For a particular reaction, ΔH° is 67.7 kJ and ΔS is 126.9 J/K. Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction? For a particular reaction, ΔH° is 67.7 kJ and ΔS is 126.9 J/K. Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction?

Question

Rudy Patel

Chemistry

13 June, 13:06

For a particular reaction, ΔH° is 67.7 kJ and ΔS is 126.9 J/K. Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction? For a particular reaction, ΔH° is 67.7 kJ and ΔS is 126.9 J/K. Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction?

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Answers (1)

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Finley Cochran · Answer 1

The forward reaction is spontaneous above 533 K.

Explanation:

A reaction is spontaneous when the standard Gibbs energy of the reaction (ΔG°) is negative. ΔG° is related to the standard enthalpy of the reaction (ΔH°) and the standard entropy of the reaction (ΔS°) through the following expression.

ΔG° = ΔH° - T.ΔS°

where,

T is the absolute temperature

When ΔG° < 0,

ΔH° - T.ΔS° < 0

ΔH° < T.ΔS°

T > ΔH° / ΔS° = (67.7 * 10³ J) / (126.9 J/K) = 533 K

The forward reaction is spontaneous above 533 K.