Given the reaction A<-->B and using ∆Go = -RTln(Keq). (Useful calculations: ln1=0, ln<1=negative, ln>1=positive; R = 8.314 J/mol K; T = 298 K) (A) If the product concentration equaled 1M and the reactant concentration equaled 2M at equilibrium, calculate ∆Go (B) Given that ΔG reaction = ΔG˚ + RTln(Keq), calculate ΔG when the product concentration is 0.5 M and the reactant concentration is 1.5 M. Is this reaction spontaneous or not? Why? (C) Calculate ΔG when the product concentration is 1.5 M and the reactant concentration is 0.5 M. Is this reaction spontaneous or not? Why?
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Given the reaction A<-->B and using ∆Go = -RTln(Keq). (Useful calculations: ln1=0, ln<1=negative, ln>1=positive; R = 8.314 J/mol K; T = 298 K)
(A) If the product concentration equaled 1M and the reactant concentration equaled 2M at equilibrium, calculate ∆Go
(B) Given that ΔG reaction = ΔG˚ + RTln(Keq), calculate ΔG when the product concentration is 0.5 M and the reactant concentration is 1.5 M. Is this reaction spontaneous or not? Why?
(C) Calculate ΔG when the product concentration is 1.5 M and the reactant concentration is 0.5 M. Is this reaction spontaneous or not? Why?
Answer:
Ratio of molar concentrations of products and reactants is equal to reaction quotient and when system is at equilibrium this reaction becomes equal to equilibrium constant.
Given data:
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