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), K=7.80 at 850 K If only COF2 is present initially at a pressure of 240 kPa, what is the partial pressure of COF2 at equilibrium? You can convert the units of pressure from kPa to bar, using the relation 1 kPa=0.01 bar. Express your answer with the appropriate units.
2COF2(g)⇌CO2(g)+CF4(g) K = 7.80
Intial partial pressure of COF2 = 240 kPa = 240 x 0.01 bar = 2.4 bar
2COF2(g) ⇌ CO2(g) + CF4(g)
Initial partial pressure 2.4 bar 0 0
Equilibrium partial pressure 2.4-2X X X
Hence, Equilibrium partial pressures are
PCOF2 = 2.4-2X
PCO2 = X
PCF4 = X
K = PCO2 . PCF4 / P2COF2
7.8 = X.X / (2.4-2X)2
44.93 + 31.2 X2- 74.88 X = X2
30.2 X2- 74.88 X + 44.93 = 0
On solving, X = 1.02 bar
Hence,
Partial pressure of COF2 at equilibrium = 2.4 - 2X = 2.4 - (2x1.02) = 0.36 bar
Therefore,
partial pressure of COF2 at equilibrium = 0.36 bar
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