# Problem: The equilibrium2NO (g) + Cl2 (g) 2NOCl (g)is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 9.50×10−2 atm , 0.175 atm , and 0.27 atm for NO, Cl2, and NOCl, respectively.Calculate Kp for this reaction at 500.0 K.

###### FREE Expert Solution

We’re being asked to determine Kp at 500 K for this reaction:

2NO (g) + Cl2 (g) 2NOCl (g)

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

We use Kp when dealing with pressure.

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}\frac{{\mathbf{P}}_{\mathbf{products}}}{{\mathbf{P}}_{\mathbf{reactants}}}}$

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

79% (487 ratings) ###### Problem Details

The equilibrium
2NO (g) + Cl2 (g) 2NOCl (g)
is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 9.50×10−2 atm , 0.175 atm , and 0.27 atm for NO, Cl2, and NOCl, respectively.

Calculate Kp for this reaction at 500.0 K.