Question

Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO₂(g)→2NO(g)+O₂(g)

In a particular experiment at 300 °C, [NO₂] drops from 0.0100 to 0.00800 M in 100 s. The rate of appearance of O₂ for this period is ________ M/s.
A) 2.0×10⁻³
B) 1.0×10⁻⁵
C) 4.0×10⁻³
D) 4.0×10⁻⁵
E) 2.0×10⁻⁵

Answer 1

The rate of appearance of O2 for the given reaction is 0.0000100 M/s.

Step-by-step explanation:

To determine the rate of appearance of O2, we need to calculate the rate of decomposition of NO2. The rate of decomposition can be determined by dividing the change in concentration of NO2 by the change in time. In this case, the change in concentration of NO2 is 0.0100 M - 0.00800 M = 0.00200 M, and the change in time is 100 seconds. Therefore, the rate of decomposition of NO2 is 0.00200 M / 100 s = 0.0000200 M/s. Since the stoichiometry of the reaction is 2NO2(g) -> 2NO(g) + O2(g), the rate of appearance of O2 is half of the rate of decomposition of NO2, which is 0.0000100 M/s.