Journal Entry:

Refer to the reaction of nitrogen monoxide (nitric oxide) and oxygen and the following data in table below. If the rate law is Rate= k[NO]²[O₂], the numerical value for the rate constant (k) is closest to:

(A) 5.9 X 10^-2
(B) 170
(C) 7.0 x 10³
(D) 1.2 X 10⁵

Learning Intentions

• We will learn how to analyze concentration vs time data to determine the rate law for zeroth, first and second order reaction. 

• We will learn how to calculate rate constant and its unit.

• We will learn how what changes rate constant for a reaction

• We will learn how to determine rate law for multipstep processes.

• We will learn about reaction intermediates and the role they play in a multistep process.

Closing Task:

You can use the integrated rate laws to determine k.

You can evaluate multi-step processes to determine rate law. 

Content Standards being covered:

Catalysts function by lowering the activation energy of an elementary step in a reaction mechanism, and by providing a new and faster reaction mechanism. (E.K. 4.D.1)

The rate law shows how the rate depends on reactants concentrations. (E.K. 4.A.2)

Elementary reactions can be unimolecular or involve collisions between two or more molecules. (E.K. 4.B.1)

The mechanisms of a multipstep reaction consists of a series of elementary reactions that add up to the overall reaction. (E.K.4.C.1)

In many reactions, the rate is set by the slowest elementary reaction, or rate limiting step. (E.K. 4.C.2)

Reaction intermediates which are formed during the reaction but not present in the overall reaction, play an important role in multistep reactions. (E.K. 4.C.3)