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### Q vs K

Posted: Thu Jan 09, 2020 3:15 pm
What's the difference between Q and K?

### Re: Q vs K

Posted: Thu Jan 09, 2020 3:16 pm
K is the ratio of products to reactants at equilibrium, while Q is the ratio of products to reactants at any given point in the reaction (not necessarily equilibrium).

### Re: Q vs K

Posted: Thu Jan 09, 2020 3:17 pm
K is the constant you get for the ratio of the concentration of products at equilibrium to the concentration of reactants at equilibrium. Q is the ratio of products to reactants at any time. Q is used as a point of comparison to K to determine which direction the reaction will proceed to reach equilibrium.

### Re: Q vs K

Posted: Thu Jan 09, 2020 3:17 pm
K is the ratio of products over reactants at equilibrium, Q is the same thing not at equilibrium

### Re: Q vs K

Posted: Thu Jan 09, 2020 4:08 pm
Q is used when the reaction is not at equilibrium and K is the ratio of products to reactant when the system is at equilibrium.

### Re: Q vs K

Posted: Thu Jan 09, 2020 4:15 pm
Q and K are calculated the same but Q is the value at any point during the reaction while K is the value at equilibrium.

### Re: Q vs K

Posted: Thu Jan 09, 2020 4:23 pm
If Q is less than K at some time during the reaction, then compared to the equilibrium concentrations [R] > [P] and the forward reaction is favored, and vice versa.

### Re: Q vs K

Posted: Thu Jan 09, 2020 6:14 pm
Q is used to evaluate the concentration of reactants and products at any given point in a reaction. If Q = K, then the reaction is in equilibrium at that time. If Q>K, then that means there are more reactants present at that time than there would be if the reaction was in equilibrium. If Q<K, that means that there are more products at that point than there would be if the reaction was in equilibrium.