Lexan is a plastic used to make compact discs, eyeglass lenses, and bullet-proof glass. One of the compounds used to make Lexan is phosgene (COCly), an extremely poisonous gas. Phosgene decomposes by the reaction Coch(o) CO(g)+Cla (9) for which K, 6.8 x 10- at 100°C. If pure phosgene at an initial pressure of 4 8 atm decomposes, calculate the equilibrium pressures of all species Partial pressure of COCh- Partial pressure of co- Partial pressure of Cla atm atm atm

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Annainn Annainn · Answer 1 · 2019-08-14T08:59:22+02:00

Answer:

p[CO] = 1.81*10⁻⁴ atm

p[Cl2] = 1.81*10⁻⁴ atm

p[COCl2] = 4.8 atm

Explanation:

Given:

Pressure of phosgene, COCl2 = 4.8 atm

Kp = 6.8*10^-9

To determine:

The equilibrium partial pressures of COCl2, Cl2, CO

Calculation:

Set-up an ICE table for the given reaction:

[tex]COCl2(g)\rightleftharpoons CO(g)+Cl2(g)[/tex]

I 4.8 0 0

C -x +x +x

E (4.8-x) x x

[tex]Kp = \frac{[CO][Cl2]}{[COCl2]}\\\\6.8*10^{-9} =\frac{(x)^{2} }{4.8-x} \\\\x = 0.000181 atm[/tex]

The equilibrium partial pressures are:

p[CO] = x = 1.81*10⁻⁴ atm

p[Cl2] = x = 1.81*10⁻⁴ atm

p[COCl2] = 4.8-x =4.8- 1.81*10⁻⁴ atm = 4.8 atm