5J.1

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Phuong Tran 1G
Posts: 33
Joined: Sat Sep 14, 2019 12:16 am

5J.1

Postby Phuong Tran 1G » Mon Feb 10, 2020 7:17 pm

Consider the equilibrium CO(g) 1 H2O(g) ∆CO2(g) 1 H2(g). (a) If the partial pressure of CO2 is increased, what happens to the partial pressure of H2? (b) If the partial pressure of CO is decreased, what happens to the partial pressure of CO2? (c) If the concentration of CO is increased, what happens to the concentra- tion of H2? (d) If the concentration of H2O is decreased, what happens to the equilibrium constant for the reaction?

Can someone explain the answers?
Would a be partial pressure of H2 going down to adjust for the increase?
Would b be partial pressure of CO2 going down?
I’m confused for c
For D, the equilibrium reaction would shift to the left favoring reactants but equilibrium constant Kc will not change.

Ryan Chang 1C
Posts: 105
Joined: Sat Aug 24, 2019 12:17 am

Re: 5J.1

Postby Ryan Chang 1C » Mon Feb 10, 2020 9:32 pm

The equilibrium constant K always remains constant, so any change in the values of the reactants has to be accounted for by another change.
A) H2 decreases to account for the increase in CO2. This is because the value of the products (numerator) has to remain constant.
B) CO2 will decrease to account for the decrease in CO, because the ratio of products to reactants must remain constant.
C) Similar to B, H2 will increase to account for the increase in CO, because the ratio of products to reactants must remain constant.
D) You are correct for part D because no matter what happens to the values of the reactants and/or products, K remains constant.


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