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Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE? Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE? This reaction will be spontaneous only at low temperatures. This reaction will be spontaneous at all temperatures. This reaction will be nonspontaneous only at low temperatures. This reaction will be nonspontaneous at all temperatures. It is not possible to determine without more information.

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Answer:

This reaction will be nonspontaneous only at low temperatures.

Explanation:

An equation that helps us determine the spontaneity of a reaction is:

ΔG = ΔH - TΔS

A reaction will be spontaneous when ΔG is negative.

A reaction will be nonspontaneous when ΔG is positive.

With a positive ΔS and ΔH, ΔG will only be positive when the multiplication TxΔS is lower than ΔH. That happens when T is a low value. That's why the answer is This reaction will be nonspontaneous only at low temperatures.

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