1. ANSWER ALL QUESTIONS
1. The data below was collected for the hypothetical reaction 2 A → B + C.
Time (s) [A]t
0 0.1
40 0.0768
80 0.059
120 0.0453
160 0.0348
a. Write both a first-order and a second-order integrated plots.
b. Based on your graphs, is the reaction zero, first or second order? Explain your reasoning.
c. Determine the value for the rate constant with correct units.
2. The rate constant for the reaction below is 6.2 x 10−5
mol L−1
s−1
. If the initial concentration
of A is 0.0500 M, what is its concentration after 115 s?
A → B + C
Chemistry Unit
Session 2013/2014
Semester 2
Sample QUIZ Paper
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2. 3. Hydrogen iodide decomposes according to the equation shown below. The second order rate
constant for this reaction is 1.6 x 10–3
L mol–1
s–1
at 700 ºC. If the initial concentration of HI
in a container is 5.1 x 10–2
M, how many minutes will it take for the concentration to be
reduced to 4.9 x 10–3
M at 700 ºC?
2 HI(g) → H2(g) + I2(g)

3. 0
ln[A]
1/[A]
1. a.
First Order Integrated Plot Second Order Integrated Plot
-2
-2.2
-2.4
-2.6
-2.8
-3
-3.2
-3.4
-3.6
y = -0.0066x - 2.3026
0 20 40 60 80 100 120 140 160 18
Time (s)
35
30
25
20
15
10
5
0
0 20 40 60 80 100 120 140 160 180
Time (s)

4. b. The reaction is first order because the first order integrated rate plot is linear, while
the second order rate plot is curved.
c. m = −k, so k = −m = −(−0.0066 s−1
) = 0.0066 s−1
2. 0.0429 M
3. 1.9 x 103
min