Question

Nitric oxide reacts with H₂ according to the reaction :

2NO_(g) + 2H_2(g) → N_2(g) + 2H₂O_(g)

What is the relationship among,

\(\frac{d[NO]}{dt}\) = \(\frac{d[H_2]}{dt}\) = \(\frac{d[N_2]}{dt}\) and \(\frac{d[H_2O]}{dt}\) ?

Answer 1

Given :

2NO_(g) + 2H_2(g) → N_2(g) + 2H₂O_(g)

The relationship among the rate of consumption of the reactants and the rate of formation of products is as follows :

Rate of reaction :

R = \(-\frac{1}{2}\)

= \(\frac{d[NO]}{dt}\) = \(-\frac{1}{2}\)

= \(\frac{d[H_2]}{dt}\)

= \(\frac{d[N_2]}{dt}\) 

= \(\frac{1}{2}\) \(\frac{d[H_2O]}{dt}\)