Question 1

Why is heating your home with gas more efficient than heating it with electricity?

Accepted Answer

Heating with gas only requires a one-ste

Question 2

Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics.

Accepted Answer

A) reversible reaction 
B) forward reaction 
C) reverse reaction 
D) equilibrium reaction 
E) STP reaction 
A) reversible reaction 
B) forward reaction 
C) reverse reaction 
D) equilibrium reaction 
E) STP reaction

Question 3

Place the following in order of increasing molar entropy at 298 K.
CO2 C3H8 SO

Accepted Answer

A) CO2 3H8 3H8 2 2 3H8 
D) C3H8 2 
E) CO2 3H8 
A) CO2 3H8 3H8 2 2 3H8 
D) C3H8 2 
E) CO2 3H8

Question 4

Above what temperature does the following reaction become nonspontaneous?
FeO(s)+ CO(g)→ CO2(g)+ Fe(s)ΔH = -11.0 kJ;ΔS = -17.4 J/K

Accepted Answer

A) 632 K 
B) 298 K 
C) 191 K 
D) This reaction is nonspontaneous at all temperatures. 
E) This reaction is spontaneous at all temperatures. 
A) 632 K 
B) 298 K 
C) 191 K 
D) This reaction is nonspontaneous at all temperatures. 
E) This reaction is spontaneous at all temperatures.

Question 5

Choose the statement below that is true.

Accepted Answer

A) If K < 1,the reaction is spontaneous in the reverse direction. 
B) If K < 1,the reaction is spontaneous in the forward direction. 
C) If K < 1,the reaction is at equilibrium. 
D) Not enough information is given. 
A) If K < 1,the reaction is spontaneous in the reverse direction. 
B) If K < 1,the reaction is spontaneous in the forward direction. 
C) If K < 1,the reaction is at equilibrium. 
D) Not enough information is given.

Question 6

Which one of the following would be expected to have the lowest standard molar entropy,S°,at 25°C?

Accepted Answer

A) C10H22(s) 
B) C10H22(l) 
C) C14H30(s) 
D) C14H30OH(l) 
A) C10H22(s) 
B) C10H22(l) 
C) C14H30(s) 
D) C14H30OH(l)

Question 7

Which process will decrease entropy?

Accepted Answer

A) H2O(g)→ H2O(l) 
B) CaCO3(s)→ CaO(s)+ CO2(g) 
C) 2N2O(g)→ 2N2(g)+ O2(g) 
D) CO2(s)→ CO2(g) 
A) H2O(g)→ H2O(l) 
B) CaCO3(s)→ CaO(s)+ CO2(g) 
C) 2N2O(g)→ 2N2(g)+ O2(g) 
D) CO2(s)→ CO2(g)

Question 8

If ΔG < 0,which of the following statements is true?

Accepted Answer

A) The reaction is spontaneous. 
B) The reaction is not spontaneous. 
C) The reaction is at equilibrium. 
D) Not enough information is given. 
A) The reaction is spontaneous. 
B) The reaction is not spontaneous. 
C) The reaction is at equilibrium. 
D) Not enough information is given.

Question 9

Consider a reaction that has a positive ΔH and a negative ΔS.Which of the following statements is true?

Accepted Answer

A) This reaction will be spontaneous only at high temperatures. 
B) This reaction will be spontaneous at all temperatures. 
C) This reaction will be nonspontaneous at all temperatures. 
D) This reaction will be nonspontaneous only at high temperatures. 
E) It is not possible to determine without more information. 
A) This reaction will be spontaneous only at high temperatures. 
B) This reaction will be spontaneous at all temperatures. 
C) This reaction will be nonspontaneous at all temperatures. 
D) This reaction will be nonspontaneous only at high temperatures. 
E) It is not possible to determine without more information.

Question 10

Which is true for a chemical reaction at equilibrium?

Accepted Answer

A) Entropy is maximum 
B) Gibbs energy is minimum 
C) ΔG° = 0 
D) All of the above 
A) Entropy is maximum 
B) Gibbs energy is minimum 
C) ΔG° = 0 
D) All of the above

Question 11

Place the following in order of decreasing molar entropy at 298 K.
H2 Cl2 F2

Accepted Answer

A) H2 > Cl2 > F2 
B) Cl2 > H2 > F2 
C) F2 > Cl2 > H2 
D) H2 > F2 > Cl2 
E) Cl2 > F2 > H2 
A) H2 > Cl2 > F2 
B) Cl2 > H2 > F2 
C) F2 > Cl2 > H2 
D) H2 > F2 > Cl2 
E) Cl2 > F2 > H2

Question 12

Above what temperature does the following reaction become nonspontaneous?
2 H2S(g)+ 3 O2(g)→ 2 SO2(g)+ 2 H2O(g)
ΔH = -1036 kJ;ΔS = -153.2 J/K

Accepted Answer

A) 6.762 × 103 K 
B) 158.7 K 
C) 298 K 
D) This reaction is nonspontaneous at all temperatures. 
E) This reaction is spontaneous at all temperatures. 
A) 6.762 × 103 K 
B) 158.7 K 
C) 298 K 
D) This reaction is nonspontaneous at all temperatures. 
E) This reaction is spontaneous at all temperatures.

Question 13

Match the following.
-Q = 1

Accepted Answer

A) ΔG  0 
D) ΔG  ΔG° 
A) ΔG  0 
D) ΔG  ΔG°

Question 14

Place the following in order of increasing molar entropy at 298 K.
NO CO SO

Accepted Answer

A) NO < CO < SO 
B) SO < CO < NO 
C) SO < NO < CO 
D) CO < SO < NO 
E) CO < NO < SO 
A) NO < CO < SO 
B) SO < CO < NO 
C) SO < NO < CO 
D) CO < SO < NO 
E) CO < NO < SO

Question 15

In which of the following processes do the molecules become more orderly?

Accepted Answer

A) water freezing 
B) ice melting 
C) water evaporating 
D) salt dissolving in water 
E) dry ice subliming 
A) water freezing 
B) ice melting 
C) water evaporating 
D) salt dissolving in water 
E) dry ice subliming

Question 16

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction.
2 Hg(g)+ O2(g)→ 2 HgO(s)ΔG° = -180.8 kJ
P(Hg)= 0.025 atm,P(O2)= 0.037 atm

Accepted Answer

A) +207 kJ 
B) -154.4 kJ 
C) -26.5 kJ 
D) -164 kJ 
E) +60.7 kJ 
A) +207 kJ 
B) -154.4 kJ 
C) -26.5 kJ 
D) -164 kJ 
E) +60.7 kJ

Question 17

Define the second law of thermodynamics.

Accepted Answer

For any spontaneous

Question 18

Determine ΔG°rxn using the following information.
FeO(s)+ CO(g)→ Fe(s)+ CO2(g)ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Accepted Answer

A) +191.0 kJ 
B) -5.8 kJ 
C) +1.6 kJ 
D) -6.4 kJ 
E) +89.5 kJ 
A) +191.0 kJ 
B) -5.8 kJ 
C) +1.6 kJ 
D) -6.4 kJ 
E) +89.5 kJ

Question 19

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction.
3 O2(g)→ 2 O3(g)ΔG° = +326 kJ
P(O2)= 0.41 atm,P(O3)= 5.2 atm

Accepted Answer

A) +341 kJ 
B) +17.8 kJ 
C) +332 kJ 
D) -47.4 kJ 
E) -109 kJ 
A) +341 kJ 
B) +17.8 kJ 
C) +332 kJ 
D) -47.4 kJ 
E) -109 kJ

Question 20

Given the following equation,
H2O(g)+ CO(g)→ H2(g)+ CO2(g)ΔG°rxn = -28.6 kJ
Calculate ΔG°rxn for the following reaction.
5 H2O(g)+ 5 CO(g)→ 5 H2(g)+ 5 CO2(g)

Accepted Answer

A) -143.0 kJ 
B) +143.0 kJ 
C) -5.72 kJ 
D) +5.72 kJ 
E) 28.6 kJ 
A) -143.0 kJ 
B) +143.0 kJ 
C) -5.72 kJ 
D) +5.72 kJ 
E) 28.6 kJ

Why is heating your home with gas more efficient than heating it with electricity?

Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics.

Place the following in order of increasing molar entropy at 298 K. CO₂ C₃H₈ SO

Above what temperature does the following reaction become nonspontaneous? FeO(s)+ CO(g)→ CO₂(g)+ Fe(s)ΔH = -11.0 kJ;ΔS = -17.4 J/K

Choose the statement below that is true.

Which one of the following would be expected to have the lowest standard molar entropy,S°,at 25°C?

Which process will decrease entropy?

If ΔG < 0,which of the following statements is true?

Consider a reaction that has a positive ΔH and a negative ΔS.Which of the following statements is true?

Which is true for a chemical reaction at equilibrium?

Place the following in order of decreasing molar entropy at 298 K. H₂ Cl₂ F₂

Above what temperature does the following reaction become nonspontaneous? 2 H₂S(g)+ 3 O₂(g)→ 2 SO₂(g)+ 2 H₂O(g) ΔH = -1036 kJ;ΔS = -153.2 J/K

Match the following. -Q = 1

Place the following in order of increasing molar entropy at 298 K. NO CO SO

In which of the following processes do the molecules become more orderly?

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g)+ O₂(g)→ 2 HgO(s)ΔG° = -180.8 kJ P(Hg)= 0.025 atm,P(O₂)= 0.037 atm

Define the second law of thermodynamics.

Determine ΔG°_rxn using the following information. FeO(s)+ CO(g)→ Fe(s)+ CO₂(g)ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 3 O₂(g)→ 2 O₃(g)ΔG° = +326 kJ P(O₂)= 0.41 atm,P(O₃)= 5.2 atm

Given the following equation, H₂O(g)+ CO(g)→ H₂(g)+ CO₂(g)ΔG°_rxn = -28.6 kJ Calculate ΔG°_rxn for the following reaction. 5 H₂O(g)+ 5 CO(g)→ 5 H₂(g)+ 5 CO₂(g)

Matter, Measurement, and Problem Solving

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Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

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Exam 17: Free Energy and Thermodynamics

Why is heating your home with gas more efficient than heating it with electricity?

Give the name of the reaction that achieves the theoretical limits with respect to free energy in thermodynamics.

Place the following in order of increasing molar entropy at 298 K. CO2 C3H8 SO

Above what temperature does the following reaction become nonspontaneous? FeO(s)+ CO(g)→ CO2(g)+ Fe(s)ΔH = -11.0 kJ;ΔS = -17.4 J/K

Choose the statement below that is true.

Which one of the following would be expected to have the lowest standard molar entropy,S°,at 25°C?

Which process will decrease entropy?

If ΔG < 0,which of the following statements is true?

Consider a reaction that has a positive ΔH and a negative ΔS.Which of the following statements is true?

Which is true for a chemical reaction at equilibrium?

Place the following in order of decreasing molar entropy at 298 K. H2 Cl2 F2

Above what temperature does the following reaction become nonspontaneous? 2 H2S(g)+ 3 O2(g)→ 2 SO2(g)+ 2 H2O(g) ΔH = -1036 kJ;ΔS = -153.2 J/K

Match the following. -Q = 1

Place the following in order of increasing molar entropy at 298 K. NO CO SO

In which of the following processes do the molecules become more orderly?

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g)+ O2(g)→ 2 HgO(s)ΔG° = -180.8 kJ P(Hg)= 0.025 atm,P(O2)= 0.037 atm

Define the second law of thermodynamics.

Determine ΔG°rxn using the following information. FeO(s)+ CO(g)→ Fe(s)+ CO2(g)ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g)→ 2 O3(g)ΔG° = +326 kJ P(O2)= 0.41 atm,P(O3)= 5.2 atm

Given the following equation, H2O(g)+ CO(g)→ H2(g)+ CO2(g)ΔG°rxn = -28.6 kJ Calculate ΔG°rxn for the following reaction. 5 H2O(g)+ 5 CO(g)→ 5 H2(g)+ 5 CO2(g)

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Place the following in order of increasing molar entropy at 298 K. CO₂ C₃H₈ SO

Above what temperature does the following reaction become nonspontaneous? FeO(s)+ CO(g)→ CO₂(g)+ Fe(s)ΔH = -11.0 kJ;ΔS = -17.4 J/K

Place the following in order of decreasing molar entropy at 298 K. H₂ Cl₂ F₂

Above what temperature does the following reaction become nonspontaneous? 2 H₂S(g)+ 3 O₂(g)→ 2 SO₂(g)+ 2 H₂O(g) ΔH = -1036 kJ;ΔS = -153.2 J/K

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 2 Hg(g)+ O₂(g)→ 2 HgO(s)ΔG° = -180.8 kJ P(Hg)= 0.025 atm,P(O₂)= 0.037 atm

Determine ΔG°_rxn using the following information. FeO(s)+ CO(g)→ Fe(s)+ CO₂(g)ΔH° = -11.0 kJ;ΔS° = -17.4 J/K

Calculate ΔG_rxn at 298 K under the conditions shown below for the following reaction. 3 O₂(g)→ 2 O₃(g)ΔG° = +326 kJ P(O₂)= 0.41 atm,P(O₃)= 5.2 atm

Given the following equation, H₂O(g)+ CO(g)→ H₂(g)+ CO₂(g)ΔG°_rxn = -28.6 kJ Calculate ΔG°_rxn for the following reaction. 5 H₂O(g)+ 5 CO(g)→ 5 H₂(g)+ 5 CO₂(g)