Question

Consider the following reaction: 2 H2(g) + 2 NO(g) → 2 H2O(g) + N2(g) If the concentration of NO changed from 0.100 M to 0.025 M in the first 15 minutes of the reaction, what is the average rate of the reaction during this time interval?

Answer 1

Answer: The average rate of the reaction during this time interval is, 0.005 M/s

Explanation:

The given chemical reaction is:

$2H_2(g)+2NO(g)\rightarrow 2H_2O(g)+N_2(g)$

The expression will be:

$\text{Average rate of reaction}=\frac{C_2-C_1}{t_2-t_1}$

where,

$C_2$ = final concentration of $NO$ = 0.025 M

$C_1$ = initial concentration of $NO$ = 0.100 M

$t_2$ = final time = 15 minutes

$t_1$ = initial time = 0 minutes

Putting values in above equation, we get:

$\text{Average rate of reaction}=\frac{0.025-0.100}{15-0}$

$\text{Average rate of reaction}=0.005M/s$

Hence, the average rate of the reaction during this time interval is, 0.005 M/s