Question

g For the reaction N2(g) + O2(g) --> 2 NO(g), the equilibrium constant, K=1.0x10-5 Which direction will the reaction move, and why, if the reactants and products have the following concentrations: [N2]=0.015 M [O2]=0.25 M [NO]=0.010

Answer 1

Answer:

Reaction will proceed in backward direction.

Explanation:

At first we have to calculate the value of reaction quotient. It measures the relative amount of products and reactants present at any instant.

So, for the reaction mentioned in the question, the reaction quotient will be

Q = $\frac{[NO]^2}{[N_2][O_2]}$ where the terms in the large bracket denote the concentrations of respective reacting species.

So,

Q = $\frac{(0.010)^2}{0.015\times 0.25}$ = $2.7\times 10^-^2$

Upon comparing the value of reaction quotient with the value of equilibrium constant K = $1\times 10^-^5$, we see that the Q is larger than that of K.

This means there are more amounts of product in the solution as compared to the equilibrium amount and that's why the reaction will go backward.