Which of the following must be true about the reaction when the free energy change is zero?

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The free energy change of the reaction A(g) B(g) is zero under certain conditions. The standard free energy change of the reaction is -42.5kJ. Which of the following must be true about the reaction when the free energy change is zero? (more than one answer)

a. The concentration of the reactant is greater than the concentration of the product.
b. The concentration of the product is greater than the concentration of the reactant.
c. The reaction is at equilibrium.
d. It is impossible for the free energy change of a reaction to be different values since it is a constant.
e. The free energy would be a positive value at high temperatures.

Best reply by Rijl:

c is the only one that must be true.

a, b, and d, are false.

e is possible, but not necessarily true. You would need to know the signs of ∆H and ∆S to know.

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Which of the following must be true about the reaction when the free energy change is zero?

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