Combustion of Hydrogen in a fuel cell at 300 K is represented as 2 H 2 g + O 2 g → 2 H 2 O g . If Δ H and Δ G are − 241 .80 kJ mol − 1 and − 228.60 kJ mol − 1 respectively for H 2 O then the value of Δ S for the above process is:

Question

Combustion of Hydrogen in a fuel cell at 300 K is represented as 2 H 2 g + O 2 g → 2 H 2 O g . If Δ H and Δ G are − 241 .80 kJ mol − 1 and − 228.60 kJ mol − 1 respectively for H 2 O then the value of Δ S for the above process is:, + 44 . J K - 1 m o l - 1, - 88 J K - 1 m o l - 1, + 88 J K - 1 m o l - 1, - 44 . J K - 1 m o l - 1

MARKS App · Accepted Answer

ΔS = ΔH − ΔG T = − 241.8 − − 228.6 300 = - 44 J K - 1 m o l e - 1

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