Consider the following reaction: I2(g)+Cl2(g)2ICl(g), K p=81.9 (at 25C) A reacti

Question

Consider the following reaction:

I2(g)+Cl2(g)2ICl(g),Kp=81.9 (at 25C)

A reaction mixture at 25C initially contains PI2 = 0.120 atm , PCl2 = 0.120 atm , and PICl = 0.00 atm.

1) Find the equilibrium partial pressure of I2 at this temperature.

2) Find the equilibrium partial pressure of Cl2 at this temperature.

3) Find the equilibrium partial pressure of ICl at this temperature.

Q2:

Part A

Find the equilibrium concentration of [S2].

hydrogen disulfide: 2H2S(g)2H2(g)+S2(g),
Kc = 1.67×107 at 800C
A 0.500 L reaction vessel initially contains 6.25×102 mol of H2S and 0.113 mol of H2 at 800C.
You may want to reference ( pages 693 - 702) Section 15.8 while completing this problem.

Part A

Find the equilibrium concentration of [S2].

Explanation / Answer

I2(g)   +    Cl2(g)   <-----> 2 ICl(g)
0.120           0.120                     0       (initial)
0.120-x        0.120-x                2x    (at equilibrium)

Kp = (p(ICl))^2 /{p(I2)*p(Cl2)}
81.9 = (2x)^2 / (0.120-x)^2
sqrt (81.9) = (2x)/(0.120-x)
(2x)/(0.120-x) = 9.05
2x = 1.09 - 9.05*x
11.05*x = 1.09
x = 0.098 atm

1)
pressure of I2= 0.120-x = 0.120 - 0.098 = 0.022 atm

2)
pressure of Cl2= 0.120-x = 0.120 - 0.098 = 0.022 atm

3)
pressure of ICl = 2x = 2*0.098 atm = 0.196 atm

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