What is the entropy change (in JK1 mol1) when one mole of ice is converted into water at 0°C ?(The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol-1 at 0°C)

Question

What is the entropy change (in JK1 mol1) when one mole of ice is converted into water at 0°C ?(The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol-1 at 0°C) (A) 21.98 (B) 20.13 (C) 2.013 (D) 2.198

Tardigrade Admin · Accepted Answer

Δ H = 6.0 kJ mol-1 = 6 × 103 J mol-1 T = 0° C = 273 K Δ S = (Δ H/T) (For a reversible process) Δ S = (6 × 103 J mol-1/273 K) = 21.98 JK-1 mol-1

Q. What is the entropy change (in $J K^{1} m o l^{1}$ ) when one mole of ice is converted into water at $0^{\circ} C$ ?(The enthalpy change for the conversion of ice to liquid water is $6.0 k J m o l^{- 1}$ at $0^{\circ} C$ )

21.98

20.13

2.013

2.198

$Δ H = 6.0 k J m o l^{- 1} = 6 \times 1 0^{3} J m o l^{- 1}$

$T = 0^{\circ} C = 273 K$

$Δ S = \frac{Δ H}{T}$ (For a reversible process)

$Δ S = \frac{6 \times 1 0 ^{3} J m o l ^{- 1}}{273 K} = 21.98 J K^{- 1} m o l^{- 1}$

Q. What is the entropy change (in JK1mol1) when one mole of ice is converted into water at 0∘C ?(The enthalpy change for the conversion of ice to liquid water is 6.0kJmol−1 at 0∘C)