Question

1. Write the rate expression for the following reaction.

2N₂O₅(g) → 4NO₂(g) + O₂(g)

2. For a hypothetical reaction, aX + bY → Products, the rate law is given as \(\frac{dx}{dt}=\) k[X]²[Y]^1/2. What happens to the rate of the reaction when

• The concentration of ‘X’ is doubled keeping that of ‘Y’ constant.
• The concentration of both ‘Y’ is doubled keeping that of ‘X’ constant. 

Answer 1

1. Rate expression :

Rate = \(-\frac{1}{2}\,\frac{d[N_2O_5]}{dt}=\)\(+\frac{1}{4}\,\frac{d[NO_2]}{dt}= + \frac{d[O_2]}{dt}\)

2.

• Increases by 4 times
• Increases by \(\sqrt2\) times.