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Q is calculated the same was as K with products/reactants, but Q is the value not at equilibrium. In respect to the equilibrium constant K, if Q<K, this means the concentration of reactants is greater than the concentration of products, so forward reaction is favored to reach equilibrium. If Q>K, this means the concentration of products is greater than the concentration of reactants so reverse reaction is favored.
Q and K are calculated in the same way. Q is calculated at any point of the reaction, but K is calculated only at equilibrium. If Q is less than K then the products are favored. If Q is less than K then the reactants are favored.
When Q>K think of drawing a little pac man guy off the greater than sign and his mouth is going towards the reactants so the reaction favors reactants and if Q<K draw the pac man going towards the products side so the reaction favors the formation of products. Silly tip but useful.
K is the reaction at equilibrium and Q is used to calculate the ratio at anytime, but they are both calculated the same way. If Q<K then the reactants are favored and will shift towards the products (forward. If Q>K then the products are favored and will shift towards the reactants (reverse).
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