Consider this equilibrium:

N2 (g) + 2O2 (g) NO2 (g).

Equal amounts of N2 and O2 are added, under certain conditions, to a closed container. Which changes occur in the reverse reaction as the system proceeds toward equilibrium?

A. reverse reaction rate increases; [NO2] increases

B. reverse reaction rate decreases; [NO2] increases

C. reverse reaction rate increases; [NO2] decreases

D. reverse reaction rate decreases; [NO2] decreases

E. reverse reaction rate and [NO2] are not affected

Question

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Chemistry

27 November, 13:47

Consider this equilibrium:

N2 (g) + 2O2 (g) NO2 (g).

Equal amounts of N2 and O2 are added, under certain conditions, to a closed container. Which changes occur in the reverse reaction as the system proceeds toward equilibrium?

A. reverse reaction rate increases; [NO2] increases

B. reverse reaction rate decreases; [NO2] increases

C. reverse reaction rate increases; [NO2] decreases

D. reverse reaction rate decreases; [NO2] decreases

E. reverse reaction rate and [NO2] are not affected

+2

Answers (1)

Know the Answer?

Miya Compton · Answer 1

At first, you have a lot of N2 and O2 but very little No2, So, the system will react so as to favour the production of No2 ... Here, NO2 Increases as system tends towards equilibrium ...

As the amount of NO2 increases, he number of moles of the reactants have to be compensated as it is a reversible reaction, thus, reverse reaction increases to meet the equilibrium demand.

Answer (A)