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If Q is less than K, there are more reactants then there should be at equilibrium so a forward reaction is favored (meaning we want to form more product. If Q is greater than K, there are more products than there should be so therefore a reverse reaction is favored (meaning we want to form more reactant to reach equilibrium)
When Q < K, that means that the ratio of products to reactants is less than it is at equilibrium, so the forward reaction is favored because by producing more products, the ratio of products:reactants will increase.
if Q is less than K, that means that there are currently more reactants than products, which means that products will continue to form until the solution reaches K, which is equilibrium. if Q is greater than K, it means that the concentrations of the products are higher than the equilibrium concentrations, so the products will continue to form the reactants until K is met again.
Kc and Kp both find the equilibrium constant for the reaction, while Qc and Qp can be calculated at any time during a reaction in order to determine which direction the reaction will proceed in. If Q < K, that means that there are more reactants (denominator) than products (numerator) at that time than there should be in order to get to equilibrium. To get to the desired number, more product and less reactant are needed, so the forward reaction is favored. If Q > K, that means that there are more products (numerator) than reactants (denominator) at that point in time than is needed for equilibrium. To get to K, more reactant and less product are needed, so the reverse reaction is favored.
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