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Solution: Consider the reaction:2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 KIn a reaction mixture at equilibrium, the partial pressure of NO is 126 torr and that of Br2 is 159torr .What is the partial pressure of NOBr in this mixture?

Problem

Consider the reaction:

2NO(g)+Br2(g)⇌2NOBr(gKp=28.4 at 298 K

In a reaction mixture at equilibrium, the partial pressure of NO is 126 torr and that of Br2 is 159torr .

What is the partial pressure of NOBr in this mixture?

Solution

We’re being asked to determine the equilibrium partial pressure of NOBr for the reaction:


2NO(g) + Br2(g) ⇌ 2NOBr(g) Kp = 28.4 at 298 K


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:


Kp=PproductsPreactants     Kc=[products][reactants]


Note that solid and liquid compounds are ignored in the equilibrium expression.


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