Ask Question
5 March, 02:45

Above what temperature does the following reaction become nonspontaneous? 2 H2S (g) + 3 O2 (g) → 2 SO2 (g) + 2 H2O (g) ΔH = - 1036 kJ; ΔS = - 153.2 J/K

+5
Answers (1)
  1. 5 March, 03:07
    0
    Above 6762 K the reaction becomes nonspontaneous.

    Explanation:

    Let's consider the following equation.

    2 H₂S (g) + 3 O₂ (g) → 2 SO₂ (g) + 2 H₂O (g)

    This reaction will become nonspontaneous when the Gibbs free energy (ΔG) is higher than zero. ΔG is related to the enthalpy of the reaction (ΔH) and the entropy of the reaction (ΔS) through the following expression.

    ΔG = ΔH - T.ΔS

    If ΔG must be positive, then

    ΔH - T.ΔS > 0

    ΔH > T.ΔS

    -1036 * 10³ J > T. (-153.2 J/K)

    T > 6762 K
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Above what temperature does the following reaction become nonspontaneous? 2 H2S (g) + 3 O2 (g) → 2 SO2 (g) + 2 H2O (g) ΔH = - 1036 kJ; ΔS = ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers