The reaction of nitrogen dioxide with carbon monoxide is given below:
NO2 + CO NO + CO2

Is second order in NO2 and zero order in CO.

a. Complete the rate law for this reaction.
b. In an experiment to determine the rate law, the rate constant was determined to be 0.790 M-1s-1. Using this value for the rate constant, the rate of the reaction when [NO2] = 1.23 M and [CO] = 0.221 M would be:

Explanation:

NO2 + CO --> NO + CO2

Is second order in NO2 and zero order in CO.

A. Rate law for the reaction:

Rate = K[NO2]²[CO]⁰

Rate = K[NO2]²

B.

k = 0.790 M-1s-1

[NO2] = 1.23 M

[CO] = 0.221 M

Rate = ?

Rate = K[NO2]²[CO]⁰

Rate = 0.790  *  1.23² * 0.221⁰

Rate = 0.790  *  1.23² * 1 =  1.1952M/s

*tilts head* sounds more like a statement

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.