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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:

Options

  1. A+ 44 . J K - 1 m o l - 1
  2. B- 88 J K - 1 m o l - 1
  3. C+ 88 J K - 1 m o l - 1
  4. D- 44 . J K - 1 m o l - 1

Correct answer

B. - 88 J K - 1 m o l - 1

Step-by-step solution

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

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