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Luyan Zhang - 2D
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Joined: Sat Jul 20, 2019 12:16 am


Postby Luyan Zhang - 2D » Thu Jan 09, 2020 8:32 pm

A gaseous mixture consisting of 2.23 mmol N2 and 6.69
mmol H2 in a 500.-mL container was heated to 600. K and
allowed to reach equilibrium. Will more ammonia be formed if
that equilibrium mixture is then heated to 700. K?

How would we do this problem if we didn't know that this reaction is exothermic?

Baoying Li 1B
Posts: 113
Joined: Sat Aug 17, 2019 12:18 am

Re: 5J.13

Postby Baoying Li 1B » Thu Jan 09, 2020 8:38 pm

You can compare the equilibrium constants of this reaction under different temperatures to see whether the reaction is exothermic or endothermic. If the equilibrium constant in the lower temperature is higher than the equilibrium constant in the higher temperature, the reaction is exothermic. The opposite result will make this reaction endothermic.

Posts: 107
Joined: Fri Aug 09, 2019 12:17 am

Re: 5J.13

Postby JChen_2I » Sat Jan 11, 2020 9:27 pm

The problem also tells you that K=7.8*10^-5 at 700K which is less than K at 600K. Therefore more ammonia (the product) would be formed at 600K since a greater K value means a greater ratio of products to reactants.

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