Ask Question
29 March, 18:28

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?

+5
Answers (1)
  1. 29 March, 21:22
    0
    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.
Know the Answer?
Not Sure About the Answer?
Find an answer to your question ✅ “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 ...” in 📘 Chemistry if you're in doubt about the correctness of the answers or there's no answer, then try to use the smart search and find answers to the similar questions.
Search for Other Answers