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Reaction Rates and Equilibrium

Total questions: 67

Worksheet time: 44mins

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.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
6.

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

7.
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.
8.
Located on the left side of the reaction
a)
reactants
b)
products
9.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
10.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
11.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
12.
What is the activation energy?
a)
the quantity of heat absorbed in a reaction
b)
the minimum energy needed to begin a reaction
c)
the energy given off after reactants collide.
d)
both the energy and frequeny of collisions in increased
the energy difference between reactants and products
13.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
14.
For the reaction...
SO2 + O2 <=>  SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
15.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
16.
For the reaction...
N2 (g) +  3 H2 (g) <=> 2 NH3 (g)

If the pressure in the system is increased,  which substance(s) will increase in concentration?
a)
N2  (as 2 mol gas  → 4 mol gas)
b)
H2 (as 2 mol gas  → 4 mol gas)
c)
N2 and H2 (as 2 mol gas  → 4 mol gas)
d)
NH3 (as 4 mol gas  → 2 mol gas)
17.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
18.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
19.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
20.
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
21.
Increasing the concentration of the reactants will slow down the reaction.
a)
false 
b)
true
22.
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
23.
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 because there are more collision sites
24.
Which of these will NOT speed up the rate of reaction between a strip of magnesium and hydrochloric acid?
a)

roll the magnesium strip into a small ball

b)

Grind up the strip of magnesium

c)
increase the concentration of the hydrocholoric acid
d)
increase the temperature of the hydrocholoric acid
25.

When we investigate the rate of reaction we are looking at the...

a)

amount of product formed

b)

speed of reaction

c)

concentration of reacting particles

d)

combining reactants with products

26.
You add more bodies into a "mosh pit" to hope for more collisions.  You have increased-
a)
temperature
b)
concentration
c)
pressure
d)
catalyst
27.
To slow down a chemical reaction you will do one of the following:
a)

Place the reaction in hot water

b)

Add more reactants

c)

Place the reaction in a ice bath

d)
Keep stirring the reactants with a stirring rod
28.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

29.

The major theory of reaction rate is called

a)

Collision theory

b)

Crash theory

c)

Newton's laws

d)

Thermodynamics

30.

You know that a chemical reaction is occurring here because you see __________________ . (Pick 3)

a)

purple color

b)

smoke

c)

ice formation

d)

fire

e)

a yellow precipitate

31.

In this chemical reaction, what was the first evidence that you saw?

a)

Production of fire

b)

Production of light

c)

Production of purple smoke

d)

Production of white powder

32.

When zinc reacted with hydrochloric acid, what was the result of this reaction?

a)

a white powder

b)

a blue liquid

c)

a brown precipitate

d)

a gas

33.

Which of the following is evidence of a chemical reaction?

a)

Tearing paper.

b)

Change in color.

c)

Production of a gas.

d)

Change in temperature.

e)

Production of a precipitate.

34.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

35.

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

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

36.
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.
37.
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
38.

A catalyst be regenerated or used again and again

a)

False

b)

True

39.
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
40.

Rank the state os matter from FASTEST to SLOWEST particle speed.

a)

solid, liquid, gas

b)

liquid, solid, gas

c)

gas, liquid, solid

d)

gas, solid, liquid

41.

The higher the temperature a substance has the

a)

more energy it has

b)

less energy it has

42.

In a solution when particles collide, most of the collisions

a)

are successful

b)

are unsuccessful

c)

result in a chemical reaction

d)

do not result in a chemical reation

43.

What factors affect reaction rate?

a)

size of atoms

b)

temperature

c)

concentration

d)

surface area

e)

catalysts

44.

A log is burning in a campfire. If the concentration of oxygen reaching the log is increased, what will happen to the reaction rate?

a)

reaction rate decreases

b)

reaction rate increases

c)

reaction rate remains the same

45.

What is necessary for a chemical reaction to occur?

a)

Correct orientation of particles when they collide

b)

particle collisions

c)

an increase or decrease in temperature

d)

particle collisions with sufficient energy

e)

a catalyst

46.

What happens to reaction rate if surface area is decreased?

a)

it increases

b)

it decreases

c)

it stays the same

47.

What happens to reaction rate when a reactants concentration is increased?

a)

it increases

b)

it decreases

c)

it remains the same

48.

What happens to reaction rate when temperature is decreased?

a)

it increases

b)

it decreases

c)

it stays the same.

49.

What does a catalyst do to speed up a reaction?

a)

It reduces the surface area of the reactants

b)

It increases the surface area of the reactants.

c)

It reduces the required energy for a chemical reaction to occur

d)

It increases the required energy for a chemical reaction to occur

50.

A reactants surface area is increased. What happens?

a)

more collisions occur

b)

the same number of collisions occur

c)

greater collision energy

d)

less collision energy

e)

the same collision energy

51.

A reactants concentration is increased. What happens?

a)

more collisions occur

b)

the same number of collisions occur

c)

greater collision energy

d)

less collision energy

e)

the same collision energy

52.

A reactants temperature is increased. What happens?

a)

more collisions occur

b)

the same number of collisions occur

c)

greater collision energy

d)

less collision energy

e)

the same collision energy

53.

The minimum quantity of energy which the reacting species must possess in order to undergo a specific reaction.

a)

collision theory

b)

activation energy

c)

reaction rate

d)

chemical reaction

54.

the rate at which a chemical reaction takes place

a)

activation energy

b)

collision theory

c)

reaction rate

d)

chemical reactions

55.

A substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change.

a)

catalyst

b)

products

c)

reactants

d)

chemical reaction

56.

A substance that takes part in and undergoes change during a reaction.

a)

products

b)

reactants

c)

catalyst

d)

collision

57.

A substance that is formed as the result of a chemical reaction.

a)

products

b)

reactants

c)

catalyst

d)

collision

58.

Describes the 3 reasons chemical reactions occur.

a)

collision theory

b)

reaction rate

c)

chemical reaction

d)

activation energy

59.

A process that involves rearrangement of the molecular or ionic structure of a substance, as opposed to a change in physical form or a nuclear reaction.

a)

collision theory

b)

reaction rate

c)

chemical reaction

d)

activation energy

60.

Which of the following is NOT true at equilibrium?

a)

The forward and reverse reactions proceed at the same rate.

b)

The amount (concentration) of reactants and products do not change.

c)

The amount (concentration) of the reactants is equal to the concentration of the products.

d)

The forward and reverse reactions continue to occur.

61.

During equilibrium, the rates of the forward and the reverse reaction are ________

a)

equal

b)

unequal

c)

unequal for exothermic reactions

d)

unequal for endothermic reactions

62.

Around what time does the reaction reach equilibrium?

a)

25 min

b)

70 min

c)

45 min

d)

80 min

63.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
64.
dynamic equilibrium
a)
condition of continuous, random movement of particles but no overall change in concentration of materials
b)
the process by which one or more substances change to produce one or more different substances
c)
a condition where the reaction occurring in a system is completely halted and there exists no movement between the reactants and the products corresponding to the chemical reaction
d)
a substance that takes part in and undergoes change in a chemical reaction
65.
static equilibrium
a)
condition of continuous, random movement of particles but no overall change in concentration of materials
b)
the reaction that forms reactants from products
c)
a condition where the reaction occurring in a system is completely halted and there exists no movement between the reactants and the products corresponding to the chemical reaction
d)
a measurement of how much solute exists within a certain volume of solvent or solution
66.
reactant
a)
the reaction that forms products from reactants
b)
a measurement of how much solute exists within a certain volume of solvent or solution
c)
a substance that takes part in and undergoes change in a chemical reaction
d)
condition of continuous, random movement of particles but no overall change in concentration of materials
67.
product
a)
condition of continuous, random movement of particles but no overall change in concentration of materials
b)
a measurement of how much solute exists within a certain volume of solvent or solution
c)
a substance that forms in a chemical reaction
d)
the reaction that forms products from reactants

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