Question

Suppose that you are given the following information for this reaction at room temperature: ΔG°f for SO2(g) = −300.19 kJ / mol ΔG°f for O2(g) = 0.0 kJ / mol ΔG°f for SO3(g) = −371.1 kJ / mol Which statement about this reaction is not correct?
A) The stoichiometry for this reaction affects your calculations for ΔG°.
B) To calculate ΔG° for the decomposition of one mole of SO3(g), you use the expression ΔG° = (ΔG°f for O2 + ΔG°f for SO2 ) − (ΔG°f for SO3 ).
C) If ΔG° is negative, the reaction is spontaneous.
D) The values for ΔG°f from the tables are given for one mole of substance.

Answer 1

Yes so kamay is the answer to this because the 10SO3 is around the beginning of the equation