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

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Nathan Nakaguchi 1G
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How to interpret reactions based on quotient in relation to equilibrium constant

Postby Nathan Nakaguchi 1G » Tue Jan 07, 2020 3:19 pm

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

Postby Alicia Lin 2F » Tue Jan 07, 2020 4:43 pm

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

Postby Daniel Honeychurch1C » Tue Jan 07, 2020 4:45 pm

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

Postby HuyHa_2H » Thu Jan 09, 2020 2:52 pm

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

Postby LNgo 1G » Thu Jan 09, 2020 3:34 pm

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

Postby bellaha4F » Thu Jan 09, 2020 4:12 pm

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.


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