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.


Kp=PproductsPreactants 


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


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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.

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