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2NOBr(g)(double arrow)2NO(g) + Br2(g) If 0.382 moles of NOBr(g), 0.517 moles of NO, and 0.579 moles...

2NOBr(g)(double arrow)2NO(g) + Br2(g)

If 0.382 moles of NOBr(g), 0.517 moles of NO, and 0.579 moles of Br2 are at equilibrium in a 17.5L container at 522 K, the value of the equilibrium constant, Kc, is

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2 NOBr Kc= - 2NO+ Brz. [N01² [Brz]? No Br72 6.579 17.5 0 382)2 178 - (0:517)*(0.579) (1715) (0.382)2 = 0.0606. And.

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