Assume that in the following reversible reaction, both the forward and the reverse reactions take place in a single step. NO (g) + O3 (g) NO2 (g) + O2 (g)

Describe the changes that take place in the reaction vessel from the time when NO (g) and O3 (g) are first added to the container until a dynamic equilibrium is reached

Question

Chemistry

Russell Harding

26 October, 06:36

Assume that in the following reversible reaction, both the forward and the reverse reactions take place in a single step. NO (g) + O3 (g) NO2 (g) + O2 (g)

Describe the changes that take place in the reaction vessel from the time when NO (g) and O3 (g) are first added to the container until a dynamic equilibrium is reached

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Cyrus Swanson · Answer 1

As NO and O3 react to create NO2 and O2, the concentrations of NO and O3 decrease (since the reactants turn to product), and the concentrations of NO2 and O2 increase. The equilibrium will shift to the right, but as time goes on, some of the NO2 and O2 will dissociate to create NO and O3 again. You reach dynamic equilibrium when the reaction rate of NO and O3 combining is equal to the reaction rate of NO2 and O2 dissociating.