Question

1. For the reaction:
2NO2 (g)→2NO(g)+O2
the rate law has been determined experimentally to be
rate=K[NO2]^2
a. What is the order of reaction with respect to NO^2 and what is the overall order?
b .How much faster will the reaction proceed when the partial pressure of NO2 is 3 atm and when the partial pressure of NO2 is 1 atm?

Answer 1

Answer:

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Answer 2

Answer:

a) Order is 2 with respect to $NO_2$. THE overall order is also 2.

b) The ratio will be 1:3 . The reaction is almost 9 times faster when the partial pressure of $NO_2$ is 1 atm.

Explanation:

The order is 2 with respect to $NO_2$ because it has been experimentally derived that the change in the rate will become twice as the change in concentration of $NO_2$

The overall order is also 2 because the rate equation has no mention of NO or $O_2$ giving us an understanding that their change in concentration will not affect the rate.

$K \alpha \frac{1}{p(NO_2)^2} \\\frac{K(3atm)}{K(1atm)} =\frac{pNO_2 (1 atm)^2}{pNO_2(3 atm)^2} \\\frac{K(3atm)}{K(1atm)} = \frac{1^2}{3^2} \\\frac{K(3atm)}{K(1atm)} = \frac{1}{9} \\9 K(3atm) = K(1 atm)$

So the rate will be 9 times faster when the partial pressure of $NO_2$ is 1 atm.