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

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 ∆ 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, 4.4 J K -1, − 88 J K -1, + 88 J K -1, − 44 J K -1

MARKS App · Accepted Answer

∆ 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

Search any question & find its solution

Looking for more such questions to practice?