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?

a)The equilibrium constant at 686°C is 0.527.

b) Concentrations of all the gases be when equilibrium is reestablished:

Explanation:

a)

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:

h let me think

pie chart because it is in percents ( % )