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Clara Cho 2K
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Joined: Wed Sep 18, 2019 12:18 am


Postby Clara Cho 2K » Wed Jan 08, 2020 11:25 am

How does increasing the concentration of reactants increase the equilibrium concentration of products?

Jason Wu 1E
Posts: 101
Joined: Thu Jul 25, 2019 12:15 am

Re: Concentration

Postby Jason Wu 1E » Wed Jan 08, 2020 12:19 pm

Because the value of K is constant from the ratio of the concentration of products over reactants. By increasing the equilibrium concentration of reactants, it will then increase the equilibrium concentration of the products in order to drive the reaction forward. This will then decrease the concentration of reactants until the equilibrium constant is reached.

Joseph Saba
Posts: 154
Joined: Thu Jul 11, 2019 12:16 am

Re: Concentration

Postby Joseph Saba » Wed Jan 08, 2020 12:19 pm

When you increase the concentration of a reactant, the reaction must shift left in order to balance out the change in the reaction.

Miriam Villarreal 1J
Posts: 105
Joined: Sat Aug 17, 2019 12:16 am

Re: Concentration

Postby Miriam Villarreal 1J » Wed Jan 08, 2020 10:11 pm

According to Le Chatelier's principle, adding additional reactant to a system will shift the equilibrium to the right, towards the side of the products because the frequency of successful collisions of that reactant would increase, allowing for an increase in the forward reaction, and thus the generation of the product

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