Calculating Equilibrium Constants

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Dustin Shin 2I
Posts: 64
Joined: Fri Sep 28, 2018 12:26 am

Calculating Equilibrium Constants

Postby Dustin Shin 2I » Wed Jan 23, 2019 5:20 pm

In the ICE charts, how are the number of x's determined for each different molecule when calculating the Change in Molarity? Is it determined by the number of moles of the substance in the given equation? I am confused.

Hovik Mike Mkryan 2I
Posts: 95
Joined: Fri Sep 28, 2018 12:25 am

Re: Calculating Equilibrium Constants

Postby Hovik Mike Mkryan 2I » Wed Jan 23, 2019 5:27 pm

For the ICE table the amount that changes to reach equilibrium is denoted by x for both the products and reactants. If the sample problem was 2A + 3B ----> 3C and we were given the initial concentrations for A and B at both 0.1, then we would do 0.1-2x for A and 0.1-3x for B. For C it's initial would be 0 and it would follow with a +3x. Hope this helped!

Gillian Murphy 2C
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

Re: Calculating Equilibrium Constants

Postby Gillian Murphy 2C » Wed Jan 23, 2019 5:30 pm

Yes- in an ice table, the number of x's you put for the change is the same as the amount in the equation. For example, in the equation "N2 + 3H2 = 2NH3", you would subtract 1x from N2, 3x from H2, and add 2x to NH3. Logically, this makes sense because in a reaction, 1 molecule of N2 will combine with 3 molecules of H2 and be lost in order to create 2 new NH3 molecules.

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