wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Rate of reaction 92Q for M5 (BMS-EP)

Total questions: 92

Worksheet time: 2hrs 18mins

Name
Class
Date
1.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

2.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

3.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

4.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
5.
What does NOT happen when the temperature is increased?
a)
Particles collide more often
b)
Particles collide with more energy
c)
Particles move faster
d)
More particles collide in the correct orientation
6.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
7.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

8.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

9.

The ______________is required to break the bonds of the reactants.

a)

Kinetic energy

b)

Activation energy

c)

Potential energy

d)

Gibbs energy

10.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
11.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
12.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
13.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
14.
Located on the left side of the reaction
a)
reactants
b)
products
15.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

16.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
17.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

18.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
19.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
20.
Catalysts permit reactions to proceed along a ___________energy path.
a)
lower
b)
higher
21.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
22.
The ___________ the surface area of the reactants, the faster the reaction rate.
a)
larger 
b)
smaller
23.
Increasing the temperature will increase the kinetic energy of particles, therefore increasing the collisions between particles.
a)
false
b)
true
24.
Usually lowering the temperature will slow down a reaction.
a)
false
b)
true
25.
Increasing the concentration of the reactants will slow down the reaction.
a)
false 
b)
true
26.
You observe bubbles after adding metal to a solution. Do you assume a chemical reaction took place?
a)
Yes
b)
No
27.
A solution is heated and bubbles form. Do you assume a chemical reaction took place?
a)
Yes
b)
No
28.
Two clear and colorless solutions are combined within a test tube. The result is very cloudy. Do you assume a chemical reaction took place?
a)
Yes
b)
No
29.
Two clear and colorless solutions are combined within a test tube. The resulting solution is purple. Do you assume a chemical reaction took place?
a)
Yes
b)
No
30.
Metal is added to a solution in a test tube. The test tube now feels cooler. Do you assume a chemical reaction took place?
a)
Yes
b)
No
31.
A beaker containing a solution is heated. The beaker now feels warm. Do you assume a chemical reaction took place?
a)
Yes
b)
No
32.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
33.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

34.

What is the energy of the activated complex?

a)

75 kJ

b)

225 kJ

c)

300 kJ

d)

50 kJ

35.

What is the name given to a catalyst in the human body?

a)

Biology

b)

Catalyst

c)

Chemical

d)

Enzyme

36.
Which of the following is/are the fundamental idea(s) of collision theory?
a)
Molecules react by colliding together
b)
The effective collisions must occur with certain minimum amounts of energy 
c)
In a large sample, the greater the number of effective collisions, and the faster the rate of reaction
d)
All of the above
37.
What is the disadvantage of using some metal catalysts
a)
expensive
b)
difficult to extract
c)
heavy
d)
toxic
38.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
39.
How does the energy in a reversible reaction in one way compare with the opposite direction?
a)
more energy going forward
b)
more energy going back
c)
the same
d)
no difference
40.

The reaction between zinc and hydrochloric acid may be represented by the equation:

Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g);

In an investigation of this reaction using excess Zn and 2 M HCl(aq) in an open flask, the graph shown was plotted from the data collected.

Which of the following would be a suitable quantity for the vertical axis of the graph?

a)

mass of zinc per second

b)

volume of hydrogen gas produced per second

c)

Temperature.

d)

mass loss per second

41.

If 5 cm3 of gas is produced in 20 seconds what is the average rate of reaction?

a)

5 cm3 s-1

b)

0.25 cm3 s-1

c)

4 cm3 s-1

42.

why is the reaction fastest at the start ?

a)

The reactants are in their greatest concentration

b)

this statement is untrue the reaction is same rate through out whole reaction

43.
To measure the speed of a reaction you will use one of the following equipment.
a)
Petri dish
b)
Stop watch
c)
stirring rod
d)
Universal indicator
44.
The graph shows how the total volume of a gas given off from a reaction changes with time. In which time interval is least gas given off? 
a)
A
b)
B
c)
C
d)
D
45.

Which unit is correct for the rate of reaction?

a)

g mol-1

b)

g min-1

c)

mol dm-3

d)

kJ mol-1

46.

What is the meaning of the rate of reaction?

a)

Decrease in amount of product

b)

Decrease in amount of product against time

c)

Increase in amount of products against time

d)

Increase in amount of reactants against time

47.

Which of the following has the lowest rate of reaction?

a)

Combustion of ethanol

b)

Fermentation of glucose

c)

Oxidation of magnesium

d)

Precipitation of silver chloride

48.

Which reactions has the highest rate of reaction?

a)

Rusting of water pipe

b)

Photosynthesis in green plant

c)

Burning of a small piece of charcoal in the air

d)

Formation of stalactites and stalagmites

49.

Which process has the highest rate of reaction?

a)

Rusting

b)

Respiration

c)

Combustion

d)

Photosynthesis

50.

The following equation represents a chemical equation.

CaCO3 + 2HCl --> CaCl2 + CO2 + H2O

Which graph shows the correct change in mass of reactant used in excess against time?

a)
b)
c)
d)
51.

Diagram shows the apparatus set up for an experiment to determine the rate of reaction.

Which of the following techniques is the most suitable to determine the rate of reaction?

a)

Record the time as soon as precipitate is formed

b)

Record the time taken to obtain the maximum temperature

c)

Record the times as soon as the cross mark cannot be seen

d)

Record the times taken for the change of the pH value until a fixed pH value is obtained

52.

The following equation represents the reaction between calcium carbonate, CaCO3 and hydrochloric acid, HCl.

CaCO3 + 2HCl --> CaCl2 + CO2 + H2O

Which changes can be used to determine the rate of reaction?

I : mass of calcium carbonate per unit time

II : Volume of carbon dioxide released per unit time

III : Colour of solution per unit time

IV : Mass of precipitate produced per unit time

a)

I and II

b)

I and III

c)

II and IV

d)

III and IV

53.

Diagram shows a graph of volume of oxygen gas collected against time in the decomposition reaction of hydrogen peroxide when using manganese dioxide as catalyst.

Which point shows the highest rate of reaction?

a)

P

b)

Q

c)

R

d)

S

54.

Diagram shows a graph to study the effect of total surface area on the rate of reaction.

What is represented by gradient tangent X?

a)

Average rate of reaction in the first 2 minutes

b)

Average rate of reaction in the 2nd minute

c)

Overall average rate of reaction

d)

Rate of reaction at the 2nd minute

55.
Hydrochloric acid can react with sodium thiosulfate solution to form a sulfur precipitate. The equation is:
Na2S2O3(aq) + 2HCl(aq) → 2S(s) + SO2(g) + 2NaCl(aq) + H2O(l)
Which list below contains only changes that will decrease the rate of this reaction?
a)
Increase the temperature, increase the hydrochloric acid concentration and add a catalyst
b)
Decrease the temperature and add a catalyst
c)
Decrease in temperature, decrease in concentration of the hydrochloric acid, addition of water to the sodium thiosulfate
d)
Decrease the concentration of the sodium thiosulfate solution and increase the temperature
56.
Under certain conditions, cyclohexane can react to form benzene and hydrogen according to the equation:
C6H12(g) → C6H6(g) + 3H2(g); ΔH=+206 kJ mol-1
Which two changes could be used to increase the rate of reaction?
a)
Add a catalyst and reduce the temperature
b)
Add a catalyst and decrease the pressure
c)
Increase the temperature and the external pressure
d)
Add a catalyst and decrease the concentration of cyclohexane
57.
The reaction between zinc and hydrochloric acid may be represented by the equation: 
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g); ΔH = -154 kJ mol-1
In an investigation of this reaction using excess Zn and 2 M HCl(aq) in an open flask, the graph shown was plotted from the data collected.
Which of the following would be a suitable quantity for the vertical axis of the graph?
a)
Number of collisions per second.
b)
Rate of reaction.
c)
Temperature.
d)
Number of ion.
58.
The equation and energy profile for combustion of methane is shown. 
According to the information provided on this profile, the activation energy for the reaction:
0.5CO2(g) + H2O(g) → 0.5CH4(g) + O2(g)
would be
a)
1635 kJ
b)
2135 kJ
c)
2490 kJ
d)
4270 kJ
59.
The main reason for the use of catalysts in most industrial processes is to
a)
reduce greenhouse gas emissions
b)
reduce the energy requirement for a reaction
c)
reduce waste production
d)
increase the yield of product
60.
Which of the following changes that can be made to a chemical reaction will result in a greater proportion of successful collisions between reactant particles?
I. addition of a catalyst
II. grinding reactant lumps into a powder
III. increasing the concentration of reactants
a)
I only
b)
II and III only
c)
I and II only
d)
I, II and III
61.
Which of the following statements regarding the energy changes for a particular exothermic chemical reactions is NOT correct?
a)
The activation energy of the forward reaction is lower than the activation energy of the reverse reaction.
b)
The enthalpy value of the products is lower than the enthalpy value of the reactants.
c)
The value of the activation energy of the reverse reaction is lower than the change in enthalpy value.
d)
The forward and reverse reactions both require the absorption of some energy.
62.
Consider the provided energy profile for a particular reaction.
Which of the following is an incorrect conclusion from the data presented?
a)
It takes more energy to break the bonds in the reactants than the energy released when the products form.
b)
The activation energy of the reverse reaction is x+y
c)
The magnitude of the heat of reaction is equal to z-x
d)
When the products form, after bonds in the reactants are broken, energy equivalent to x+y-z is released.
63.

Reaction between calcium carbonate and hydrochloric acid will produce what type of gas?

a)

CO2 gas

b)

H2 gas

c)

O2 gas

d)

Cl2 gas

64.
A solution of hydrogen peroxide releases oxygen slowly at room temperature.
 hydrogen peroxide → water + oxygen
 The diagrams show the effect of adding blood to the solution. What could be the reason for the observed change? 
a)
Blood contains an enzyme. 
b)
Blood contains water. 
c)
The hydrogen peroxide becomes more concentrated. 
d)
The hydrogen peroxide is neutralised by blood. 
65.
Calcium carbonate reacts with hydrochloric acid to form carbon dioxide. Which changes would slow this reaction down?
 1  decreasing the concentration of hydrochloric acid
 2  decreasing the particle size of calcium carbonate
3  decreasing the temperature 
a)
1 and 2 only 
b)
1 and 3 only 
c)
2 and 3 only 
d)
1, 2 and 3 
66.
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]
67.
A reaction has the rate law: Rate = k [A][B].
What will happen to the rate of reaction if the concentration of A is doubled and the concentration of B is tripled?
a)
increases by a factor of 3
b)
increases by a factor of 4
c)
increases by a factor of 5
d)
increases by a factor of 6
68.
The rate law for the reaction 2NO(g) + O2(g) → 2NO2(g) is first order in O2 and third order overall. What is the rate law for the reaction?
a)
Rate = k [NO]2[O2]2
b)
Rate = k [NO]1[O2]2
c)
Rate = k [NO]2[O2]1
d)
Rate = k [2NO]2[O2]1
69.

The only factor that can change the value of k is:

a)

concentration

b)

pressure

c)

surface area

d)

temperature

70.

For the reaction: 2HI → 2H2 + I2


If HI is first order, which of the following will yield a linear plot?

a)

log [HI] vs time

b)

1/[HI] vs time

c)

[HI]2 vs time

d)

[HI] vs time

e)

ln[HI] vs time

71.

For the reaction: 2HI → 2H2 + I2


If HI is first order, which of the following will yield a negative exponential plot?

a)

log [HI] vs time

b)

1/[HI] vs time

c)

[HI]2 vs time

d)

[HI] vs time

e)

ln[HI] vs time

72.

For the reaction: 2HI → 2H2 + I2


If HI is second order, which of the following will yield a linear plot?

a)

log [HI] vs time

b)

1/[HI] vs time

c)

[HI]2 vs time

d)

[HI] vs time

e)

ln[HI] vs time

73.

For which order reaction is the half-life of the reaction independent of the initial concentration of the reactant(s)?

a)

zero order

b)

first order

c)

second order

d)

all of these

e)

none of these

74.
Which two trials would you use to find the rate exponent for A?
a)
trials 1 and 2
b)
trials 1 and 3
c)
trials 2 and 3
75.
The following data were measured for the reaction BF3(g) + NH3(g) —> F3BNH3(g)
What is the rate law for the reaction? 
a)
R=K[NH3]
b)
R=K[BF3]2[NH3]
c)
R=K[BF3][NH3]
d)
R=K[BF3][NH3]2
76.
A reaction was found to be third order in A. Increasing the concentration of A by a factor of 3 will cause the reaction rate to __________. 
a)
increase by a factor of 27 
b)
increase by a factor of 9 
c)
triple 
d)
decrease by a factor of the cube root of 3  
77.
Write the rate expression for the disappearance of hydrogen according to the following balanced equation: H2 + O2→H2O
a)
ΔH2 / Δt
b)
-ΔH2 / Δt
c)
Δt  / ΔH2 
d)
-Δt  / ΔH2 
78.

Consider the reaction and its rate law given below.

2 A (g) + B(g) --> 2 C(g)

Rate = k[A][B]

At the beginning of one trial of this reaction, [A] = 3.0 M and [B] = 1.0 M. The observed rate for the formation of C is 0.36 mol L-1 s-1.

The numerical value of k, the rate constant is closest to

a)

0.040

b)

0.12

c)

108

d)

6.0

79.

State the equation shown in diagram below

a)

Activation energy

b)

Arrhenius equation

c)

Rate equation

d)

Arrhenius Constant

80.
The following statements are true EXCEPT
a)
k is rate constant
b)
It is Maxwell Boltzmann equation
c)
shaded portion is fraction molecules with energy > Ea
d)
A is orientation factor and collision frequency
81.
Plot below is used to calculate activation energy. What is x and y axis?
a)
x = T, y = ln k
b)
x = ln k, y = 1/T
c)
x = 1/T, y = ln k
d)
x = T, y = k
82.
Plot below is used to calculate activation energy. How Ea can be calculated?
a)
From the gradient. Gradient = - R/Ea
b)
From the gradient. Gradient = - Ea/R
c)
From the gradient. Gradient = Ea
d)
None of the above
83.
An enzyme speeds up a reaction by
a)
lowering the activation energy.
b)
raising the activation energy.
c)
releasing energy.
d)
absorbing energy.
84.
In a chemical reaction, a reactant binds to an enzyme at a region known as the
a)
catalyst.
b)
product.
c)
substrate.
d)
active site. 
85.
Chemical reactions always involve
a)
the breaking of bonds in reactants.
b)
the formation of new bonds in products.
c)
the breaking of bonds in reactants and the formation of new bonds in products.
d)
enzymes. 
86.
Chemical reactions that release energy often occur 
a)
spontaneously.
b)
nonspontaneously.
c)
rapidly.
d)
slowly. 
87.
Chemical reactions that absorb energy often occur 
a)
spontaneously.
b)
nonspontaneously.
c)
rapidly.
d)
slowly. 
88.
The enzyme catalase speeds up the chemical reaction that changes hydrogen peroxide into oxygen and water. The amount of oxygen given off is an indication of the rate of the reaction. Based on the graph, what can you conclude?
a)
Reaction rate decreases with increasing enzyme concentration.
b)
Reaction rate increases with decreasing enzyme concentration.
c)
Reaction rate increases with increasing enzyme concentration.
d)
The variables are indirectly proportional.
89.
Which concentration of catalase will produce the fastest reaction rate?
a)
5%
b)
10%
c)
15%
d)
20%
90.
What type of catalyst is an enzyme?
a)
Biological
b)
Mechanical
c)
Chemical
d)
Electrical
91.
Which of the factors does NOT affect enzymatic activity?
a)
Temperature
b)
pH
c)
Concentration
d)
Color
92.
What are the PRODUCTS of the chemical reaction pictured?
a)
CH4 and CO2
b)
CH4 and O2
c)
CO2 and H2O
d)
O2 and H2O

Similar Resources on Wayground

Physical Science Unit 2 Review

90 questions

Physical Science Unit 2 Review

quiz

Worksheet

•

9th - 12th Grade

Semester 1 Final Exam Review-Chemistry

94 questions

Semester 1 Final Exam Review-Chemistry

quiz

Worksheet

•

10th - 12th Grade

TEST: Bonding/VESPER/Inter& Intramolecular forces

89 questions

TEST: Bonding/VESPER/Inter& Intramolecular forces

quiz

Worksheet

•

10th - 11th Grade

Full Elements Quiz Review

90 questions

Full Elements Quiz Review

quiz

Worksheet

•

9th - 12th Grade

C09 Electron Dot Structure

88 questions

C09 Electron Dot Structure

quiz

Worksheet

•

9th - 12th Grade

Chem01.1 Alchemy and Scientific Method

89 questions

Chem01.1 Alchemy and Scientific Method

quiz

Worksheet

•

11th Grade

ÔN TÂP HK1-HOA 10

90 questions

ÔN TÂP HK1-HOA 10

quiz

Worksheet

•

10th - 12th Grade

Unit Test #1 Chemistry

90 questions

Unit Test #1 Chemistry

quiz

Worksheet

•

9th - 12th Grade