Calculate the following quantities.
Delta ∆ S (sys) —– j/K
Delta ∆ S (sur) —– j/K
Delta ∆ S (univ) —– j/K
C Graphite = 5.7 S° J/(mol·K)
2H2(g) = 130.7 S° J/(mol·K)
CH4(g) = 186.3 S° J/(mol·K)
I do not know how to find the answer, my chemistry teacher is horrible at teaching. Please help frustrated from college kid.
1 Answer

Calculate the ΔS for the system:
Sum of entropy of products – sum of entropy of reactants
186.3 – [2(130.7) + 5.7 ]
186.3 – [ 261.4 + 5.7 ]
186.3 – 267.1 = 80.8 Joules/K
Entropy change of surroundings: Since the reaction evolves heat, the entropy change
of the surrounding is a positive value.
Delta H = 74.6 kilojoules x 1000 Joules/ kilojoule = 74,600 Joules
ΔS = ΔH / T = +74,600 Joules/ 298.15 K = +250.2 Joules/K
Entropy change of universe: 80.8 Joules + 250.2 Joules = +169.4 Joules/K