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shtirl [24]
3 years ago
7

Nitric oxide reacts with chlorine gas according to the reaction: 2 NO( g) + Cl2( g) ∆ 2 NOCl( g) Kp = 0.27 at 700 K A reaction m

ixture initially contains equal partial pressures of NO and Cl2. At equilibrium, the partial pressure of NOCl is 115 torr. What were the initial partial pressures of NO and Cl2 ?
Chemistry
1 answer:
11Alexandr11 [23.1K]3 years ago
8 0

Answer:  The initial partial pressures of NO and Cl_2 is 139.4 torr.

Explanation:

The equilibrium reaction is

                           2NO(g)+Cl_2(g)\rightleftharpoons 2NOCl(g)

initially conc.         p            p                  0

At eqm.                p-2x        p-x               2x

Given: p_{NOCl}= 2x= 115torr

x=57.5 torr

The expression for equilibrium constant is :

K_p=\frac{p_{NOCl}^2}{p_{NO}^2\times p_{Cl_2}}

p_{NOCl} = 2x =115 torr

p_{NO} = (p-2x) = p-115 torr

p_{Cl_2} = (p-x)= p-57.5 torr

Now put all the given values in this expression, we get

0.27=\frac{(115)^2}{(p-115)^2\times (p-57.5)}

p=139.4torr

Therefore, the initial partial pressures of NO and Cl_2 is 139.4 torr.

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