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.

0.28 M

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

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Moles at eq:    2.00-2x                        x                      x

The expression for the equilibrium constant is:

So,

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

thats a little if u want the answer just look it up on google thats what i do haha : )