We’re being asked to determine the equilibrium partial pressure of NOCl.
We are given the equation:
2 NO(g) + Cl2(g) ↔ 2 NOCl(g)
Recall that the equilibrium constant is the ratio of the products and reactants.
We use Kp when dealing with pressure and Kc when dealing with concentration:
Note that solid and liquid compounds are ignored in the equilibrium expression.
For the following reaction, Kp = 8,532 at a given temperature.
2 NO(g) + Cl2(g) <=> 2 NOCl(g)
At equilibrium, PNO = 0.734 and PCl2 = 0.303. What is the equilibrium partial pressure of NOCl?
Give your answer to 3 significant figures.
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