## How to interpret reactions based on quotient in relation to equilibrium constant

Nathan Nakaguchi 1G
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Joined: Wed Sep 18, 2019 12:22 am
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### How to interpret reactions based on quotient in relation to equilibrium constant

How can you tell if more products or more reactants will be formed in a reaction based on the Q compared to K? Is there a rule? Like if Q<K it makes products?

Alicia Lin 2F
Posts: 83
Joined: Wed Sep 18, 2019 12:17 am

### Re: How to interpret reactions based on quotient in relation to equilibrium constant

Q is equal to the products raised to their coefficients divided by the reactant raised to their coefficients. It is the reaction quotient (not necessarily at equilibrium). K is the constant at equilibrium. So at equilibrium, K=Q. If Q is smaller than K, that means that there are too many reactants in comparison to products. This is because the only way to make Q smaller is to increase the denominator (reactants). The reaction has too many reactants, which shifts the reaction towards products to bring the ratio closer to K. The opposite is true for if Q is larger than K.

Daniel Honeychurch1C
Posts: 109
Joined: Thu Jul 11, 2019 12:15 am

### Re: How to interpret reactions based on quotient in relation to equilibrium constant

If K>Q, more products will be formed from the reactants to reach equilibrium. If K<Q, more reactants will be formed from the products to reach equilibrium. If K=Q, the reaction is at equilibrium.

HuyHa_2H
Posts: 100
Joined: Wed Sep 11, 2019 12:15 am

### Re: How to interpret reactions based on quotient in relation to equilibrium constant

If Q<K, then the forward reaction is favored, resulting in more product to reach equilibrium while if Q>K, then the reverse reaction is favored which results in more reactants to reach equilibrium.

LNgo 1G
Posts: 100
Joined: Sat Aug 24, 2019 12:16 am

### Re: How to interpret reactions based on quotient in relation to equilibrium constant

When Q > K there is a larger amount of products than there are at equilibrium, so the reaction will proceed in the reverse direction to use up the excess products. When Q < K there is a larger amount of reactants than there are at equilibrium, so the reaction will proceed in the forward direction to use up the excess reactants.

bellaha4F
Posts: 104
Joined: Wed Sep 18, 2019 12:20 am

### Re: How to interpret reactions based on quotient in relation to equilibrium constant

If Q=K, the reaction is at equilibrium
If Q>K, the reaction is at post-equilibrium. the reverse reaction will proceed because there's too much product or not enough reactants.
If Q<K, the reaction is a pre-equilibrium. the forward reaction will proceed because not enough product has been made yet.