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madisonsolis05
27.02.2020 •
Chemistry
Be sure to answer all parts. Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0500 M, [H2] = 0.0410 M, [CO2] = 0.0880 M, and [H2O] = 0.0380 M. (a) Calculate Kc for the reaction at 686°C.(b) If we add CO2 to increase its concentrationto 0.30 mol/L, what will theconcentrations of all the gases be when equilibrium isreestablished?
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Ответ:
a)The equilibrium constant at 686°C is 0.527.
b) Concentrations of all the gases be when equilibrium is reestablished:
Explanation:
a)![CO_2(g) + H_2(g)\rightleftharpoons CO(g) + H_2O(g)](/tpl/images/0526/9800/db636.png)
Equilibrium concentrations:
The value of an equilibrium constant will be given as:
The equilibrium constant at 686°C is 0.527.
b)
Initially
0.30 M 0.0410 M 0.0500 M 0.0380 M
At reestablishment of an equilibrium;
(0.30-x) M (0.0410-x) M (0.0500+x) M (0.0380+x) M
The value of an equilibrium constant will be given as:
Solving for x;
x = 0.0166
Concentrations of all the gases be when equilibrium is reestablished:
Ответ:
N = M - n (mass - number)
34 - 15 = 19
So your answer is 19
Hope it helped