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Reaction Rates

Total questions: 21

Worksheet time: 16mins

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.

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.

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

8.

The ______________is required to break the bonds of the reactants.

a)

Carbonic energy

b)

Activation energy

c)

Plutonic energy

d)

Energi Gaib

9.
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.
10.
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
11.
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
12.

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

13.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
14.
A substance that increases speed of chemical reaction without being being changed is called:
a)
Catalyst
b)
Acid
c)
Base
d)
pressure
15.
The amount of a substance in a given volume.
a)
concentration
b)
temperature
c)
surface area
d)
catalyst
16.
Exposing more particles for collisions is an increase in 
a)
concentration
b)
surface area
c)
temperature
d)
catalyst
17.
Increasing the concentration increases the speed of reaction by
a)
lowering activation energy
b)
increasing collisions
c)
speeding up the reactants
d)
exposing more reactant
18.
Which of the following slows down the rate of a chemical reaction?
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
19.
If more reactants are used in a chemical reaction, more products will be produced. This is because
a)
More reactants cause the reaction to heat up
b)
More reactants take up the same volume
c)
More reactants have more atoms to react to form more products
d)
Too many products can slow down the reaction
20.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
21.

When surface area is decreased the rate of reaction...

a)

Decreases, because there are LESS possible sites for correct collisions

b)

Increases, because there are LESS possible sites for correct collisions

c)

Decreases, because there are MORE possible sites for correct collisions

d)

Increases, because there are MORE possible sites for correct collisions

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