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Question:
Calculate the entropy change in surroundings when 1.00 mol of H₂O(l) is formed under standard conditions. Δ_fH⁰ = –286 kJ mol^–1.

Answer:

It is given that 286 kJ mol^-1of heat is evolved on the formation of 1 mol of H₂O_(l). Thus, an equal amount of heat will be absorbed by the surroundings.

q_surr= +286 kJ mol^-1

Entropy change (ΔS_surr) for the surroundings = q_surr/ 7

= 286 kJ mol^-1 / 298k

$\therefore$ ΔS_surr= 959.73 J mol^-1K^-1

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Question:
Calculate the entropy change in surroundings when 1.00 mol of H₂O(l) is formed under standard conditions. Δ_fH⁰ = –286 kJ mol^–1.

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Question: Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ΔfH0 = –286 kJ mol–1.

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Question:
Calculate the entropy change in surroundings when 1.00 mol of H₂O(l) is formed under standard conditions. Δ_fH⁰ = –286 kJ mol^–1.