# Problem: A mixture of 1.00 atm of NO, 0.50 atm of H 2, and 1.00 atm of N2 was allowed to reach equilibrium according to the reaction given below (initially there was no H2O). At equilibrium, the partial pressure of NO was found to be 0.62 atm. Determine the value of the equilibrium constant, Kp, for the reaction: 2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g) a) 6.08 b) 31.0 c) 215.0 d) 26.5 e) 651.0

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A mixture of 1.00 atm of NO, 0.50 atm of H 2, and 1.00 atm of N2 was allowed to reach equilibrium according to the reaction given below (initially there was no H2O). At equilibrium, the partial pressure of NO was found to be 0.62 atm. Determine the value of the equilibrium constant, Kp, for the reaction:

2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g)

a) 6.08

b) 31.0

c) 215.0

d) 26.5

e) 651.0

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Based on our data, we think this problem is relevant for Professor Reck & Snaddon's class at IU.