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Considering only the signs of ΔH & ΔS predict whether the reaction is spontaneous or is...

Considering only the signs of ΔH & ΔS predict whether the reaction is spontaneous or is not. If it is temperature dependent, should the temperature be high or low for the reaction to be spontaneous? Explain your reasoning.

i) NH4NO3(s) + heat → NH4^+(aq) + NO3^−(aq)

ii) 2 H2O (l) + heat → 2H2 (g) + O2 (g)

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Answer #1

In both Reactions heat is given to the reactants thus the Reaction is endothermic and  H is positive for both Reactions. While moles of products is greater than moles of reactants thus the degree of randomness is increasing in the product side, hence  S is also positive for both Reactions.

We know for a spontaneous Reaction G should be negative.

Also G = H - TS

Thus for both of these given reactions to be spontaneous the temperature needs to be high so that the value of G gets negative

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