For N2(g) + O2(g) (Equilibrium arrows) 2NO(g) The equilibrium constant, Kp for t

Question

For N2(g) + O2(g) (Equilibrium arrows) 2NO(g)

The equilibrium constant, Kp for the reaction is .0025 at 2127 degrees C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

The answer is 7.8 atm

Soooo, I made a table with Initial pressures, change in pressures and equilibrium pressures, then tried to solve for x using the quadratic equation but am clearly missing something, because I didn't come close to the answer. ?? Help and EXPLAINATIONS of STEPS PLEASE, particularly with the math.

Thank you!!

Explanation / Answer

N?(g) + O?(g) <------> 2 NO(g)
=>
Kp = (p(NO))

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