Question

The reaction of nitrogen gas and oxygen gas to form nitrogen monoxide gas is shown below. If the measured concentrations of all three chemicals at some point in time are: [N2] = 0.80 M
[O2] = 0.050 M
[NO] = 0.10 M
Which statement is TRUE about the reaction at this point in time? N2(g) + O2(g) â 2 NO(g) K = 0.10

The reaction is at equilibrium.
The reverse reaction is occurring at a faster rate than the forward reaction.
The forward reaction is occurring at a faster rate than the reverse reaction.
This set of concentration values is impossible because the concentrations of N2 and O2 must be the same.

Answer 1

Answer:

The forward reaction is occurring at a faster rate than the reverse reaction.

Explanation:

Reaction quotient (Q) of the given reaction is -

                                     $Q=\frac{[NO]^{2}}{[N_{2}][O_{2}]}$

where [NO], $[N_{2}]$ and $[O_{2}]$ represents concentrations of respective species at a certain time.

Here $[N_{2}]$= 0.80 M, $[O_{2}]$= 0.050 M and [NO] = 0.10 M

So, $Q=\frac{(0.10)^{2}}{(0.80)\times (0.050)}=2$

Hence $Q> K$

It means that forward reaction is faster than reverse reaction at that point. Because then only concentration of NO is higher than concentrations of $[N_{2}]$ and $[O_{2}]$ which makes Q higher than K.