Nitrogen monoxide can be synthesized by combining nitrogen and oxygen under certain conditions: N2(g) + O2(g)...

 

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Nitrogen monoxide can be synthesized by combining nitrogen and oxygen under certain conditions: N2(g) + O2(g) = 2NO(g) At 1500K, the reaction has an equilibrium constant of 1.10x10-5. If air is pumped into a reaction vessel up to a pressure of 85.0 atm, what will be the partial pressure of NO at equilibrium? (Assume that air is 80% nitrogen and 20% oxygen). Nitrogen monoxide can be synthesized by combining nitrogen and oxygen under certain conditions: N2(g) + O2(g) = 2NO(g) At 1500K, the reaction has an equilibrium constant of 1.10x10-5. If air is pumped into a reaction vessel up to a pressure of 85.0 atm, what will be the partial pressure of NO at equilibrium? (Assume that air is 80% nitrogen and 20% oxygen).