The standard potential Eo
is related to equilibrium constant K
by the following relation:
In a reaction occurring at standard state conditions, if the concentrations of the products are greater than that of the reactants, which of the following is true?
|A|| K is negative|
|B|| Eo is negative|
|C|| The reaction is nonspontaneous|
|D|| None of the above|
Ans. D Based on the given information in the question, we can say that Eo is directly related to K. The question also says that the product concentrations are greater than the reactant concentrations. So we can say that the equilibrium constant value is greater than 1. We can rule out Choice A, because there is no such thing as a negative concentration. So K cannot be negative anyway. Since we know that K is greater than 1, the natural logarithm of K will be positive. So from the equation, we can say that Eo cannot be negative, which rules out Choice B. Hence, the Eo value should be positive. Since we have a positive Eo value, the reaction is most likely to be spontaneous. Keep in mind the conditions at which the reaction occurs - standard state (1 atm, 25 oC).