Consider the reaction: 2no(g) o2(g) --> 2no2(g) suppose that at a particular moment during the reaction nitric oxide (no) is reacting at the rate of 0.0022 m/s.

a. at what rate is no2 being formed?
b. at what rate is molecular oxygen reacting?

NO2 is beign formed at a rate of 0.0022 M/s

O2 is disappearing at a rate of 0.0011 M/s

Explanation:

Step 1: Data given

The rate of 0.0022 M/s.

-1/2*[NO]/ΔT = -[O2]/ΔT = 1/2*[NO2]/ΔT

Step 2: The balanced equation

2NO(g) + O2(g) ⇆ 2NO2(g)

Step 3: Calculate the rate of (dis)appearance

[NO2]/ΔT = 0.0022/2 M/s = 0.0011 M/s (Positive because NO2 is being formed)

-1/2[O2]/ΔT = -1/2*0.0022/ΔT = -0.0011 M/s (negative because O2 is disappearing)

NO2 is beign formed at a rate of 0.0022 M/s

O2 is disappearing at a rate of 0.0011 M/s

it is a solid

explanation: