At 6689 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 1.16. If the initial pressure of NO is 0.00781 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) =_______ . p(N2) = ______ . p(O2) =_______ .
At 6689 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 1.16. If the initial pressure of NO is 0.00781 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) =_______ . p(N2) = ______ . p(O2) =_______ .
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 6RQ: Distinguish between the terms equilibrium constant and reaction quotient. When Q = K, what does this...
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At 6689 oC the equilibrium constant for the reaction:
2 NO(g) N2(g) + O2(g)
is KP = 1.16. If the initial pressure of NO is 0.00781 atm, what are the equilibrium partial pressures of NO, N2, and O2?
p(NO) =_______ .
p(N2) = ______ .
p(O2) =_______ .
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