Kinetics Module 1

Course Name:  Chemistry
Course No.132 NT
Teacher:  Bill Cook
Teacher's Email:  bcook@icc.edu

No. of Questions= 3


1.  The oxidation of ammonia produces nitrogen and water via the reaction

4 NH3 + 3 O2 ®  2 N2 + 6 H2O.

If the rate of formation of N2 is 2.0 mol/(L.s), then the rate at which:

a) H2O is being formed is 0.67 mol/(L.s).
b) NH3 reacts is 4.0 mol/(L.s).
c) O2 reacts is 1.5 mol/(L.s).
d) NH3 reacts is 0.50 mol/(L.s).
e) H2O is formed is 2.0 mol/(L.s).
2.  The reaction of iodide ion with hypochlorite ion, OCl – (which is found in liquid bleach), follows the reaction

                                          OCl – + I – ® OI – + Cl –                  

It is a rapid reaction that gives the following rate data.

Experiment number

[OCl –]

[I –]

Initial rate M/s

1

1.7 x 10 –3

1.7 x 10 –2

1.75 x 10 4

2

3.4 x 10 –3

1.7 x 10 –2

3.5 x 10 4

3

1.7 x 10 –3

3.4 x 10 –2

3.5 x 10 4

 

 

 

 

What is the rate law for the reaction?

a) Rate = k[OCL-]2[I-]
b) Rate = k[OCL-]2[I-]2
c) Rate = k[OCL-] [I-]2
d) Rate = k[OCL-] [I-]
e) None of these
3.  What is the numerical value of "k" in question #2?
a) 3.56 x 1011
b) 6.06 x 108
c) 3.56 x 1011
d) 2.09 x 1013
e) none of these



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