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Predict in which of the following, entropy increases/decreases :
For an isolated system, ∆U = 0, what will be ∆S ?
Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ∆f H⊖ = –286 kJ mol–1.
Given the condition, ΔH = 0 for the mixing of the two gases. Explain if the diffusion of these gases into each other in the closed container is a spontaneous process or not.
(a) For an isolated system ΔU = 0; what will be ΔS? (b) For a reaction at 298 K 2A + B————->C ΔH = 400 kj mol-1 and ΔS = 0.2 kj K-1 mol-1. At what temperature will the reaction become spontaneous considering ΔH and ΔS to be constant over the temperature range?
(a) Define entropy. (b) Why is entropy a state function?
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