We’re being asked to **determine the equilibrium partial pressure of NOCl.**

We are given the equation:

**2 NO _{(g)} + Cl_{2}_{(g)} ↔ 2 NOCl**

Recall that the ** equilibrium constant** is the ratio of the products and reactants.

We use **K _{p}** when dealing with pressure and

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

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

For the following reaction, K_{p} = 8,532 at a given temperature.

2 NO(g) + Cl_{2}(g) <=> 2 NOCl(g)

At equilibrium, P_{NO} = 0.734 and P_{Cl2} = 0.303. What is the equilibrium partial pressure of NOCl?

Give your answer to 3 significant figures.

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