Initial Concentration and Equilibrium Concentration

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Nathan Mariano 2G
Posts: 68
Joined: Fri Sep 28, 2018 12:29 am

Initial Concentration and Equilibrium Concentration

Postby Nathan Mariano 2G » Sat Mar 09, 2019 10:26 pm

"If one starts with higher concentrations of reactants, the equilibrium concentrations of the products will be larger." Why is this statement true? Can there be a case where the equilibrium concentration of the product is smaller than the initial concentration of the reactants?

Sara Flynn 2C
Posts: 60
Joined: Fri Sep 28, 2018 12:23 am

Re: Initial Concentration and Equilibrium Concentration

Postby Sara Flynn 2C » Sat Mar 09, 2019 10:40 pm

I think it just means that if you have more reactant initially then compared to how much product would be formed if you had less reactant there would be more. Like if you had 2 moles of reactant and it made 3 moles of product, if you had 4 moles of reactant then it would make 6 moles of product.

Gary Qiao 1D
Posts: 66
Joined: Fri Sep 28, 2018 12:26 am

Re: Initial Concentration and Equilibrium Concentration

Postby Gary Qiao 1D » Sun Mar 10, 2019 1:03 am

I'm guessing that the question is kind of talking about how relative to the equilibrium concentration, when there is more initial concentration, then the reaction tends to favor the products in order to reach the equilibrium concentrations. So there probably is a case where the product is smaller than the initial concentration of reactants.

KimGiang2F
Posts: 31
Joined: Fri Sep 28, 2018 12:19 am

Re: Initial Concentration and Equilibrium Concentration

Postby KimGiang2F » Tue Mar 12, 2019 4:14 am

Although adding a reactant increases the concentration of products at equilibrium, the increase in product concentration won't necessarily mean that the equilibrium product concentration becomes higher than that for the reactants. If K is bigger than one, the equilibrium concentration of the products will be greater than that for the reactants. If K is less than one, the equilibrium concentration of the reactants is bigger.


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