Question

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction:

2NO_{2} --------->2NO+ O_{2}

In a particular experiment at 300 °C, [NO_{2}] drops from 0.0100 to 0.00650 M in 100s.
Calculate the rate of appearance of O_{2} for this period in terms of M/s.

Answer 1

The rate of appearence of O2 is 1.75 * 10^-5 M/s

Step-by-step explanation:

Step 1: Data given

at 300 °C, [NO2] drops from 0.0100 to 0.00650 M in 100s.

Step 2: The balanced equation:

2NO2 ⇒ 2NO+ O2

Step 3: Calculate the rate of appearence of O2

Rate = Δconcentrtion )/Δtime

Rate of disappearence of NO2 = (0.01M - 0.0065M)/100s= 0.000035 M/s

The mol ratio NO2:O2 = 2:1

-1/2 *0.000035 = 1/1 * rate O2

Rate of appearence of O2 = 0.000035/2 =0.0000175 = 1.75 * 10^-5 M/s

The rate of appearence of O2 is 1.75 * 10^-5 M/s