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Q and K are similar in the sense that they are calculated the same way with products divided by reactants. They are different however with K being the equilibrium constant and Q being the reaction quotient. Q happens at any time during the reaction and K is the overall equilibrium
They are similar to each other as the calculation of products divided by reactants is the same. The main difference is that k occurs at equilibrium while q occurs before equilibrium is reached. By calculating Q and comparing it to K, we can tell which way the reaction is going more towards.
Q and K are calculated using the same rules and formula. However Q is used when you are given initial concentration/pressure values, and K is used when you are given equilibrium concentration/pressure values. You can compare Q and K to determine in which direction the reaction will proceed.
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