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Q is the reaction quotient. By comparing this value to K, we can determine how the reaction will progress. If Q<K, the formation of products will be favored. If Q>K, the formation of reactants will be favored. If Q=K, then the reaction is at equilibrium.
Q is the ratio of the products and the reactants with the initial concentrations or whatever data the problem gives you, whereas K is the equilibrium concentration for the reaction, which does not change with changes to pressure and concentration, however it does change with change to temperature.
To expand and clarify, Q and K are calculated the same way. The only difference is the value found for K will be the constant value at equilibrium. Using the same math, you can calculate the reaction quotient (Q) but for any point in the reaction (not necessarily when the reaction is at equilibrium).
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