The value of the equilibrium constant, Kc, at a certain temperature is 2.56 x 10-1. If the reaction quotient for a mixture of these species at the same temperature is found to be 9.90 x 10-4, would the mixture yield more products, more reactants or is it at or near equilibrium? Assume a reaction quotient within a factor of 10 of the equilibrium constant is at equilibrium. Enter P, R or EQ.

Question

The value of the equilibrium constant, Kc, at a certain temperature is 2.56 x 10-1. If the reaction quotient for a mixture of these species at the same temperature is found to be 9.90 x 10-4, would the mixture yield more products, more reactants or is it at or near equilibrium? Assume a reaction quotient within a factor of 10 of the equilibrium constant is at equilibrium. Enter P, R or EQ.

CH4(g)+H2O(g) = CO(g)+3H2(g)

Answer 1

This is much like the problem above that wanted to know were products are reactants favored. Here you compare K with Q

Answer 2

To determine whether the mixture would yield more products, more reactants, or if it is at or near equilibrium, we need to compare the reaction quotient (Qc) to the equilibrium constant (Kc).

Given:
Kc = 2.56 x 10^(-1)
Qc = 9.90 x 10^(-4)

If the value of Qc is significantly smaller than Kc, it means that there are more reactants relative to products in the mixture. In this case, Qc is smaller than Kc, as 9.90 x 10^(-4) is much smaller than 2.56 x 10^(-1).

Since Qc is smaller than Kc, the mixture is expected to yield more products.