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WorksheetsChemical Kinetics
Total questions: 10
Worksheet time: 8mins
Name
Class
Date
1.
Which of the following best describes why increasing temperature increase reaction rate?
a)
Activation energy is reduced.
b)
Collisions become more frequent.
c)
Collisions become more energetic.
d)
Collisions become more frequent and more energetic.
2.
Which factors increase the rate of a reaction?
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of the above
3.
Which of the following is expressions represents correctly rate of following reaction?
X + Y → Z + Q ΔH = +22kj/mol
X + Y → Z + Q ΔH = +22kj/mol
a)
Rate = +Δ[X] / Δt
b)
Rate = +Δ[Y] / Δt
c)
Rate = +Δ[Z] / Δt
d)
Rate = -Δ[Q] / Δt
4.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment
5.
What does [ ] denote?
a)
concentration, M
b)
concentration, m
c)
concentration, mass %
d)
squared
6.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
7.
Reaction rate means...
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
8.
A possible rate law for a third overall order of a reaction is __________________
a)
Rate = k [A]2[B]2
b)
Rate = k [A][B]3
c)
Rate = k [A]3 [B]
d)
Rate = k [A]2[B]
9.
Units of rate is _______-
a)
M/s
b)
mol/s
c)
m.s
d)
s/M
10.
Limestone chunks are reaction with hydrochloric acid solution at constant temperature with average speed. If we crash the chunks of limestone into powder how would speed of reaction change?
a)
Reaction speeds up
b)
Reaction does not change
c)
Reaction slows down
d)
Reaction stops
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