A reaction has H = 61.9 kJ/mol and S = 405.4 J/K. Is this ...

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Question 1

For the reaction below ΔG° = +33.0 kJ, ΔH° = +92.2 kJ, and ΔS° = +198.7 J/K. Estimate the temperature at which this reaction becomes spontaneous.

2 NH3(g) → N2(g) + 3 H2(g)

◦ 298 K
◦ 0.464 K
◦ 166 K
◦ 464 K

Question 2

A reaction has ΔH° = 61.9 kJ/mol and ΔS° = 405.4 J/K. Is this reaction spontaneous or nonspontaneous? At what temperature (if any) can the spontaneity be reversed?
◦ nonspontaneous, can be made spontaneous at 153 K
◦ spontaneous, can be made nonspontaneous at 153 K
◦ spontaneous, cannot be made nonspontaneous at any temperature
◦ nonspontaneous, cannot be made spontaneous at any temperature

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Thanks for the timely response, appreciate it

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