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Kinetics and equilibrium test another retake

Total questions: 53

Worksheet time: 59mins

Name
Class
Date
1.

What is equal in equilibrium reactions?

a)

The concentrations of products and reactants

b)

the products equals the heat of reaction

c)

the rate of the forward and reverse reaction

d)

the heat of reaction equals the activation energy

2.

SO2 + 1/2 O2 = SO3

Once equilibrium is reached, the concentration of SO2 is increased, which way does the reaction shift?

a)
left
b)
right
3.

SO2 + 1/2 O2 = SO3

As soon as SO3 is created, it dissolves in water and is washed away.  Which way does this shift the equilibrium?

a)
left
b)
right
4.
When temperature is increased, the reaction shifts to the left.  This reaction must be
a)
exothermic
b)
endothermic
5.

CaCO3 --> CaO + CO2

If pressure is increased, which way does the reaction shift?

a)
toward products
b)
toward reactants
c)
no change
6.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is conctant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
7.

Identify the incorrect statement about achieving equilibrium.

a)

achieved when product and reactant concentrations are equal

b)

achieved when forward and reverse reaction rates are same

c)

achieved when concentration of reactants is stable/constant

d)

achieved when concentration ratio of reactants to products becomes stable, thus fixing the equilibrium constant (equilibrium position)

8.
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
9.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
10.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product
11.
How does a catalyst change during a reaction?
a)
It is part of the products
b)
It combines with the reactants
c)
It precipitates
d)
It remains unchanged
12.
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
13.
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
14.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
15.
For the reaction...
H2 (g)  + Cl2 (g) <=>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium position will _______.
a)
shift to the left
b)
shift to the right
c)
not shift position at all as 2 mol gas <=> 2 mol gas
16.

Given the reaction:

CH4(g) + 2O2(g) --> 2H2O(g) + CO2(g)

What is the overall result when CH4(g) burns according to this reaction?

a)

Energy is released and the ΔH is positive

b)

Energy is released and the ΔH is negative

c)

Energy is absorbed and the ΔH is positive

d)

Energy is absorbed and the ΔH is negative

17.

Which statement correctly describes an endothermic chemical reaction?

a)

The products have lower potential energy than the reactants, and the ΔH is positive

b)

The products have lower potential energy than the reactants, and the ΔH is negative

c)

The products have higher potential energy than the reactants, and the ΔH is positive

d)

The products have higher potential energy than the reactants, and the ΔH is negative

18.

Which balanced equation represents an endothermic reaction?

a)

N2(g) + 3H2(g) --> 2NH3(g)

b)

N2(g) + O2(g) --> 2NO(g)

c)

CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l)

d)

C(s) + O2(g) --> CO2(g)

19.

Given the reaction


S(s) + O2(g) --> SO2(g) + energy


Which diagram best represents the potential energy changes for this reaction?

a)

a

b)

b

c)

c

d)

d

20.

The potential energy diagram below represents a reaction.


Which arrow represents the activation energy of the forward reaction

a)

A

b)

B

c)

C

d)

D

21.

Given the potential energy diagram for the chemical reaction:


Which statement correctly describes the energy changes that occur in the forward reaction

a)

The activation energy is 50kJ and the reaction is exothermic

b)

The activation energy is 50kJ and the reaction is endothermic

c)

The activation energy is 10kJ and the reaction is exothermic

d)

The activation energy is 10kJ and the reaction is endothermic

22.

Increasing the temperature increases the rate of a reaction by

a)

lowering the activation energy

b)

increasing the frequency of effective collisions between reacting molecules

c)

lowering the frequency of effective collisions between reacting molecules

d)

increasing the activation energy

23.

The beakers shown below, a 2.0 centimeter strip of magnesium ribbon reacts with 100 milliliters of HCl(aq) under the conditions shown


In which beaker will the reaction occur at the fastest rate?

a)

A

b)

B

c)

C

d)

D

24.

At STP, which 4.0-gram zinc sample will react fastest with dilute hydrochloric acid?

a)

sheet metal

b)

powdered

c)

bar

d)

granules

25.

Which statement best explains the role of a catalyst in a chemical reaction?

a)

A catalyst changes the kinds of products produced

b)

A catalyst provides an alternate reaction pathway that requires less activation energy

c)

A catalyst limits the amount of reactants used

d)

A catalyst is added as an additional reactant and is consumed but not regenerated

26.

which phase change represents a decrease in entropy?

a)

solid to gas

b)

liquid to gas

c)

solid to liquid

d)

gas to liquid

27.

Which sample has the lowest entropy?

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of KNO3(aq)

d)

1 mole of KNO3(g)

28.

Which process is accompanied by a decrease in entropy?

a)

boiling of water

b)

melting of ice

c)

condensation of water

d)

subliming of iodine

29.

Given the balanced equation


Which statement best describes this proces

a)

It is endothermic and entropy decreases

b)

It is endothermic and entropy increases

c)

It is exothermic and entropy decreases

d)

It is exothermic and entropy increases

30.

Systems in nature tend to undergo changes toward

a)

lower energy and lower entropy

b)

lower energy and higher entropy

c)

higher energy and lower entropy

d)

higher energy and higher entropy

31.
If a catalyst is added to a system at equilibrium and the temperature and pressure remain constant, there will be no effect on the
a)
rate of the forward reaction
b)
activation energy of the reaction
c)
rate of the reverse reaction
d)
heat of reaction
32.
Two reactant particles collide with proper orientation.The collision will be effective if the particles have
a)
high activation energy
b)
high ionization energy
c)
sufficient kinetic energy
d)
sufficient potential energy
33.
Adding a catalyst to a chemical reaction changes the rate of reaction by causing
a)
a decrease in the activation energy
b)
an increase in the activation energy
c)
a decrease in the heat of reaction
d)
an increase in the heat of reaction
34.
When one mole of a certain compound is formed from its elements under standard conditions, it absorbs 85 kiloJoules of heat. A correct conclusion from this statement is that the reaction has a
a)
ΔH equal to –85 kJ/mole
b)
ΔH equal to +85 kJ/mole
c)
 Δequal to –85 kJ/mole
d)
 Δequal to +85 kJ/mole
35.
Which interval represents the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
E
36.
Which interval represents the heat of reaction for the reaction?
a)
A
b)
B
c)
D
d)
E
37.
Which numbered interval on the diagram would change when a catalyst is added?
a)
B & C
b)
C & D 
c)
E & C
d)
A & D 
38.

Temperature is a measure of average ________ energy of individual atoms.

a)

heat

b)

potential

c)

mechanical

d)

kinetic

39.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
40.
Given the reaction at equilibrium:
N2(g) + 3H2(g) ↔ 2NH3(g)
Increasing the concentration of N2(g) will increase the foward reaction rate due to
a)
a decrease in the number of effective collisions
b)
an increase in the number of effective collisions
c)
a decrease in the activation energy
d)
an increase in the activation energy
41.
Given the reaction at equilibrium:
N2(g) + O2(g) ↔ 2NO(g)
As the concentration of N2(g) increases, the concentration of O2(g) will
a)
decrease
b)
increase
c)
remain the same
42.
Given the reaction system in a closed container at equilibrium and at a temperature of 298 K:
N2O4 (g)  <-->  2NO2 (g)
The measurable quantities of the gases at equilibrium must be
a)
decreasing
b)
increasing
c)
equal
d)
constant
43.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
44.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
45.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
46.
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
47.
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
48.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
49.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
50.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
51.

H2(g)+Cl2(g)⇌2HCl(g)

The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?

a)

equilibrium shifts right

b)

equilibrium shifts left

c)

You cannot predict the effect

d)

no change

52.

H2(g)+Cl2(g)⇌2HCl(g)

Increasing the pressure will

a)

shift equilibrium right

b)

shift equilibrium left

c)

You cannot predict the effect

d)

have no change

53.

H2(g)+Cl2(g)⇌2HCl(g)

Removing Cl2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

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