# Problem: 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?

###### FREE Expert 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:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{products}}}{{\mathbf{P}}_{\mathbf{reactants}}}}$     $\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{\left[}\mathbf{products}\mathbf{\right]}}{\mathbf{\left[}\mathbf{reactants}\mathbf{\right]}}}$

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

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###### Problem Details

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?