Question

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) <--> 2NO(g) The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a 2.00 L container is charged with 5.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, (i) what will be the equilibrium partial pressure of nitrogen, PN2, and (ii) how many grams of O2(g) are present at equilibrium? (HINT: Set up an ICE table; R = 0.08206 L.atm/mol.K)

PN2 = atm ; Mass of O2 at equilibrium = g

Answer 1

Here is the Solution:

Thanks! :-)