1 mol of ice is converted to liquid at 273 K; H 2 O (s) and H 2 O (l) have entropies 38.20 and 60.03 J m o l - 1 d e g . Enthalpy changes in the conversion will be

Question

1 mol of ice is converted to liquid at 273 K; H 2 O (s) and H 2 O (l) have entropies 38.20 and 60.03 J m o l - 1 d e g . Enthalpy changes in the conversion will be, 59.59 J/mol, 5959.59 J/mol, 595.959 J/mol, 5.959 J/mol

MARKS App · Accepted Answer

Δ S = S f i n a l - S i n i t i a l = ( 60.03 - 38.20 ) J m o l - 1 K - 1 = 21.83 J m o l - 1 K - 1 Also Δ S = Δ H f u s i o n T or Δ H f u s i o n = T Δ S = 273 K × 21.83 J m o l - 1 K - 1 = 5959.59 J m o l - 1 .

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