One mole of ice is converted into water at 273 K. The entropies of H2O(s) and H2O(l) are 38.20 and 60.01 J mol-1 K-1 respectively. The enthalpy change for the conversion is

Question

One mole of ice is converted into water at 273 K. The entropies of H2O(s) and H2O(l) are 38.20 and 60.01 J mol-1 K-1 respectively. The enthalpy change for the conversion is (A) 59.54 J mol-1 (B) 5954 J mol-1 (C) 595.4 J mol-1 (D) 320.6 J mol-1

Tardigrade Admin · Accepted Answer

ΔH = TΔS = 273 × (60 01 - 38-20) = 5954-13 J mol-1

Q. One mole of ice is converted into water at 273 K. The entropies of $H_{2} O (s) an d H_{2} O (l)$ are 38.20 and 60.01 $J m o l^{- 1} K^{- 1}$ respectively. The enthalpy change for the conversion is

$59.54 J m o l^{- 1}$

$5954 J m o l^{- 1}$

$595.4 J m o l^{- 1}$

$320.6 J m o l^{- 1}$

$Δ$ H = T $Δ$ S = 273 $\times$ (60 01 - 38-20) = 5954-13 J $m o l^{- 1}$

Q. One mole of ice is converted into water at 273 K. The entropies of H2​O(s)andH2​O(l) are 38.20 and 60.01 Jmol−1K−1 respectively. The enthalpy change for the conversion is

59.54Jmol−1

5954Jmol−1

595.4Jmol−1

320.6Jmol−1