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11 Dec 2019

QUESTION 9

Which has the lowest entropy?

CH3OH(s, –25°C)

CH3OH(s, –15°C)

CH3OH(l, 15°C)

CH3OH(l, 25°C)

1 points (Extra Credit)

QUESTION 10

Which statement is true about the formation of CaCO3(s) from CaO(s) and CO2(g) at 1.00 atm?

CaO(s) + CO2(g) → CaCO3(s) ΔH° = -178.7 kJ and ΔS° = -150.4 J/K

The reaction is spontaneous at all temperatures.

The reaction is spontaneous at high temperatures.

The reaction is spontaneous at low temperatures.

The reaction is not spontaneous at any temperature.

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13 Dec 2019

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Related questions

1. (a)Consider the reaction:

N2(g)+ 3 F2(g) → 2 NF3(g)ΔH ° = -249 kJ and ΔS ° = -278 J/K at 25°C

CalculateΔG ° and state whether the equilibrium composition shouldfavor reactants or products at standard conditions. Explain yourreasoning

(b) Consider theformation of CaCO3(s) from CaO(s) andCO2(g) at 1.00 atm;

CaO(s) +CO2(g) → CaCO3(s)ΔH ° = -178.7 kJ and ΔS ° = -150.4 J/K

Is this reactionspontaneous at low, high, or all temperatures? Show yourcalculations clearly and explain your reasoning.

Consider the following reaction:
CaCO3(s)→CaO(s)+CO2(g).
Estimate ΔG∘ for this reaction at each of the following temperatures. (Assume that ΔH∘ and ΔS∘ do not change too much within the given temperature range.)

Part A

320 K
ΔG∘ = kJ

Part B

1095 K
ΔG∘ = kJ

Part C

1445 K
ΔG∘ = kJ

Part D

Predict whether or not the reaction in part A will be spontaneous at 320 K .

-spontaneous
-nonspontaneous

Part E

Predict whether or not the reaction in part B will be spontaneous at 1095 K .

-spontaneous
-nonspontaneous

Part F

Predict whether or not the reaction in part C will be spontaneous at 1445 K .

-spontaneous
-nonspontaneous

For the reaction   4Ag(s)+O2(g)→2Ag2O(s),   ΔH°=–61.14kJ   and    ΔS° = –132   and  J/K  at 25°C.   Which of the following statements is false?

Assume that ΔH° and ΔS° are essentially temperature independent.Assume that ΔH° and ΔS° are essentially temperature independent.

a. The change in entropy is the driving force at high temperatures.

b. The enthalpy of the products is less than the enthalpy of the reactants.

c. The entropy of the products is less than the entropy of the reactants.

d. The reaction will be spontaneous at low temperatures, and the reverse reaction will be spontaneous at high temperatures.

e. The enthalpy change for the reaction is the driving force of the reaction at low temperatures.

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