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NCERT Class XI Chemistry Thermodynamics Solutions

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Question : 22 of 22
Marks: +1, -0
Calculate the entropy change in surroundings when 1.00 mol of H2O(l)\mathrm{H_2O}_{(l)} is formed under standard conditions.
ΔfH∘\Delta_{\mathrm{f}}H^{\circ} = – 286 kJ mol−1\text{kJ mol}^{-1}.
Solution:  
ΔfH∘[H2O(l)]\Delta_{\mathrm{f}}H^{\circ}[\mathrm{H_2O}_{(l)}] = – 286 kJ mol−1\text{kJ mol}^{-1}
∴ qsurroundingsq_{\text{surroundings}} = + 286 kJ/mol
ΔS(surr)\Delta S_{(\text{surr})} = q298\frac{q}{298} = 286×1000298\frac{286 \times 1000}{298} J K−1mol−1\text{J K}^{-1} \text{mol}^{-1} = 959.73 J K−1mol−1\text{J K}^{-1} \text{mol}^{-1}
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