I need help with my chemistry homework my teacher didn't give an example of this. Can someone explain what to do step by step?

The reaction of NO2 with ozone produces No3 in a second-order reaction overall: NO2 (g) + O3 (g) > NO3 (g) + O2 (g) The rate constant for the reaction is 1.93 x 10^4 M^-1s^-1 at 298 K. What is the rate of the reaction when [NO2] = 1.8 x 10^-8 M and [O3] = 1.4 x 10^-7 M? What is the rate of the appearance of... show more The reaction of NO2 with ozone produces No3 in a second-order reaction overall:
NO2 (g) + O3 (g) > NO3 (g) + O2 (g)

The rate constant for the reaction is 1.93 x 10^4 M^-1s^-1 at 298 K.
What is the rate of the reaction when [NO2] = 1.8 x 10^-8 M and [O3] = 1.4 x 10^-7 M?

What is the rate of the appearance of NO3 under these conditions?

The back of my textbook has the answers and it says the answer to both questions is: 4.9 x 10^-11 M/s
How do you get this answer?
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