1
Question
Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ΔfHθ=−286 kJ mol−1.
Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ΔfHθ=−286 kJ mol−1.
Open in App
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=+286kJ mol−1
Entropy change (Δ S surr) for the surroundings =q surrT
=286 kJ mol−1298 k
∴ Δ S surr=959.73Jmol−1K−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=+286kJ mol−1
Entropy change (Δ S surr) for the surroundings =q surrT
=286 kJ mol−1298 k
∴ Δ S surr=959.73Jmol−1K−1
Suggest Corrections
83
Similar questions