(a) Calculate ΔH0rxn , ΔS0rxn and ΔG0rxn for the reaction A + 3B -> 2P under standard conditions (25oC), using the following data and comment on whether the reaction is spontaneous. Standard entropy of formation ΔSf°(A) = 191.6 J.mol-1.K-1 Standard entropy of formation ΔSf° (B) = 130.7 J.mol-1.K-1 Standard entropy of formation ΔSf° (P) = 192.8 J.mol-1.K-1 Standard enthalpy of formation ΔHf° (P) = −45.9 kJ.mol-1 A and B are elements whose enthalpies of formation = 0
(a) Calculate ΔH0rxn , ΔS0rxn and ΔG0rxn for the reaction A + 3B -> 2P under standard conditions (25oC), using the following data and comment on whether the reaction is spontaneous.
Standard entropy of formation ΔSf°(A) = 191.6 J.mol-1.K-1
Standard entropy of formation ΔSf° (B) = 130.7 J.mol-1.K-1
Standard entropy of formation ΔSf° (P) = 192.8 J.mol-1.K-1
Standard enthalpy of formation ΔHf° (P) = −45.9 kJ.mol-1
A and B are elements whose enthalpies of formation = 0
(b) 0 moles of gas A and 1.0 moles of gas B are added to a 2-litre reactor which is then sealed. The reactor is maintained at a constant temperature of 25oC the following reaction occurs until equilibrium is reached: A + B ⇄ AB.
At equilibrium, there are 0.75 moles of product AB in the reactor, which is also a gas.
(i) Calculate the molarities of A, B and AB at equilibrium and the equilibrium constant Kc.
(ii) Calculate the standard Gibbs energy change for this reaction.
(iii) If some of the product (AB) is removed from the reactor such that the reaction quotient Q = 20, in which direction will the reaction proceed?
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