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Factors Affecting Reaction Rates

Total questions: 60

Worksheet time: 1hrs 28mins

Name
Class
Date
1.
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
2.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
3.
Reaction rate means...
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
4.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
5.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
6.

The catalyst alters the rate of a chemical reaction by,

a)

providing an alternative pathway with a lower Ea

b)

changing the products formed in the direction of the reaction

c)

providing a surface on which the molecules react

d)

increasing the frequencies of collisions between molecules

7.

Which of the following are true of reaction rates?

I. The overall rate law is determined by the fastest step of a reaction

II. The presence of a catalyst will increase the number of molecules entering the transition state

III. An increase in temperature will increase the rate of a reaction

IV. Decreasing the concentration of reactants will increase the rate at which products yield

a)

II+III+IV

b)

I+IV

c)

II + III

d)

I+II+III

8.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing surface area

d)

all of the above

9.

What letter represents the activation energy?

a)

A

b)

B

c)

C

d)

D

10.
Usually lowering the temperature will slow down a reaction.
a)
false
b)
true
11.
Catalysts permit reactions to happen with a __________ activiation energy.
a)
lower
b)
higher
12.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
13.
What are the two criteria for a collision to be effective?
a)
proper orientation and particle size
b)
enough energy to overcome the activation energy and proper orientation
c)
enough energy to overcome the activation energy and homogeneity
d)
proper orientation and heterogeneity
14.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
15.

Based on the collision model, the atoms in the top of potential energy ‘’hill’’ are called

a)

Top of hill

b)

Activation energy

c)

Transition state

d)

Steric factor

16.

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.

17.

Which of the following statements about the catalyst is true?

a)

A catalyst accelerates the rate of reaction by bringing down the activation energy.

b)

A catalyst does not participate in reaction mechanism.

c)

A catalyst makes the reaction feasible by making ∆G more negative.

d)

A catalyst makes equilibrium constant more favorable for forward reaction.

18.

An endothermic reaction with high activation energy for the forward reaction is given by the diagram.

a)

A

b)

B

c)

C

d)

D

19.
To measure rate of reaction, we can monitor change in which of the following?
a)
Reactants only
b)
Products only
c)
Reactants or products
20.

4 factors that affects reaction rate.

a)

temperature

b)

surface area

c)

presence of catalyst

d)

Chemical nature of reactant

e)

In solid form

21.
Grinding a seltzer tablet into powder increases the rate of reaction due to...
a)
increased concentration of reactants
b)
increased surface area
c)
increased speed of particles.
d)
better orientation of reactants
22.

An addition of a catalyst to the following reaction would have what effect?

a)

A would be increased

b)

B would be increased

c)

C would be decreased

d)

No change

23.

Which sample of HCl(aq) reacts at the fastest rate with a 1.0-gram sample of iron filings?

a)

10 mL of 1 M HCl(aq) at 10°C

b)

10 mL of 1 M HCl(aq) at 25°C

c)

10 mL of 3 M HCl(aq) at 10°C

d)

10 mL of 3 M HCl(aq) at 25°C

24.

During a laboratory activity to investigate reaction rate, a student reacts 1.0-gram samples of solid zinc with 10.0-milliliter samples of HCl(aq). The table below shows information about the variables in five experiments the student performed. Which two experiments can be used to investigate the effect of the concentration of HCl(aq) on the reaction rate?

a)

1 and 3

b)

1 and 5

c)

4 and 2

d)

4 and 3

25.

For a given chemical reaction, the addition of a catalyst provides a different reaction pathway that

a)

decreases the reaction rate and has a higher activation energy

b)

decreases the reaction rate and has a lower activation energy

c)

increases the reaction rate and has a higher activation energy

d)

increases the reaction rate and has a lower activation energy

26.

Each of four test tubes contains a different concentration of HCl(aq) at 25°C. A 1-gram cube of Zn is added to each test tube. In which test tube is the reaction occurring at the fastest rate?

a)

1

b)

2

c)

3

d)

4

27.

A 5.0-gram sample of zinc and a 50.-milliliter sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the fastest reaction rate?

a)

a zinc strip and 1.0 M HCl(aq)

b)

a zinc strip and 3.0 M HCl(aq)

c)

zinc powder and 1.0 M HCl(aq)

d)

zinc powder and 3.0 M HCl(aq)

28.

Adding a catalyst to a chemical reaction results in

a)

a decrease in activation energy and a decrease in the reaction rate

b)

a decrease in activation energy and an increase in the reaction rate

c)

an increase in activation energy and a decrease in the reaction rate

d)

an increase in activation energy and an increase in the reaction rate

29.

Which conditions will increase the rate of a chemical reaction?

a)

decreased temperature and decreased concentration of reactants

b)

decreased temperature and increased concentration of reactants

c)

increased temperature and decreased concentration of reactants

d)

increased temperature and increased concentration of reactants

30.

Given the reaction at equilibrium: N2(g) + 3H2(g) ⇌ 2NH3(g). Increasing the concentration of N2(g) will increase the forward reaction rate due to

a)

an increase in the number of effective collisions

b)

a decrease in the number of effective collisions

c)

a decrease in the activation energy

d)

an increase in the activation energy

31.

A 1-cubic-centimeter cube of sodium reacts more rapidly in water at 25°C than does a 1-cubic-centimeter cube of calcium at 25°C. The difference in rate of reaction is most closely associated with the different

a)

surface area of the metal cubes

b)

nature of the metals

c)

density of the metals

d)

concentration of the metals

32.

A chemical reaction occurs when reactant particles

a)

are separated by great distances

b)

have no attractive forces between them

c)

collide with proper energy and proper orientation

d)

convert chemical energy into nuclear energy

33.

A reaction is most likely to occur when the colliding particles have proper orientation and

a)

mass

b)

volume

c)

half-life

d)

energy

34.

An effective collision between reactant particles requires the particles to have the proper

a)

charge and mass

b)

charge and orientation

c)

energy and mass

d)

energy and orientation

35.

What is required for a chemical reaction to occur?

a)

standard temperature and pressure

b)

a catalyst added to the reaction system

c)

effective collisions between reactant particles

d)

an equal number of moles of reactants and products

36.

A chemical reaction between iron atoms and oxygen molecules can only occur if

a)

the particles are heated

b)

the atmospheric pressure decreases

c)

there is a catalyst present

d)

there are effective collisions between the particles

37.

As the concentration of reacting particles increases, the rate of reaction generally

a)

decreases

b)

increases

c)

remains the same

38.

Increasing the temperature increases the rate of a reaction by

a)

lowering the activation energy

b)

increasing the activation energy

c)

lowering the frequency of effective collisions between reacting molecules

d)

increasing the frequency of effective collisions between reacting molecules

39.

Given the balanced equation representing a reaction:

2HCl(aq) + Na2S2O3(aq) → S(s) + H2SO3(aq) + 2NaCl(aq)

Decreasing the concentration of Na2S2O3(aq) decreases the rate of reaction because the:

a)

activation energy decreases

b)

activation energy increases

c)

frequency of effective collisions decreases

d)

frequency of effective collisions increases

40.

What is the relationship between rate of reaction and temperature?

a)

No relationship

b)

Directly proportional

c)

Inversely proportional

d)

Jointly proportional

41.

Given the reaction inside a container of CO2(g) + H2O(g) →\rightarrow H2CO3(aq).

What will happen if the pressure of the container is increased?

a)

The rate increases

b)

The rate decreases

c)

The rate will remain the same

d)

It has no effect

42.

What is the relationship between rate of reaction and concentration of reactants?

a)

No relationship

b)

Directly proportional

c)

Inversely proportional

d)

Jointly proportional

43.

How does the presence of catalyst increase reaction rate?

a)

It lowers down activation energy

b)

It increases collision of particles

c)

It increases the energy of the reactant

d)

It increases activation energy

44.

change in concentration, Δ[conc]change in time, Δ t\frac{change\ in\ concentration,\ \Delta\left[conc\right]}{\text{change in time, }\Delta\ t} = ?

a)

Rate of reaction

b)

constant, k

c)

rate law

d)

reaction order

45.

The following are the terms used to describe the relationship between the rate of a chemical reaction and the concentration of its reactants EXCEPT

a)

Rate laws

b)

Differential rate laws

c)

Rate equations

d)

Chemical kinetics

46.

The rate constant of a reaction is 5.8 ×\times 10 M-1s-1. The order of the reaction is...

a)

0th order

b)

1st order

c)

2nd order

d)

3rd order

47.

The plot shows the decomposition of H2O2.

What is the order of the reaction?

a)

0th order

b)

1st order

c)

2nd order

d)

3rd order

48.

The half-life of a first-order reaction...

a)

is constant

b)

is the time necessary for the reactant concentration to drop

to half its original value

c)

does not depend on the initial reactant concentration

d)

All of the choices are correct

49.

What is the half-life (t1/2) of a reactant with a decay constant (λ)\left(\lambda\right) of 0.693?

a)

1

b)

2

c)

3

d)

4

50.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
51.
Reaction rate means...
a)
amount of product formed
b)
speed of reaction
c)
concentration of reacting particles
d)
combining reactants with products
52.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
53.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
54.
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]
55.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate law for the reaction?

a)

rate = k[NH3]

b)

rate = k[BF3]2[NH3]

c)

rate = k[BF3][NH3]

d)

rate = k[BF3][NH3]2

56.

Given the following rate law,

rate = k[A]2[B]

if [A] were doubled, what must happen to [B] to keep the rate constant?

a)

[B] must quadruple

b)

[B] must double

c)

[B] must be havled

d)

[B] must be quartered

57.

The catalyst alters the rate of a chemical reaction by,

a)

providing an alternative pathway with a lower Ea

b)

changing the products formed in the direction of the reaction

c)

providing a surface on which the molecules react

d)

increasing the frequencies of collisions between molecules

58.

Which of the following are true of reaction rates?


I. The overall rate law is determined by the fastest step of a reaction


II. The presence of a catalyst will increase the number of molecules entering the transition state


III. An increase in temperature will increase the rate of a reaction


IV. Increasing the concentration of reactants will increase the rate at which products yield

a)

II+III+IV

b)

I+IV

c)

II + III

d)

I+II+III

59.

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?

a)

rate = [OCl-]2[I-]

b)

rate = [OCl-][I-]2

c)

rate = [OCl-][I-]

d)

rate = [OCl-]

60.

Units of rate is _______-

a)

M/s

b)

mol/s

c)

m.s

d)

s/M

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