The concentrations of reactants and products for a chemical reaction can be calc

Question

The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting

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

2COF2(g)CO2(g)+CF4(g),    Kc=4.00

Express your answer with the appropriate units.

concentrations of reactants and/or products are known.

Part A

2COF2(g)CO2(g)+CF4(g),    Kc=4.00

Express your answer with the appropriate units.

The concentrations of reactants and products for a chemical reaction can be calculated if the equilibrium constant for the reaction and the starting

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=4.00

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.

[COF2] =

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=4.00

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.

Explanation / Answer

For obtaining concentration at equilibrium, we make our BCA table:

We now use those concentrations in the constant definition:

4 = [CO2][CF4] / [COF2]2

4 = x2 / (2-2x)2

x = 4/5

Concentration of COF2 at equilibrium:

[COF2] = 2 - (2*(4/5)) = 2 - 8/5 = 2/5 = 0.4 M

2COF2 <-> CO2 + CF4 B 2 M 0 0 C -2x +x +x A 2-2x x x

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