At 7914 oc the equilibrium constant for the reaction 2 nog
At 7914 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 0.726. If the initial pressure of NO is 0.00366 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) = . p(N2) = . p(O2) = .
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Gaseous NOBr is placed in a closed container at -180 oC, where it partially decomposes to NO and Br2: 2 NOBr(g) 2 NO(g) + 1 Br2(g) At equilibrium it is found that p(NOBr) = 0.008230 atm, p(NO) = 0.004080 atm, and p(Br2) = 0.004130 atm.
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