Test #1 Problem #2

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

Test #1 Problem #2

Postby CosetteBackus_4F » Tue Feb 11, 2020 1:25 pm

Can anyone explain the correct way to reach the answer for problem 2 on test 1?

Carbon monoxide is a toxic gas that irreversibly binds to hemoglobin. Determine which way the reaction will shift given the initial concentrations.
CO(g) + H2O(g) -> CO2(g) + H2(g), Kc = 31.4

[CO] = 2.00M, [H2O] = 0.241M, [CO2] = 3.52M, [N2] = 4.30M

Benjamin Feng 1B
Posts: 102
Joined: Sat Sep 07, 2019 12:19 am

Re: Test #1 Problem #2

Postby Benjamin Feng 1B » Tue Feb 11, 2020 1:29 pm

You can find the equilibrium quotient given the initial conditions and compare it with equilibrium. In this case, Q = [H2][CO2]/[CO][H2O]. You can input the concentrations into it and see if it's larger or smaller than K =31.4. If larger, then there is too much product and the reaction shifts to the left to form more reactant and vise versa for smaller.

CalvinTNguyen2D
Posts: 102
Joined: Thu Jul 25, 2019 12:16 am

Re: Test #1 Problem #2

Postby CalvinTNguyen2D » Sun Feb 23, 2020 11:39 pm

With these initial concentrations and the Kc value, you are able to determine which way the reaction shifts by calculating Q. Form there, compare Q to Kc to determine the reaction direction.


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