Consider the following reaction, which is carried out at 300 K:

CH3CH2OH + 3O2 → 2CO2 + 3H2O ∆H = - 1,235 kJ/mol and ∆S = + 0.22kJ/mol•K

1.) What is the value of ∆G? Show your work.

2.) Classify the reaction as spontaneous or nonspontaneous.

3.) Suggest why the value for ∆S is positive in this reaction

Question

15 October, 06:13

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Answers (1)

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Misael Huff · Answer 1

G = H - T S

-1235 - (300 x 220)

-67.24kJ/mol

Since the Gibbs energy reaction is negative the reaction is spontaneous