Question

Entropy 1. Predict whether the entropy change is greater than or less than zero for each of the following processes. a) freezing water b) sublimation of dry ice c) dissolving sugar in water d) A liquid boils 2. Calculate the standard entropy values for the following reactions at 25°C. a) N2(g) + 3H2(g) ? 2NH3(g) b) H2(g) + Cl2(g) ? 2HCl(g) c) 2CO(g) + O2(g) ? 2CO2(g) d) 3O2(g) ? 2O3(g) e) 2NH3(g) + CO2(g) ? NH2CONH2(aq) + H2O(l) 3. Determine if liquid water will spontaneously freeze at -5.00 °C? Is it spontaneous at +5.00 °C? What can you say about the values of ?Suniv? Show your solution. Gibbs Free Energy 1. For the reaction, H2O(l)?H2O(g), calculate ?G at a) 20°C, b) 100°C c) 150°C. 2. Calculate the standard-free energy changes for the reaction at 25°C . a. 2MgO(s) ? 2Mg(s) + O2(g) b. H2(g) + Br2(l) ? 2HBr(g) c. 2C2H6(g) + 7O2(g) ? 4CO2(g) + 6H2O(l) 3. From the values of ?H and ?S, predict which of the following reactions would be spontaneous at 25°C: Reaction A: ?H = 10.5 kJ/mol, ?S = 30 J/K • mol; Reaction B: ?H = 1.8 kJ/mol, ?S = -113 J/K • mol. If either of the reactions is nonspontaneous at 25°C, at what temperature might it become spontaneous?

          Entropy

1. Predict whether the entropy change is greater than or less than zero for each of the following processes.

a) freezing water
b) sublimation of dry ice
c) dissolving sugar in water
d) A liquid boils

2. Calculate the standard entropy values for the following reactions at 25°C.

a) N2(g) + 3H2(g) ? 2NH3(g)
b) H2(g) + Cl2(g) ? 2HCl(g)
c) 2CO(g) + O2(g) ? 2CO2(g)
d) 3O2(g) ? 2O3(g)
e) 2NH3(g) + CO2(g) ? NH2CONH2(aq) + H2O(l)

3. Determine if liquid water will spontaneously freeze at -5.00 °C? Is it spontaneous at +5.00 °C? What can you say about the values of ?Suniv? Show your solution.

Gibbs Free Energy

1. For the reaction, H2O(l)?H2O(g), calculate ?G at

a) 20°C,
b) 100°C
c) 150°C.

2. Calculate the standard-free energy changes for the reaction at 25°C .

a. 2MgO(s) ? 2Mg(s) + O2(g)
b. H2(g) + Br2(l) ? 2HBr(g)
c. 2C2H6(g) + 7O2(g) ? 4CO2(g) + 6H2O(l)

3. From the values of ?H and ?S, predict which of the following reactions would be spontaneous at 25°C:
Reaction A: ?H = 10.5 kJ/mol, ?S = 30 J/K • mol;
Reaction B: ?H = 1.8 kJ/mol, ?S = -113 J/K • mol.
If either of the reactions is nonspontaneous at 25°C, at what temperature might it become spontaneous?

Entropy

1. Predict whether the entropy change is greater than or less than zero for each of the following processes.

a) freezing water
b) sublimation of dry ice
c) dissolving sugar in water
d) A liquid boils

2. Calculate the standard entropy values for the following reactions at 25°C.

a) N2(g) + 3H2(g) ? 2NH3(g)
b) H2(g) + Cl2(g) ? 2HCl(g)
c) 2CO(g) + O2(g) ? 2CO2(g)
d) 3O2(g) ? 2O3(g)
e) 2NH3(g) + CO2(g) ? NH2CONH2(aq) + H2O(l)

3. Determine if liquid water will spontaneously freeze at -5.00 °C? Is it spontaneous at +5.00 °C? What can you say about the values of ?Suniv? Show your solution.

Gibbs Free Energy

1. For the reaction, H2O(l)?H2O(g), calculate ?G at

a) 20°C,
b) 100°C
c) 150°C.

2. Calculate the standard-free energy changes for the reaction at 25°C .

a. 2MgO(s) ? 2Mg(s) + O2(g)
b. H2(g) + Br2(l) ? 2HBr(g)
c. 2C2H6(g) + 7O2(g) ? 4CO2(g) + 6H2O(l)

3. From the values of ?H and ?S, predict which of the following reactions would be spontaneous at 25°C:
Reaction A: ?H = 10.5 kJ/mol, ?S = 30 J/K • mol;
Reaction B: ?H = 1.8 kJ/mol, ?S = -113 J/K • mol.
If either of the reactions is nonspontaneous at 25°C, at what temperature might it become spontaneous?

Added by Jose Antonio R.

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