Exam 13: Chemical Kinetics: Reactions in the Atmosphere

What is the predicted rate law for the following mechanism for the reduction of nitrogen in NO by hydrogen? Step 1: (slow) Step 2: (fast) What is the rate law?

Using the reaction shown below, which statement is correct?

Which of the following plots indicates that the reaction is second order?

A proposed mechanism for the reduction of nitrogen as NO by hydrogen is: Step 1: Step 2: What is the molecularity of step 1?

The difference between an average rate and an instantaneous rate is ________

The energy profiles for four different reactions are shown below. The scales are the same for each. Which reaction requires the most energetic collisions to reach the transition state?

Which statement A-D regarding the reaction described by the energy profile below is not correct?

For the rate law Rate  k[A]^1/2[B], the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________.

Which point in the reaction profile below represents an intermediate?

Large cities often issue ozone advisories. At what time of year would an advisory be likely to occur most often?

From the following concentration versus time plot for four different reactions, which has the greatest instantaneous rate of disappearance at the time indicated by the arrow?

In a first order reaction, the initial concentration of A is 0.40 M. What is the concentration of A after 15 seconds if the half-life of the reaction is 3 seconds?

If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N₂?

The energy profiles for four different reactions are shown below. The scales are the same for each. Which of the reactions will have the smallest rate constant?

The order in which ozone, nitrogen monoxide, and nitrogen dioxide build up in the atmosphere over the course of the day is first ________ then ________ then ________.

For the rate law Rate  k[A][B]^1/2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________.

The high temperatures in an automobile engine cause nitrogen and oxygen to form noxious nitrogen monoxide. Use the following data on the temperature dependence of the rate constant to determine the activation energy for this reaction. T (K) K (M^1 s^1) 2,200 1,800 2,400 7,400

If the rate of the reaction: is 0.250 M/s over the first 5.50 s, how much ozone will be consumed during this time?

The second-order reaction A B is found to have a rate constant of 0.978 M^1s^1. What is the half-life of this reaction when [A]₀  0.0300 M?

For the reaction 2A  3B 4C  5D, the rate of the reaction in terms of A would be written as ________.