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.
*Note that solid and liquid compounds are ignored in the equilibrium expression.
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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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Equilibrium Expressions concept. If you need more Equilibrium Expressions practice, you can also practice Equilibrium Expressions practice problems.
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Based on our data, we think this problem is relevant for Professor Czernuszewicz's class at UH.