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energetics and kinetics

Total questions: 54

Worksheet time: 33mins

Name
Class
Date
1.

Which reaction is endothermic?

a)

acid neutralising alkali causing a temperature increase

b)

adding magnesium to hydrochloric acid

c)

calcium carbonate decomposing when heated combustion of fossil fuels

2.

Which statements about exothermic and endothermic reactions are correct?

a)

During an exothermic reaction, heat is given out

b)

The temperature of an endothermic reaction goes up because heat is taken in

c)

Burning methane in the air is an exothermic reaction

3.

Which is an endothermic process?

a)

Burning hydrogen

b)

Distilling petroleum

c)

Reacting potassium with water

d)

Using petrol in a motor car engine

4.

Which fuel does not produce carbon dioxide when it burns?

a)

Coal

b)

Hydrogen

c)

Methane

5.

Statement 1 Hydrogen is used as a fuel.

Statement 2 When hydrogen burns in the air to form water, heat energy is produced.

Which is correct?

a)

Both statements are correct and statement 2 explains statement 1

b)

Both statements are correct but statement 2 does not explain statement 1

c)

C Statement 1 is correct but statement 2 is incorrect

6.

Some white anhydrous copper(II) sulfate powder is put into a beaker of water and stirred. What would show that the process was exothermic?

a)

A blue solution is formed

b)

The beaker feels cooler

c)

The beaker feels warmer

7.

Which of the following is true about the formation of bonds between molecules?

a)

Energy is given off when bonds are formed between molecules.

b)

Energy is absorbed by the molecule when bonds are formed.

c)

Energy is neither given off nor absorbed when bonds are formed.

8.

Which of the following statement is true about the breaking of bonds between molecules?

a)

To break a bond between molecules, energy must be released by the molecule

b)

To break a bond between molecules, no energy is needed.

c)

To break a bond between molecules, energy must be absorbed by the molecule.

9.
Which letter corresponds to the energy of the products?
a)
A
b)
B
c)
C
d)
D
10.
If ∆H is negative, the reaction is?
a)
exothermic
b)
endothermic
11.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
12.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
13.

The initial temperature was measured to be 20oC and the final temperature was 10oC. The reaction was

a)

exothermic

b)

endothermic

14.

The initial temperature was measured to be 20oC and the final temperature was 45oC. The reaction was

a)

exothermic

b)

endothermic

15.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
16.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

17.

The graph above is from which type of reaction?

a)

Endothermic reaction

b)

Exothermic reaction

18.
Melting 
a)
exothermic
b)
endothermic
19.

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

20.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
21.
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)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
22.
Why does a catalyst increase the rate of reaction?
a)
it produces extra energy for the reactants
b)
it increases the speed of the reactant particles
c)
it increases the frequency of particle collisions
d)
it reduces the activation energy of the reaction 
23.
Which of the following increase the reaction rate?
a)
less surface area
b)
lower temperature
c)
an inhibitor
d)
increased concentration
24.
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
25.
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
26.
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
27.

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

28.

What does the M after a concentration value stand for?

a)

meters

b)

music

c)

Molarity

d)

moles

29.

The major theory of reaction rate is called

a)

Collision theory

b)

Crash theory

c)

Newton's laws

d)

Thermodynamics

30.

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

31.

Which graph shows the effect of increasing temperature on the rate of reaction of calcium carbonate with dilute hydrochloric acid?

a)
b)
c)
d)
32.
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
33.
In an experiment, a 2 g lump of zinc and 2 g of powdered zinc are added separately to equal volumes of dilute sulphuric acid. The solid line on the graph shows the volume of gas given off when the 2 g lump is used. Which dotted line is obtained when the zinc is powdered? 
a)
A
b)
B
c)
C
d)
D
34.
A student investigated the rate of reaction of calcium carbonate with dilute hydrochloric acid. Every minute, the student recorded the total volume of carbon dioxide produced, until some time after the reaction was complete.
Which graph shows the correct results? 
a)
A
b)
B
c)
C
d)
D
35.
Order the letters from highest to lowest rate of reaction.
a)
A > B > C > D
b)
A > BC > D (B and C have the same rate)
c)
A > B > CD (C and D have the same rate)
d)
D > C > B > A
36.
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
37.
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.
38.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
39.

A student reacted a carbonate with an acid and measured the volume of carbon dioxide gas at regular intervals. Between which two times was the reaction fastest?

a)

0-2 minutes

b)

2-4 minutes

c)

4-6 minutes

d)

8-10 minutes

40.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

41.

Which colour on the graph would represent the solution with the higher temperature?

a)

Red

b)

Blue

c)

None

d)

Both

42.
What type of reaction is this?
a)

Endothermic

b)

Exothermic

c)

Physical

d)

Chain

43.
In an endothermic reaction the products have 
a)
more energy than the reactants
b)
less energy than the reactants
c)
the same energy as the reactants
d)
no energy
44.

Which group of particles shows that increasing surface area increases collisions among particles?

a)

Left side

b)

Right side

c)

Cannot be determined by either picture

45.

From the data given, calculate the average rate at which A disappears over the time interval from 20 s to 40 s.

Average Rate = −Δ[A]ΔtAverage\ Rate\ =\ -\frac{\Delta\left[A\right]}{\Delta t}  

4 lines
46.

Calculate the average rate of the appearance of B over the time interval from 0 to 40 s. 

4 lines
47.

Which of the following is not a correct statement about the effect of a catalyst?

a)

Provides an alternative route to the products

b)

Lowers the energy which molecules need for successful collisions

c)

Provides energy so that more molecules have successful collisions

d)

Reactant molecules form weak bonds on active sites

48.

You were asked to find the instantaneous rate of the reaction at 60 seconds in terms of g/s carbon dioxide produced. calculate using the points (20,0.14) (100,0.35). Pick the correct answer

a)

2.3 x 10¯³g/s

b)

2.625 x 10¯³g/s

c)

2.625 x 10¯³kg/s

d)

2.3 x 10¯³kg/s

49.

Hydrogen and Iodine gas react to form hydrogen iodide, as shown in the equation H2 + I2 → 2HI. Suppose you are given a time interval from t1=10 sec and t2=20 sec where the change in H2 concentration from 0.210 mol/L to 0.185 mol/L. Calculate the average reaction rate in that period.

(a)  

50.

What quantity is defined by the rate of decomposition of a reactant at a specific time?

a)

Specific rate constant

b)

Rate order

c)

Instantaneous rate

d)

Catalyst

51.

The term that describes the change in the concentration of a reactant divided by the change in time of the reaction is the ______________.

a)

Rate constant

b)

Average reaction rate

c)

Activated complex

d)

Chemical reaction

52.

Catalyst helps to

a)

increase the amount of product obtained

b)

to lower the activation energy

c)

provide an alternative reaction route

d)

decrease the frequency of collision

53.
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
54.

What is collision theory?

a)

Molecules must collide in the correct orientation with enough energy to bond.

b)

Molecules need enough energy to collide and react.

c)

Atoms constantly collide and react.

d)

The minimum energy needed for atoms to react

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