For the following reaction Kp = 4.796 at a given temperature. 2NO(g) + Cl2(g) <==> 2NOCl (g) At equilibrium PNO = 8.647 x 10-1 and PCl2 = 4.387 x 10-1. What is the equilibrium partial pressure of NOCl(g)?

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For the reaction

`2NO + Cl_2 -gt 2 NOCl `

the equilibrium constant expression Kp is:

`K_p = ((P_(NOCl))^2)/(((P_(NO))^2)(P_(Cl_2)))` 

The P's in the expression represent the partial pressures of the indicated gases. Partial pressure is used instead of molarity to express the concentration of gases when calculating the pressure equilibrium...

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For the reaction

`2NO + Cl_2 -gt 2 NOCl `

the equilibrium constant expression Kp is:

`K_p = ((P_(NOCl))^2)/(((P_(NO))^2)(P_(Cl_2)))` 

The P's in the expression represent the partial pressures of the indicated gases. Partial pressure is used instead of molarity to express the concentration of gases when calculating the pressure equilibrium constant Kp.

We can solve this by substituting the given values and letting x equal the partial pressure of NOCl:

`4.796 = (x^2)/((0.8647)^2(0.4387))`

`x^2 = (4.796)(0.8647)^2(0.4387) = 1.573`

`x` = `sqrt(1.573) = 1.254 = P_(NOCl)`

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