Adding reactions

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Adding reactions

Postby 205150314 » Thu Jan 09, 2020 10:37 pm

Why is it that when we add reactions together we multiply the K's ?

Jasmine Fendi 1D
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Re: Adding reactions

Postby Jasmine Fendi 1D » Thu Jan 09, 2020 10:40 pm

I think that is just part of the formula, but I was also wondering the same thing.

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Re: Adding reactions

Postby Isha_Maniyar_Dis2E » Thu Jan 09, 2020 10:59 pm

It's a similar concept as determining the formula for K.

For example, if you have Br2Cl2 --> Br2 + Cl2, you would write K as:

K = [Br2][Cl2] / [Br2Cl2]

Even though you're adding Br2 and Cl2 in the reaction, you multiply them in K. So, adding translates to multiplying when calculating K.

Hope this helped!

andrewcj 2C
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Re: Adding reactions

Postby andrewcj 2C » Fri Jan 10, 2020 1:20 am

When adding chemical equations, the reactants stay reactants and the products stay products. Therefore, in the combined equation, all reactants would be in the denominator and would be multiplied together. A similar logic can be applied to the products for the numerator. This is equivalent to multiplying the 2 equilibrium constants of each reaction together, assuming combined reaction takes place in an environment with a constant temperature.

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Re: Adding reactions

Postby CosetteBackus_4F » Fri Jan 10, 2020 11:52 am

When adding reactions it is almost like you are adding all the reactants on one side of the equation and all of the products on the other. Therefore, when finding the equilibrium of the added reactions, you go through the same process as you would if it was just one reaction, where the concentrations of all the products are multiplied together on the top of the ratio and the concentrations of all of the reactants are multiplied together on the bottom of the ratio. With this in mind, multiplying all of the products on top and reactants on bottom is essentially the same thing as multiplying the K values of each reaction together.

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