ICE tables

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Marsenne Cabral 1A
Posts: 59
Joined: Fri Sep 28, 2018 12:19 am

ICE tables

Postby Marsenne Cabral 1A » Sat Jan 12, 2019 5:12 pm

When calculating concentrations and the stoichiometric coefficients are not one, how would one account for that? Would you square the concentrations of multiply them by the coefficients?

Alexa Tabakian 1A
Posts: 38
Joined: Fri Sep 28, 2018 12:20 am

Re: ICE tables

Postby Alexa Tabakian 1A » Sat Jan 12, 2019 5:20 pm

When the coefficient is not equal to one you would simply add the coefficient in front of the x. For example if you had 2H2 you would subtract or add 2x.

Meghanhe1l
Posts: 60
Joined: Fri Sep 28, 2018 12:17 am

Re: ICE tables

Postby Meghanhe1l » Sat Jan 12, 2019 5:42 pm

That would depend on what information you are using to find your concentration. If you are using a given k and the equilibrium concentrations of all the other reactants and products, then the coefficient would be in the exponent. If you are using an ice table, then the coefficient would be multiplied in front of x.


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