Chemical Kinetics Worksheet With Answers By Prof. Abdullah M. Asiri - 2009 Page 28
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33August 16, 2009
[PROBLEM SET FROM R. CHANG TEST
BANK]
97. The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction
→ H
-
+
-
H
AsO
+ 3I
+ 2 H
O
AsO
+ I
+ H
O. The experimental rate law for this reaction is Rate =
3
4
3
3
3
3
2
-
+
k[H
AsO
][I
][H
O
].
3
4
3
-
What is the order of the reaction with respect to I
?
98. The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction
→ H
-
+
-
H
AsO
+ 3I
+ 2 H
O
AsO
+ I
+ H
O. The experimental rate law for this reaction is
3
4
3
3
3
3
2
-
+
Rate = k[H
AsO
][I
][H
O
].
3
4
3
According to the rate law for the reaction, an increase in the concentration of hydronium ion has what
effect on this reaction?
99. For the following exothermic reaction, the rate law at 298 K is Rate = k [H
] [I
]:
2
2
(g) → 2HI(g)
H
(g) + I
2
2
Predict the effect of each of the following changes on the initial rate of the reaction.
a. Addition of hydrogen gas at constant temperature and volume
b. Increase in volume of the reaction vessel at constant temperature
c. Addition of a catalyst
d. Increase in temperature
O → 2N
100. In the reaction, 2N
+ O
, oxygen and nitrogen gases are formed at the same rate (mol/L·s) .
2
2
2
True False
101. The rate constant of a first-order reaction, A → products, can be determined from a graph of ln[A] versus
t.
True False
28
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