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

Step-by-step 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}=(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}=(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