Chemistry: 2. 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 0.066 m/s. a. at what rate is no2 being formed? (3 points) b. at what rate is molecular oxygen reacting? (3 points)

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2. consider the reaction 2no(g) + o2(g) → 2no2(g)

luusperezzz

15.03.2022

Answer :

(a) The rate of NO_2 formed is, 0.066 M/s

(b) The rate of O_2 formed is, 0.033 M/s

Explanation : Given,

$\frac{d[NO]}{dt}$ = 0.066 M/s

The balanced chemical reaction is,

$2NO(g)+O_2(g)\rightarrow 2NO_2(g)$

The rate of disappearance of = $-\frac{1}{2}\frac{d[NO]}{dt}$

The rate of disappearance of O_2 = $-\frac{d[O_2]}{dt}$

The rate of formation of NO_2 = $\frac{1}{2}\frac{d[NO_2]}{dt}$

As we know that,

$\frac{d[NO]}{dt}$ = 0.066 M/s

(a) Now we have to determine the rate of NO_2 formed.

$\frac{1}{2}\frac{d[NO_2]}{dt}=\frac{1}{2}\frac{d[NO]}{dt}$

$\frac{d[NO_2]}{dt}=\frac{d[NO]}{dt}=0.066M/s$

The rate of NO_2 formed is, 0.066 M/s

(b) Now we have to determine the rate of molecular oxygen reacting.

$-\frac{d[O_2]}{dt}=-\frac{1}{2}\frac{d[NO]}{dt}$

$\frac{d[O_2]}{dt}=\frac{1}{2}\times 0.066M/s=0.033M/s$

The rate of O_2 formed is, 0.033 M/s

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