Question

The same reaction is begun with an initial concentration of 0.05 M O3 and 0.02 M NO. Under these conditions, the reaction reaches completion in 8 seconds. What is the initial rate of this reaction with respect to O3?

Answer 1

The initial rate of the reaction with respect to O3 can be calculated using the rate law equation. The initial rate is found to be 160 M/s.

Step-by-step explanation:

The initial rate of the reaction with respect to O3 can be determined by looking at the reaction rate law. In this case, we are given that the reaction reaches completion in 8 seconds, so we can use this information to calculate the initial rate. The rate law for the reaction can be represented as rate = k[O3]^[NO] where k is the rate constant. Since the concentration of O3 is given as 0.05 M, we can plug in this value into the rate law equation along with the other given values to calculate the initial rate.

Using the given information, the rate law equation becomes rate = k(0.05)^1(0.02)^0 = k(0.05)

The time taken for the reaction to reach completion is 8 seconds, so we can divide this by the concentration of O3 to find the initial rate:

Initial rate = 8 seconds / 0.05 M = 160 M/s

Answer 2

The balanced equation of the reaction is:

O3(g) + NO (g) → O2 (g) + NO2 (g)

Then the ratios of reaction is 1 mol O3 : 1 mol NO : 1 mol O2 : 1 mol NO2

If you have initially 0.05 M of O3 and 0.02 M of NO, the reaction will end when all the NO is consumed.

The by the stoichiometry 0.02 mol of O3 will be consumed in 8 seconds.

And the rate of reaction is change in concetration divided by the time.

The change in concentration in O3 is 0.02 M

Then, the rate respect O3 is 0.02 M / 8 seconds = 0.0025 M/s