Chemistry, 10.10.2019 00:00 Kassymatt

For the following reaction, kc = 15 at 700 k. 2 no(g) + cl2(g) ⇄ 2 nocl(g) if we have [no] = 0.15 m, [cl2] = 0.15 m, [nocl] = 0.40 m at 700 k, what will happen? group of answer choices the equilibrium will not shift. the equilibrium will shift to the left, but will use up only part of the nocl. the equilibrium will shift to the right, but will use up only part of the no and cl2. the equilibrium will shift to the right until all the reactants are used up. the equilibrium will shift to the left until all the nocl is used up.

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For the following reaction, kc = 15 at 700 k. 2 no(g) + cl2(g) ⇄ 2 nocl(g) if we have [no] = 0.15 m,...

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