Question

The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting concentrations of reactants and/or products are known. Part A Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction 2COF2(g)⇌CO2(g)+CF4(g), Kc=8.80 If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium? Express your answer with the appropriate units.

Answer 1

0.28 M

Step-by-step explanation:

Concentration of [COF₂] = 2.00 M

Considering the ICE table for the equilibrium as:

2COF₂ (g) ⇔ CO₂ (g) + CF₄ (g)

t = o 2.00

t = eq -2x x x

--------------------------------------------- --------------------------

Moles at eq: 2.00-2x x x

The expression for the equilibrium constant is:

`K_c=\frac {[CO_2][CF_4]}{[COF_2]^2}=8.80`

So,

`(x^2)/((2.00-2x)^2)=8.80`

Solving for x, we get that

x = 0.86 M

Equilibrium concentrations :

[CO₂] = [CF₄] = 0.86 M

[COF₂] = 2.00 - 2*0.86 = 0.28 M