

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

Accepted Answer

A) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
B) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
C) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
D) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
E) never, because logarithmic relationships are intrinsically nonlinear. 
A) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
B) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
C) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
D) with a slope of F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/R and an intercept of F1F1F1S1F1F1F10SF1F1F1S1F1F1F10/R. 
E) never, because logarithmic relationships are intrinsically nonlinear.

Question 2

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

Question 3

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. 
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 4

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

Question 5

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. 
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 6

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)  (  values for the reactants and products of the new reaction) 
C) (F1F1F1S1F1F1F10Hf and SF1F1F1S1F1F1F10 values for the reactants and products of the new reaction) 
D) all of the above 
A) equilibrium constants for the equilibrium reactions that can be combined to make the new equilibrium 
B)  (  values for the reactants and products of the new reaction) 
C) (F1F1F1S1F1F1F10Hf and SF1F1F1S1F1F1F10 values for the reactants and products of the new reaction) 
D) all of the above

Question 7

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 F1F1F1S1F1F1F10 191.5 J/mol F1F1F1S1

Question 8

Determine F1F1F1S1F1F1F10F1F1F1S1F1F1F10   for       given the following information:

Accepted Answer

A) (F1F1F1S1F1F1F1041.10 J/K) 
B) (F1F1F1S1F1F1F10165.29 J/K) 
C) (F1F1F1S1F1F1F10398.75 J/K) 
D) (F1F1F1S1F1F1F10165.29 J/K) 
E) (F1F1F1S1F1F1F1041.10 J/K) 
A) (F1F1F1S1F1F1F1041.10 J/K) 
B) (F1F1F1S1F1F1F10165.29 J/K) 
C) (F1F1F1S1F1F1F10398.75 J/K) 
D) (F1F1F1S1F1F1F10165.29 J/K) 
E) (F1F1F1S1F1F1F1041.10 J/K)

Question 9

Determine   F1F1F1S1F1F1F10     given the following information:

Accepted Answer

A) (F1F1F1S1F1F1F102,705 kJ) 
B) (F1F1F1S1F1F1F10608.0 kJ) 
C) (F1F1F1S1F1F1F101,791 kJ) 
D) (F1F1F1S1F1F1F103,457 kJ) 
E) (F1F1F1S1F1F1F10608.0 kJ) 
A) (F1F1F1S1F1F1F102,705 kJ) 
B) (F1F1F1S1F1F1F10608.0 kJ) 
C) (F1F1F1S1F1F1F101,791 kJ) 
D) (F1F1F1S1F1F1F103,457 kJ) 
E) (F1F1F1S1F1F1F10608.0 kJ)

Question 10

Jane can accept that F1F1F1S1F1F1F10GF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10RT ln K, but she cannot reconcile the relationship between F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 and ln K. Please explain it to her.

Accepted Answer

A) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 R ln K F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T) 
B) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10ln (K/R) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T) 
C) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10R ln (K/T) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10) 
D) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10R ln (K) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T) 
E) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10R ln (K) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T) 
A) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 R ln K F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T) 
B) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10ln (K/R) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T) 
C) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10R ln (K/T) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10) 
D) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10R ln (K) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T) 
E) (F1F1F1S1F1F1F10SF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F10R ln (K) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10H F1F1F1S1F1F1F10/T)

Question 11

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) SF1F1F1S1F1F1F10 (J/mol · K)
O2(g) 0 0 205.0
O3(g) 142.3 163.4 237.6

Accepted Answer

A) 2.04 F1F1F1S1F1F1F10 107 
B) 5.44 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 
C) 2.67 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 
D) 2.91 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 
E) 3.65 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012 
A) 2.04 F1F1F1S1F1F1F10 107 
B) 5.44 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 
C) 2.67 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 
D) 2.91 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 
E) 3.65 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012

Question 12

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 25F1F1F1S1F1F1F10C is 1.95 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1031, what is the value at 2,000F1F1F1S1F1F1F10C?       Thermodynamic Properties of Nitrogen Monoxide     SF1F1F1S1F1F1F1087.6 kJ/mol 90.3 kJ/mol
211 J/(mol F1F1F1S1F1F1F10 K)

Accepted Answer

A) 2.8 F1F1F1S1F1F1F10 103 
B) 3.7 F1F1F1S1F1F1F10 102 
C) 6.9 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 
D) 6.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
E) 1.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
A) 2.8 F1F1F1S1F1F1F10 103 
B) 3.7 F1F1F1S1F1F1F10 102 
C) 6.9 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102 
D) 6.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
E) 1.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106

Question 13

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

Accepted Answer

F1F1F1S1F

Question 14

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

Question 15

The symbol F1F1F1S1F1F1F10F1F1F1S1F1F1F10   (CH3OH, l) refers to which of the following reactions?

Accepted Answer

A)    
B)        
C)        
D)    
E)    
A)    
B)        
C)        
D)    
E)

Question 16

The standard molar entropy of lead(II) bromide (PbBr2) is 161 J/(mol F1F1F1S1F1F1F10 K). What is the entropy of 2.45 g of PbBr2?

Accepted Answer

A) (F1F1F1S1F1F1F101.07 J/K) 
B) (F1F1F1S1F1F1F101.07 J/K) 
C) (F1F1F1S1F1F1F10161 J/K) 
D) (F1F1F1S1F1F1F10161 J/K) 
E) 0 J/K 
A) (F1F1F1S1F1F1F101.07 J/K) 
B) (F1F1F1S1F1F1F101.07 J/K) 
C) (F1F1F1S1F1F1F10161 J/K) 
D) (F1F1F1S1F1F1F10161 J/K) 
E) 0 J/K

Question 17

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. 
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 18

If for a given chemical reaction at 298 K, the change in free energy, F1F1F1S1F1F1F10G, is positive and the change in the standard free energy, F1F1F1S1F1F1F10G F1F1F1S1F1F1F10, is negative, then ________

Accepted Answer

A) Q F1F1F1S1F1F1F10 K and product is turning back into reactant. 
B) Q F1F1F1S1F1F1F10 K and more product is being produced. 
C) Q F1F1F1S1F1F1F10 K and product is turning back into reactant. 
D) Q F1F1F1S1F1F1F10 K and more product is being produced. 
E) Q F1F1F1S1F1F1F10 K and the reaction has stopped. 
A) Q F1F1F1S1F1F1F10 K and product is turning back into reactant. 
B) Q F1F1F1S1F1F1F10 K and more product is being produced. 
C) Q F1F1F1S1F1F1F10 K and product is turning back into reactant. 
D) Q F1F1F1S1F1F1F10 K and more product is being produced. 
E) Q F1F1F1S1F1F1F10 K and the reaction has stopped.

Question 19

If a reaction   has   F1F1F1S1F1F1F10 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. 
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 20

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; F1F1F1S1

Exam 17: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

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

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.

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?

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 ________

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

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?

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.

Determine  for given the following information:

Determine given the following information:

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

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

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

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

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

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

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

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 ________

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

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 ________.

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

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.

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

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

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

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 .