## Finding K

$K = \frac{k_{forward}}{k_{reverse}}$

Mya Majewski 1L
Posts: 89
Joined: Fri Sep 25, 2015 3:00 am

### Finding K

When given the K of the reverse reaction and concentrations of the forward. How do you find the overall K? Also, how do you know whether the reaction is favoring the products or the reactants?

Chem_Mod
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Joined: Thu Aug 04, 2011 1:53 pm
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### Re: Finding K

Could you give an example in which the problem is like what you are describing?

Charlene Tang 1B
Posts: 25
Joined: Fri Sep 25, 2015 3:00 am

### Re: Finding K

I'm going to assume the K for the overall reaction is the K for the forward reaction.

If you're given the K (equilibrium constant) for the reverse reaction, all you need to do is just 1/Kreverse to get the Kforward.

If K is large (or just >1), then concentration of the products is larger than that of the reactants (since K=[products]/[reactants]), and we can assume that product formation (or the forward reaction) is favored. If K is small (<1), then the concentration of reactants is larger than that of the products. So reactant formation is favored and the reverse reaction is favored.

Hope this helps!