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 ∆ H and ∆ G are - 241.60 k J m o l - 1 and - 228.40 k J m o l - 1 are respectively for H 2 O then the value of ∆ S for the above process is

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Correct answer: B. − 88 J K -1

∆ S = ∆ H - ∆ G T = - 241.6 - - 228.4 300 For 1 mole of H 2 O =- 44 J K -1 Hence, for 2 moles = − 88 J K -1

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 ∆ H and ∆ G are - 241.60 k J m o l - 1 and - 228.40 k J m o l - 1 are respectively for H 2 O then the value of ∆ S for the above process is

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