Calculate the entropy change in surroundings when 1.00 mol of H₂O₍_l₎ is formed under standard conditions. Δ_fH^θ = –286 kJ mol^–1.

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Solution

It is given that 286 kJ mol^–1 of 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 =

ΔS_surr = 959.73 J mol^–1 K^–1

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Calculate the entropy change in surroundings when 1.00 mol of $H_{2} O_{(l)}$ is formed under standard conditions. $Δ_{f} H^{θ} = - 286 k J m o l^{- 1}$ .

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

It is given that 286 kJ mol–1 of heat is evolved on the formation of 1 mol of H2O(l). Thus, an equal amount of heat will be absorbed by the surroundings. qsurr = +286 kJ mol–1 Entropy change (ΔSsurr) for the surroundings = ΔSsurr = 959.73 J mol–1 K–1

Calculate the entropy change in surroundings when 1.00 mol of H₂O₍_l₎ is formed under standard conditions. Δ_fH^θ = –286 kJ mol^–1.

It is given that 286 kJ mol^–1 of 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 =

ΔS_surr = 959.73 J mol^–1 K^–1