## Equilibrium Constants

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Eric Quach 1C
Posts: 30
Joined: Fri Sep 28, 2018 12:20 am

### Equilibrium Constants

For the equilibrium constant K, how does changing the coefficients in the chemical reaction affect K?
For example, how does doubling each coefficient change the value of K?

Tuong Nguyen 2I
Posts: 71
Joined: Fri Sep 28, 2018 12:26 am
Been upvoted: 1 time

### Re: Equilibrium Constants

If you double the moles of a certain molecule/atom in a chemical reaction, you'll have to take that coefficient and use it as the exponent for the concentration of that respective molecule/atom in the equilibrium constant.

Jennifer Su 2L
Posts: 47
Joined: Wed Nov 21, 2018 12:20 am

### Re: Equilibrium Constants

This will depend on whether you are changing the coefficient of a reactant or product. Let's say the equilibrium equation has aA and bB as the reactants, and cC as the product, with the lowercased letters representing the coefficients. Therefore, K=(partial pressure of C)^c/(partial pressure of A)^a * (partial pressure of B)^b. If you were to increase the coefficient "c", then the numerator will become significantly larger, so K will be larger. If you were to increase the coefficients "a" or "b", then the denominator will become significantly larger, so K will become smaller.

But since these are equilibrium equations, I don't think you can just change one coefficient without having to change all of the other coefficients. In other words, if you increase one coefficient, you will probably have to increase all the other coefficients as well and so you'll end up with the same K. (correct me if I'm wrong)

105085381
Posts: 44
Joined: Fri Sep 28, 2018 12:15 am

### Re: Equilibrium Constants

By doubling the the number of moles of a specific molecule, do the coefficients and exponents work proportional to one another in order to maintain the equilibrium of K?

taryn_baldus2E
Posts: 62
Joined: Fri Sep 28, 2018 12:24 am

### Re: Equilibrium Constants

These will impact the equilibrium constant because K is the ration of products divided by reactants. The concentration of each component is then multiplied by its stoichiometric coefficient, causing a change to the ratio itself from what would be expected if the coefficients were one.