Ask Question
10 February, 22:32

What can be said about a reaction with H = 62.4 kJ/mol and S = 0.145 kJ / (mol·K) ?

+5
Answers (2)
  1. 10 February, 22:47
    0
    The answer is "It is spontaneous at 500 k"
  2. 11 February, 00:29
    0
    At 430.34 K the reaction will be at equilibrium, at T > 430.34 the reaction will be spontaneous, and at T < 430.4K the reaction will not occur spontaneously.

    Explanation:

    1) Variables:

    G = Gibbs energy

    H = enthalpy

    S = entropy

    2) Formula (definition)

    G = H + TS

    => ΔG = ΔH - TΔS

    3) conditions

    ΔG spontaneous reaction

    ΔG = 0 = > equilibrium

    ΔG > 0 non espontaneous reaction

    4) Assuming the data given correspond to ΔH and ΔS

    ΔG = ΔH - T ΔS = 62.4 kJ/mol + T 0.145 kJ / mol * K

    => T = [ΔH - ΔG] / ΔS

    ΔG = 0 = > T = [ 62.4 kJ/mol - 0 ] / 0.145 kJ/mol*K = 430.34K

    This is, at 430.34 K the reaction will be at equilibrium, at T > 430.34 the reaction will be spontaneous, and at T < 430.4K the reaction will not occur spontaneously.
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “What can be said about a reaction with H = 62.4 kJ/mol and S = 0.145 kJ / (mol·K) ? ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers