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The reaction CH2Cl2 (g) --> CH4 (g) + CCl4 (g) has Kp = 1.33 at 400K....

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Chemistry

The reaction CH2Cl2 (g) --> CH4 (g) + CCl4 (g) has Kp = 1.33at 400K. A 5.00L reaction vessel is evacuated, and 15.00 g ofCH2Cl2 (l) is added to the flask. The CH2Cl2 (l) rapidly vaporizesand the reaction starts. a. What will be all of the partialpressures of the gases when equilibrium is reached? b. Sketch agraph showing the initial concentration of each gas and how theychange as the mixture approaches equilibrium. Set-up your graph sothat equilibrium is reacched two thirds of the way from the startto the end of the graph

Answer & Explanation Solved by verified expert
4.1 Ratings (509 Votes)

[CH2Cl2] = 15.00 / (85 * 5) = 0.0353 M

PCH2Cl2 = [CH2Cl2] R T = 0.0353*0.0821*400 = 1.16 atm

CH2Cl2 (g) --> CH4 (g) + CCl4 (g)

1.16 atm            0 atm           0 atm                 Initial

1.16 - x               x                   x                       Equilibrium

Kp = PCH4 * PCCl4 / PCH2Cl2

1.33 = x * x / (1.16 - x)

1.54 - 1.33 x = x2

x2 + 1.33 x - 1.54 = 0

Solving quadratic equation

x = [ - 1.33 +/- (1.77 + 6.16)1/2 ] / 2 = 0.743 atm

At equilibruim,

PCH2Cl2 = 1.16 - 0.743 = 0.417 atm

PCH4 = PCl2 = 0.743 atm
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