11.29

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Lauren Reade 3I
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Joined: Fri Sep 25, 2015 3:00 am

11.29

Postby Lauren Reade 3I » Sat Nov 07, 2015 9:47 pm

If Q=1.0 for the reaction N2(g) + O2(g) --> 2NO(g) at 25 oC, will the reaction have a tendency to form products or reactants, or will it be at equilibrium?

ConnieDo3I
Posts: 31
Joined: Fri Sep 25, 2015 3:00 am

Re: 11.29

Postby ConnieDo3I » Sun Nov 08, 2015 4:34 pm

Hey!

To find out if a reaction tends towards products or tends towards reactants, we would need to compare the reaction quotient (Q) with the equilibrium constant (K). In this case, K = 4.0 x 10^-31 (but to find this, we would have to use methods described in section 11.3, which we didn't learn). So since Q > K, the reaction will tend towards reactants.

(Think of it this way: If Q > K, Q's numerator to denominator ratio is larger in comparison to K's. That means there are more products than reactants. So to reach equilibrium, the reaction would tend towards reactants.)

Hope this helps!

SubparChemist
Posts: 27
Joined: Fri Sep 25, 2015 3:00 am

Re: 11.29

Postby SubparChemist » Thu Nov 12, 2015 6:59 pm

I got mixed up on that too, just do as the above said and treat it based only off the Q as we haven't learn the stuff yet related to Gibbs Free Energy and all that jazz.


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