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Postby Megan_Ervin_1F » Tue Jan 08, 2019 11:31 am

Why is it that if you start out with an initial larger value of reactants, the products will be favored at equilibrium?

Madeline Ho 1C
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Joined: Mon Apr 23, 2018 3:00 am

Re: Concentrations

Postby Madeline Ho 1C » Tue Jan 08, 2019 12:52 pm

If I understand it correctly, products will be favored at equilibrium if you increase the amount of reactant when the reaction is at equilibrium in order to minimize the effect of adding more reactant; the forward reaction is favored, producing more product. Initial concentrations of reactants or products do not necessarily tell you whether or not the reactant/product is favored at equilibrium.

Cody Do 2F
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Re: Concentrations

Postby Cody Do 2F » Tue Jan 08, 2019 1:13 pm

Something that helps me figure out which side of the equation is favored is to visualize the equation as a tub of water. If you add more water to the left side (adding more of a reactant), then the water will move to the right side (favor the products) in order to reach equilibrium. The opposite is true if you add more water to the left side (adding more product) which will cause water to move to the left side (favoring the reactants). If you take water away from the left side (remove reactants), then water from the right side will move to the left in order to fill in the hole (favoring more reactants) and vice versa.

Brian Hom 2F
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Re: Concentrations

Postby Brian Hom 2F » Tue Jan 08, 2019 1:29 pm

According the Le Chatelier's Principle, when there is a high concentration of reactants, you favor the forward reaction. For the solution to reach its equilibrium it must make more of the product.

Sydney To 1D
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Re: Concentrations

Postby Sydney To 1D » Tue Jan 08, 2019 2:07 pm

In regards to amount/number of moles, I like to visualize Le Chatelier's Principle like a seesaw. Let's say the left of the seesaw are the reactants and the right of the seesaw are the products. Increasing the amount of reactant leaves the seesaw tilted, having more weight on the left side. In order to achieve an equilibrium (seesaw is neutral and a horizontal line), more products are formed and is favored in the forward reaction.

Ian Marquez 2K
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Re: Concentrations

Postby Ian Marquez 2K » Tue Jan 08, 2019 3:04 pm

Like the replies above, it is very helpful to view these changes visually. Similarly, it's helpful to think of adding reactants or products to a reaction at equilibrium as tipping a scale or seesaw. In order to react to this increase, either the forward or reverse reaction is favored to even everything out.

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