Question 1

State the second and third laws of thermodynamics.

Accepted Answer

All spontaneous processes are

Question 2

What term is given to the fact that the entropy of a perfect crystalline solid is zero at absolute zero?

Accepted Answer

A)  1st law of thermodynamics 
B)  2nd law of thermodynamics 
C)  3rd law of thermodynamics 
D)  crystalline lattice theory 
E)  absolute crystallinity 
A)  1st law of thermodynamics 
B)  2nd law of thermodynamics 
C)  3rd law of thermodynamics 
D)  crystalline lattice theory 
E)  absolute crystallinity

Question 3

The complete combustion of liquid benzene is represented by the equation:
C6H6(l) + 7   O2(g) → 6CO2(g) + 3H2O(l)
Using the data below, calculate, for this reaction
a. ΔH°
b. ΔG° at 25°C.

Accepted Answer

a. -3271 k

Question 4

For a chemical reaction to be spontaneous at all temperatures, which conditions must be met?

Accepted Answer

A)  ΔS°rxn > 0, ΔH°rxn > 0 
B)  ΔS°rxn > 0, ΔH°rxn rxnrxn rxn rxn > 0 
E)  ΔS°rxn = 0, ΔH°rxn = 0 
A)  ΔS°rxn > 0, ΔH°rxn > 0 
B)  ΔS°rxn > 0, ΔH°rxn rxnrxn rxn rxn > 0 
E)  ΔS°rxn = 0, ΔH°rxn = 0

Question 5

What is the third law of thermodynamics?

Accepted Answer

At 0 K all perfectly

Question 6

Which of these species has the highest entropy (S°) at 25°C?

Accepted Answer

A)  CH3OH(l) 
B)  CO(g) 
C)  MgCO3(s) 
D)  H2O(l) 
E)  Si(s) 
A)  CH3OH(l) 
B)  CO(g) 
C)  MgCO3(s) 
D)  H2O(l) 
E)  Si(s)

Question 7

What is ΔS° for the combustion of propane? C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

Accepted Answer

A)  -100.7 J/K 
B)  -72.6 J/K 
C)  72.6 J/K 
D)  100.7 J/K 
E)  877.2 J/K 
A)  -100.7 J/K 
B)  -72.6 J/K 
C)  72.6 J/K 
D)  100.7 J/K 
E)  877.2 J/K

Question 8

For a process that is spontaneous at high temperatures but not at low temperatures, the sign of ΔH is ________.

Accepted Answer

The answer of For a process that is spontaneous at...

Question 9

What is ΔG°rxn for the following reaction? 3NO2(g) + H2O(l) → 2HNO3(l) + NO(g)

Accepted Answer

A)  +8.7 kJ/mol 
B)  +192.2 kJ/mol 
C)  -178.6 kJ/mol 
D)  -192.2 kJ/mol 
E)  +639.1 kJ/mol 
A)  +8.7 kJ/mol 
B)  +192.2 kJ/mol 
C)  -178.6 kJ/mol 
D)  -192.2 kJ/mol 
E)  +639.1 kJ/mol

Question 10

In 1774 Joseph Priestly prepared oxygen by heating mercury(II) oxide according to the reaction HgO(l)  Hg(l) + ½O2(g), for which ΔHo = 90.84 kJ/mol and ΔSo = 108 J/K.mol. Which of the following statements is true for this reaction?

Accepted Answer

A)  The reaction is spontaneous only at low temperatures. 
B)  The reaction is spontaneous at all temperatures. 
C)  ΔGo becomes less favorable as temperature increases. 
D)  The reaction is spontaneous only at high temperatures. 
E)  The reaction is at equilibrium at 25oC and 1 atm pressure. 
A)  The reaction is spontaneous only at low temperatures. 
B)  The reaction is spontaneous at all temperatures. 
C)  ΔGo becomes less favorable as temperature increases. 
D)  The reaction is spontaneous only at high temperatures. 
E)  The reaction is at equilibrium at 25oC and 1 atm pressure.

Question 11

Predict the sign of ΔS for the reaction 6CO2(g) + 6H2O(g) → C6H12O6(s) + 6O2(g).

Accepted Answer

Question 12

For a process where a gas condenses to a liquid, the entropy ________.

Accepted Answer

The answer of For a process where a gas condenses...

Question 13

As the molar mass of a compound increases, the entropy ________.

Accepted Answer

A)  decreases 
B)  is constant 
C)  increases 
A)  decreases 
B)  is constant 
C)  increases

Question 14

What is ΔS° for the following reaction? 2Cl2(g) + SO2(g) → SOCl2(g) + Cl2O(g)

Accepted Answer

A)  -118.2 J/K • mol 
B)  -104.8 J/K • mol 
C)  104.8 J/K • mol 
D)  118.2 J/K • mol 
E)  1270.0 J/K • mol 
A)  -118.2 J/K • mol 
B)  -104.8 J/K • mol 
C)  104.8 J/K • mol 
D)  118.2 J/K • mol 
E)  1270.0 J/K • mol

Question 15

At constant temperature and pressure, which is the correct relationship between ΔG and other thermodynamic quantities?

Accepted Answer

A)  ΔG = ΔH - TΔS 
B)  ΔG = ΔH + TΔS 
C)  ΔG = ΔU - TΔS 
D)  ΔG = -TΔS 
E)  ΔG = q/T 
A)  ΔG = ΔH - TΔS 
B)  ΔG = ΔH + TΔS 
C)  ΔG = ΔU - TΔS 
D)  ΔG = -TΔS 
E)  ΔG = q/T

Question 16

How many types of vibrations does a bent triatomic molecule exhibit?

Accepted Answer

A)  0 
B)  1 
C)  2 
D)  3 
E)  4 
A)  0 
B)  1 
C)  2 
D)  3 
E)  4

Question 17

At temperatures below 273 K, it is observed that liquid water spontaneously freezes to form solid ice. What must be true about the entropy changes of the system and surroundings for this process?

Accepted Answer

A)  ΔSsys > 0, ΔSsurr > 0 
B)  ΔSsys surr > 0 
C)  ΔSsys surr sys > 0, ΔSsurr sys = 0, ΔSsurr > 0 
A)  ΔSsys > 0, ΔSsurr > 0 
B)  ΔSsys surr > 0 
C)  ΔSsys surr sys > 0, ΔSsurr sys = 0, ΔSsurr > 0

Question 18

The most probable state is the one with the ________.

Accepted Answer

A)  highest energy 
B)  largest number of possible arrangements 
C)  lowest number of possible arrangements 
D)  most symmetry 
E)  highest enthalpy 
A)  highest energy 
B)  largest number of possible arrangements 
C)  lowest number of possible arrangements 
D)  most symmetry 
E)  highest enthalpy

Question 19

For the process C6H6(l)  C6H6(s) at a temperature above the freezing point of C6H6,

Accepted Answer

A)  ΔS is positive. 
B)  ΔH is positive. 
C)  ΔG is positive. 
D)  ΔG = O. 
A)  ΔS is positive. 
B)  ΔH is positive. 
C)  ΔG is positive. 
D)  ΔG = O.

Question 20

What is ΔS° for the following reaction? 4Cr(s) + 3O2(g) → 2Cr2O3(s)

Accepted Answer

A)  -549.19 J/K • mol 
B)  -148.26 J/K • mol 
C)  +148.26 J/K • mol 
D)  +66.22 J/K • mol 
E)  +871.80 J/K • mol 
A)  -549.19 J/K • mol 
B)  -148.26 J/K • mol 
C)  +148.26 J/K • mol 
D)  +66.22 J/K • mol 
E)  +871.80 J/K • mol

Exam 18: Entropy, Free Energy, and Equilibrium

State the second and third laws of thermodynamics.

What term is given to the fact that the entropy of a perfect crystalline solid is zero at absolute zero?

The complete combustion of liquid benzene is represented by the equation: C6H6(l) + 7 O2(g) → 6CO2(g) + 3H2O(l) Using the data below, calculate, for this reaction a. ΔH° b. ΔG° at 25°C.

For a chemical reaction to be spontaneous at all temperatures, which conditions must be met?

What is the third law of thermodynamics?

Which of these species has the highest entropy (S°) at 25°C?

What is ΔS° for the combustion of propane? C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g)

For a process that is spontaneous at high temperatures but not at low temperatures, the sign of ΔH is ________.

What is ΔG°rxn for the following reaction? 3NO2(g) + H2O(l) → 2HNO3(l) + NO(g)

In 1774 Joseph Priestly prepared oxygen by heating mercury(II) oxide according to the reaction HgO(l) <----> Hg(l) + ½O2(g), for which ΔHo = 90.84 kJ/mol and ΔSo = 108 J/K.mol. Which of the following statements is true for this reaction?

Predict the sign of ΔS for the reaction 6CO2(g) + 6H2O(g) → C6H12O6(s) + 6O2(g).

For a process where a gas condenses to a liquid, the entropy ________.

As the molar mass of a compound increases, the entropy ________.

What is ΔS° for the following reaction? 2Cl2(g) + SO2(g) → SOCl2(g) + Cl2O(g)

At constant temperature and pressure, which is the correct relationship between ΔG and other thermodynamic quantities?

How many types of vibrations does a bent triatomic molecule exhibit?

At temperatures below 273 K, it is observed that liquid water spontaneously freezes to form solid ice. What must be true about the entropy changes of the system and surroundings for this process?

The most probable state is the one with the ________.

For the process C6H6(l) <-----> C6H6(s) at a temperature above the freezing point of C6H6,

What is ΔS° for the following reaction? 4Cr(s) + 3O2(g) → 2Cr2O3(s)

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

The complete combustion of liquid benzene is represented by the equation: C₆H₆(l) + 7 O₂(g) → 6CO₂(g) + 3H₂O(l) Using the data below, calculate, for this reaction a. ΔH° b. ΔG° at 25°C.

What is ΔS° for the combustion of propane? C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g)

What is ΔG°_rxn for the following reaction? 3NO₂(g) + H₂O(l) → 2HNO₃(l) + NO(g)

In 1774 Joseph Priestly prepared oxygen by heating mercury(II) oxide according to the reaction HgO(l) <----> Hg(l) + ½O₂(g), for which ΔH^o = 90.84 kJ/mol and ΔS^o = 108 J/K.mol. Which of the following statements is true for this reaction?

Predict the sign of ΔS for the reaction 6CO₂(g) + 6H₂O(g) → C₆H₁₂O₆(s) + 6O₂(g).

What is ΔS° for the following reaction? 2Cl₂(g) + SO₂(g) → SOCl₂(g) + Cl₂O(g)

For the process C₆H₆(l) <-----> C₆H₆(s) at a temperature above the freezing point of C₆H₆,

What is ΔS° for the following reaction? 4Cr(s) + 3O₂(g) → 2Cr₂O₃(s)