Given that the reaction quotient, Q, for a given system is greater than the equi

Question

Given that the reaction quotient, Q, for a given system is greater than the equilibrium constant K, in which direction will the reaction spontaneously, predominantly proceed? The reaction will proceed predominantly towards the reactants side. The rates of both the forward and reverse reactions will increase to reestablish equilibrium as quickly as possible. The reaction will proceed predominantly towards the products side. The reaction has reached a new dynamic equilibrium and both the forward and reverse reactions will proceed at identical rates. There is not enough information given to determine the predominant direction of the reaction.

Explanation / Answer

if Q>K then, the reaction moves in the reverse direction, coverting the products to reactants.

hence, The reaction proceed towards reactant side. (option A)

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