WorksheetsChemical kinetics
Total questions: 25
Worksheet time: 41mins
Which of the following plots will show a linear relationship for a second order reaction?
[A] vs time
1/[A] vs time
ln[A] vs time
[A]2 vs time
The following data were measured for the reaction
BF3(g) + NH3(g) ⟶ F3BNH3(g)
What is the rate law for the reaction?
rate = k[NH3]
rate = k[BF3]2[NH3]
rate = k[BF3][NH3]
rate = k[BF3][NH3]2
What letter represents the activation energy?
A
B
C
D
Which of the two graphs show a state of equilibrium being reached?
A
B
A and B
Neither.
Given the following rate law,
rate = k[A]2[B]
if [A] were doubled, what must happen to [B] to keep the rate constant?
[B] must quadruple
[B] must double
[B] must be havled
[B] must be quartered
Which of the following best describes why increasing temperature increase reaction rate?
Activation energy is reduced.
Collisions become more frequent.
Collisions become more energetic.
Collisions become more frequent and more energetic.
Which species is the catalyst in this reaction mechanism?
R
W
X
There is no catalyst.
The addition of a catalyst to this reaction would cause a change in which of the indicated energy differences?
I
II
III
I and II
Which factors increase the rate of a reaction?
increasing temperature
increasing concentration
increasing surface area
all of the above
The iodide ion reacts with hypochlorite ion in the following way:
OCl- + I- ⟶ OI- + Cl-.
This rapid reaction gives the rate data shown. What is the rate law?
rate = [OCl-]2[I-]
rate = [OCl-][I-]2
rate = [OCl-][I-]
rate = [OCl-]
The following data were measured for the reaction
BF3(g) + NH3(g) ⟶ F3BNH3(g)
What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M ?
.01704 M/s
.0852 M/s
.1704 M/s
.852 M/s
A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction __________.
doubles
remains unchanged
increases by a factor of 4
is reduced by a factor of 2
rate = k[A]
The rate constant in the rate law above is 0.5 L/mol·s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?
0.7 s
1.4 s
2.8 s
There is not enough information given.
What is the rate law for this mechanism?
rate = k[A][B]2
rate = [B][X]
rate = [A]0.5[B]1.5
rate = [W][Y][Z]
X + Y → Z + Q ΔH = +22kj/mol
How can above reaction be classified in terms of energy exchange during chemical change?
The catalyst alters the rate of a chemical reaction by,
providing an alternative pathway with a lower Ea
changing the products formed in the direction of the reaction
providing a surface on which the molecules react
increasing the frequencies of collisions between molecules
The iodide ion reacts with hypochlorite ion in the following way:
OCl- + I- ⟶ OI- + Cl-.
This rapid reaction gives the rate data shown. What is the rate law?
rate = [OCl-]2[I-]
rate = [OCl-][I-]2
rate = [OCl-][I-]
rate = [OCl-]
Units of rate is _______-
M/s
mol/s
m.s
s/M
The following data were measured for the reaction
BF3(g) + NH3(g) ⟶ F3BNH3(g)
What is the rate law for the reaction?
rate = k[NH3]
rate = k[BF3]2[NH3]
rate = k[BF3][NH3]
rate = k[BF3][NH3]2
