## Adding reactions

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205150314
Posts: 106
Joined: Wed Feb 20, 2019 12:16 am

### Adding reactions

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

Jasmine Fendi 1D
Posts: 108
Joined: Sat Aug 24, 2019 12:15 am

### Re: Adding reactions

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

Isha_Maniyar_Dis2E
Posts: 110
Joined: Thu Jul 11, 2019 12:16 am

### Re: Adding reactions

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
Posts: 102
Joined: Thu Jul 11, 2019 12:17 am

### Re: Adding reactions

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.

CosetteBackus_4F
Posts: 23
Joined: Wed Feb 20, 2019 12:18 am

### Re: Adding reactions

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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