Problem: For the reaction at 298 K,2NO2 (g) ⇌ N2O4 (g)the values of ΔH° and ΔS° are -58.03 kJ and -176.6 J/K, respectively. What is the value of ΔG° at 298 K? Assuming that ΔH° and ΔS° do not depend on temperature, at what temperature is ΔG° = 0? Is ΔG° negative above or below this temperature?

FREE Expert Solution

Step 1

G° = H° - TS°


G° =(-58.03 kJ) - (298 K)(-176.6 JK×1 kJ103 J)


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Problem Details

For the reaction at 298 K,

2NO2 (g) ⇌ N2O4 (g)

the values of ΔH° and ΔS° are -58.03 kJ and -176.6 J/K, respectively. What is the value of ΔG° at 298 K? Assuming that ΔH° and ΔS° do not depend on temperature, at what temperature is ΔG° = 0? Is ΔG° negative above or below this temperature?

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