CBSE (Science) Class 11CBSE
Share
Notifications

View all notifications

Calculate the Entropy Change in Surroundings When 1.00 Mol of H2o(L) Is Formed Under Standard Conditions. - CBSE (Science) Class 11 - Chemistry

Login
Create free account


      Forgot password?

Question

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

Solution 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 = `q_"surr"/7`

`= (286 kJ mol^(-1))/298 k`

∴ ΔSsurr = 959.73 J mol–1 K–1

Solution 2

`q_"rev" = (-triangle_f H^(Theta)) = - 286 kJ mol^(-1) = 286000 J mol^(-1)`

`triangleS_(("Surroundings")) = q_"rev"/T = (286000 J mol^(-1))/(298 K) = 959 J K^(-1) mol^(-1)`

  Is there an error in this question or solution?

APPEARS IN

Solution Calculate the Entropy Change in Surroundings When 1.00 Mol of H2o(L) Is Formed Under Standard Conditions. Concept: Enthalpy Change, ∆_rH of a Reaction - Reaction Enthalpy - Standard Enthalpy of Reactions.
S
View in app×