Ask Question
4 April, 17:29

Be sure to answer all parts. consider the combustion of butane gas: c4h10 (g) + 13 2 o2 (g) → 4co2 (g) + 5h2o (g) (a) predict the signs of δs o and δh o. δs o : negative positive δh o : negative positive (b) calculate δg o at 298 k. kj

+3
Answers (1)
  1. 4 April, 18:21
    0
    Answers are:

    1) ΔH is negative because that is combustion reaction and heat is released, enthalpy of combustion is - 2877.5 kJ/mol.

    2) ΔS is positive, because there more molecules on the right side of balanced chemical reaction, standard molar entropy is 310.23 J/mol · K.

    3) ΔG = ΔH - TΔS.

    ΔG = - 2877.5 kJ/mol - 298 K · 310.23 J/mol·K.

    ΔG = - 2969.95 kJ/mol.
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Be sure to answer all parts. consider the combustion of butane gas: c4h10 (g) + 13 2 o2 (g) → 4co2 (g) + 5h2o (g) (a) predict the signs of ...” 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