wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

REACTION KINETICS - CHEMICAL EQUILIBRIUM - ELECTROCHEMISTRY

Total questions: 118

Worksheet time: 2hrs 32mins

Name
Class
Date
1.
Which statement correctly describes the 2 electrodes?
a)
The anode is negative and the cathode is positive
b)
The anode and cathode are both positive
c)
The anode is positive and the cathode is negative
d)
The anode and cathode are both negative.
2.
It is essetial that the electrolyte is a liquid so that...
a)
Charged ions can migrate towards the electrodes. 
b)
Charged ions can migrate towards the electrodes.
c)
The solution can move around.
d)
The current can flow through it.
3.
Positive ions (cations) will move towards the cathode (-) where they will discharge by....
a)
Breaking apart
b)
Losing electrons
c)
Clumping together.
d)
Gaining electrons
4.
When NaCl solution is electrolysed what has forms at the anode?
a)
Hydrogen
b)
Oxygen
c)
Chlorine
d)
Sodium
5.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

a)

Bromine atoms in lead(II) bromide are converted to ions when it is melted

b)

Electrons flow through the lead(II) bromide when it is melted

c)

The ions in lead(II) bromide are mobile charge carriers in the molten state.

d)

There are no ions in solid lead(II) bromide

6.
What is the product formed at the anode during the electrolysis of concentrated copper(II) chloride?
a)
copper
b)
chlorine
c)
hydrogen
d)
oxygen
7.

What is the half-equation for the discharge of hydroxide ions?

a)

2O2- --> O2 + 4e-

b)

OH- --> OH + e

c)

4OH- --> 2H2O + O2 + 4e-

d)

2H2O + O2 + 4e- --> 4OH-

8.

The picture shows electrolysis of copper(II) sulphate solution using graphite electrodes. Besides formation of brown solid on the cathode, what other observations can be made?

a)

The mass of graphite anode decreases.

b)

The blue colour solution becomes paler.

c)

Bubbles of gas form at the anode.

d)

The blue colour solution becomes darker.

9.
What is the product formed at the cathode during the electrolysis of molten magnesium fluoride?
a)
magnesium
b)
hydrogen
c)
fluorine
d)
oxygen
10.

What are the products at the electrodes when dilute sulfuric acid is electrolysed using inert electrodes?

a)

A

b)

B

c)

C

d)

D

11.

The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous

sodium chloride using carbon electrodes.

At which electrode(s) is hydrogen produced?

a)

electrode 1 only

b)

electrodes 1 and 3

c)

electrode 2 only

d)

electrodes 2 and 4

12.

Polls of Graphite or Platinum through which an electric current enters the electrolyte are collectively called what ?

a)

Electrodes

b)

Anode

c)

Cathode

d)

Cation

13.

In electrolysis, Oxidation occurs in which of the following electrodes?

a)

Cathode

b)

Anode

c)

Both cathode and Anode

d)

Non of the above

14.

In electrolysis, reduction takes place in which of the following electrodes?

a)

Cathode

b)

Anode

c)

Both cathode and anode

d)

Non of the above

15.
In an aqueous solution of copper chloride, which ions are attracted to the negative electrode?
a)
Cu2+ and Cl- and H+ and OH-
b)
Cu2+ and H+ 
c)
 Cl- and OH-
d)
Cu2+ 
16.
a)

A

b)

B

c)

C

d)

D

17.
a)

A

b)

B

c)

C

d)

D

18.

The diagram shows the electrolysis of dilute sulfuric acid.


Which substance is produced at the negative electrode?

a)

hydrogen

b)

oxygen

c)

sulfur dioxide

d)

water

19.

What are the ions present in molten Al2O3?

a)

Al2+ and O3-

b)

Al2- and O3+

c)

Al3+ and O2-

d)

Al3- and O2+

20.

The diagram shows apparatus for plating a spoon with silver.

Which statement is not correct?

a)

Silver would stick to the spoon because it is a very reactive metal.

b)

The electrolyte would be a silver salt dissolved in water.

c)

The metal electrode would be made from silver..

d)

The spoon would be connected to the negative terminal of the power supply.

21.

The diagram shows the electroplating of a steel object.

A student made the following statements.

1 The object turns a reddish-brown colour.

2 The copper sulfate solution changes to a paler blue colour.

3 The copper electrode becomes smaller.

Which statements are correct?

a)

1, 2 and 3

b)

1 and 2 only

c)

1 and 3 only

d)

2 and 3 only

22.

Sodium chloride solution is electrolysed and a gas is collected at each electrode. One gas decolourises moist litmus paper, the other gas burns with a pop.


Which statement is correct?

a)

Chlorine gas is collected at the anode.

b)

Hydrogen gas is collected at the anode.

c)

Oxygen gas is collected at the cathode.

d)

The cathode is the positive electrode.

23.
Object is electroplated with copper using copper(II) sulfate. Which statement is correct?
a)
Positive electrode increases in mass
b)
Concentration of Cu2+ ions in solution decreases
c)
Reduction occurs at positive electrode
d)
Reaction at negative electrode is Cu2+ + 2e– → Cu
24.
Name product C
a)
hydrogen
b)
chlorine
c)
water
d)
sodium hydroxide
25.
Electrolysis is .....
a)
conduction of electricity by the ionic compound in solid state
b)
conduction of electricity by ionic compound in molten and aqueous state
26.

CO32- and OH- are attracted to the positive electrode (anode). What gas forms?

a)

OH-

b)

CO2

c)

O2

d)

H2

27.

PO42- and OH- are attracted to the positive electrode (anode). What gas forms?

a)

OH-

b)

PO42-

c)

O2

d)

H2

28.

If the fork is to be electroplated with silver metal, what electrolyte should be used?

a)

Molten silver chloride

b)

Aqueous silver nitrate

c)

Sodium chloride solution

d)

Copper(II) sulphate solution

29.

Which is not a reason that cryolite is used in aluminum extraction?

a)

Cryolite dissolves aluminum oxide

b)

Cryolite reduces the melting point of aluminum oxide

c)

Cryolite decreases the cost of aluminum extraction

d)

Cryolite removes impurities from aluminum oxide

30.

Which of the following solutions would produce hydrogen gas at the cathode upon electrolysis?

1 Dilute nitric acid

2 Aqueous potassium hydroxide

3 Aqueous sodium chloride

a)

1 only

b)

1 and 2

c)

2 and 3

d)

All of the above

31.

The electrolytic deposition of a superior metal on a baser metal is:

a)

electro-refining

b)

electro-plating

c)

electro-metallurgy

d)

electrolysis

32.

An electric current of 1.04A was passed through a solution of dilute sulphuric acid for 6 minutes. The volume of hydrogen produced at r.t.p. was 43.5 cm3. How many coulombs of charge were passed during the experiment?

a)

6.24C

b)

374.4C

c)

373.4C

d)

324.4C

33.

An electric current of 1.04A was passed through a solution of dilute sulphuric acid for 6 minutes. The volume of hydrogen produced at r.t.p. was 43.5 cm3. How many coulombs of charge are required to liberate 1 mol of H2(g)? (F = 96500C mol-1)

a)

96500C

b)

19300C

c)

193000C

d)

289500C

34.

A student conducted an experiment to calculate a value for the Faraday constant, F. An electric current of 0.3A was passed through the solution of copper (II) sulphate for exactly 40 minutes. 0.240g of copper was deposited at cathode. Use this information to calculate a value of F. (Ar of Cu is 63.5)

a)

96500C

b)

95250C

c)

95350C

d)

96400C

35.

Which statement is correct on electrolysis of aqueous copper (II) sulphate using graphite electrodes?

a)

Colourless gas is produced at negative electrode

b)

Electrolyte does not change colour

c)

Negative electrode decreases in mass

d)

Colourless gas is produced at positive electrode

36.
Object is electroplated with copper using copper(II) sulfate. Which statement is correct?
a)
Positive electrode increases in mass
b)
Concentration of Cu2+ ions in solution decreases
c)
Reduction occurs at positive electrode
d)
Reaction at negative electrode is Cu2+ + 2e– → Cu
37.

Which apparatus could be used to electroplate an iron nail with copper?

a)

A

b)

B

c)

C

d)

D

38.

What is the Equation for Charge Flow?

a)

Charge Flow = Current x Time (Q=It)

b)

Charge Flow = Current / Time (Q=I/t)

c)

Charge Flow = Time / Current (Q=t/I)

39.

A current of 5.0 A flows for 4 hours through an aqueous solution of copper sulphate (VI). Calculate the mass of copper deposited at the cathode.

a)

21.69 g

b)

22.69 g

c)

23.69 g

40.

When a certain amount of electric charge flows through an aqueous solution of silver nitrate, 3.24 g of silver is deposited on the cathode.

Calculate the mass of aluminium, Al that will be deposited by the same quantity of charge.

a)

0.27 g

b)

0.29 g

c)

0.40 g

41.

How do you complete the circuit when using 2 half-cells?

a)

acid bridge

b)

base bridge

c)

salt bridge

42.

Different pairs of metals produce different voltages.

a)

True

b)

False

43.
Which of the following is not a similarity between voltaic and electrolytic cells?
a)
electrons flow from anode to cathode
b)
reduction occurs at cathode
c)
oxidation occurs at anode
d)
charges on anode and cathode are the same
44.
If the cell potential is negative, the reaction is?
a)
 a success
b)
spontaneous
c)
not spontaneous
45.

The E0 value for all electrolysis reactions is

a)

positive

b)

neutral

c)

negative

46.

The E0 value for all electrochemical cell reactions is

a)

positive

b)

neutral

c)

negative

47.

Which is not a reason for metal plating?

a)

decorative purposes

b)

prevent rust and corrosion

c)

to make the metal stronger

d)

all of the above

48.
Metal A is more reactive than metal B. Which statement is correct?
a)
Electrons flow in the external circuit from A to B
b)
Positive ions flow through salt bridge from A to B
c)
Positive ions flow in external circuit from B to A.
d)
Electrons flow through salt bridge from B to A
49.
This electrode in a voltaic cell gains mass
a)
anode
b)
cathode
50.

Diagram shows an electrolysis cell.

Which of the substances cause the bulb to light up when electricity passes through it?

a)

Ethanol

b)

Dilute ethanoic acid

c)

Solid lead(II) bromide

d)

Tetrachloromethane

51.

Chemical cells convert

a)

mechanical energy in to electrical energy

b)

potential energy in to electrical energy

c)

electrical energy in to chemical energy

d)

chemical energy in to electrical energy

52.

State one functions of salt bridge

a)

to maintain the movement of electron

b)

to allowing electron to flow and complete the circuit

c)

to separate two electrolyte

d)

to allowing movement of ion to complete the circuit

53.

What is the name of the positive terminal in an electrolytic cell?

a)

cathode

b)

anode

54.
Below shows a cell diagram for voltaic cell. Which of the following is FALSE?
a)
Electrons flow from anode to cathode
b)
Oxidation happens in anode
c)
Copper undergo reduction to form copper ions
d)
Zinc undergo oxidation to form Zinc ions
55.

The overall reaction in an electrochemical cell is

Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)

As the reaction in this cell takes place, the

a)

mass of the Zn electrode decreases

b)

Zn2+concentration remains the same

c)

mass of the Cu electrode decreases

d)

Cu2+ concentration remains the same

56.
What reaction occurs at the anode?
a)
Ag+ + e- →Ag
b)
Ag → Ag+ + e-
c)
Ni2+ + 2e- → Ni
d)
Ni → Ni2+ + 2e-
57.

The anode is where oxidation occurs in...

a)

A Galvanic Cell/ voltaic

b)

A Electrolytic Cell

c)

Both Galvanic and Electrolytic cells

58.

In a Galvanic Cell, the anode is...

a)

positive

b)

negative

59.

In a Galvanic Cell, the cathode is...

a)

positive

b)

negative

60.

In a Galvanic cell, the electrons flow from the...

a)

anode to the cathode

b)

cathode to the anode

61.

Ecell =

a)

Ered - Eox

b)

Ered + Eox

c)

Eox - Ered

d)

Eox + Ered

62.

In a Galvanic Cell, the salt bridge...

a)

completes the circuit so that electrons can flow through the wire

b)

maintains charge balance

c)

is soaked in an unreactive electrolyte such as KNO3

d)

all of the above

63.

Consider the galvanic cell reaction Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq) When the cell is running spontaneously, which is the only true statement?

a)

The copper electrode loses mass and the zinc electrode is the cathode.

b)

The copper electrode gains mass and the copper electrode is the cathode.

c)

The zinc electrode gains mass and the zinc electrode is the anode.

d)

The zinc electrode loses mass and the zinc electrode is the cathode.

64.

WHICH IS ANODE?

a)

COPPER ELECTRODE

b)

ZINC ELECTRODE

c)

ZINC SULFATE SOLUTION

d)

SALT BRIDGE

65.

If an electrochemical reaction is spontaneous, what will Ecell be?

a)

positive

b)

negative

66.
Calculate the cell potential of voltaic cell
a)
–1.51
b)
- 0.03
c)
+0.03
d)
+1.51
67.
Voltaic cell is made by connecting two half-cells below. Which statement is correct?
a)
Mn is oxidized and voltage is 1.06 V
b)
Pb is oxidized and voltage is 1.06 V
c)
Mn is oxidized and voltage is 1.32 V
d)
Pb is oxidized and voltage is 1.32 V
68.

Which electrode will increase in size as the spontaneous reaction takes place?

a)

anode

b)

cathode

69.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
70.

What is the equilibrium-constant expression for

CO2(g) + H2(g) ⇌ CO(g) + H2O(l)

a)

Kc= [CO][H2O] / [CO2][H2]

b)

Kc= [CO2][H2] / [CO]

c)

Kc= [CO2][H2] / [CO][H2O]

d)

Kc= [CO] / [CO2][H2]

71.

Le Chatelier's Principle states that "If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium __________"

a)

shifts to increase the change

b)

shifts to counteract the change

c)
does not change
72.

The following reaction :     SO2 (g) +  NO2 (g) ⇌ SO3 (g) + NO (g)   had reached a state of equilibrium, was found to contain   0.40 mol L-1 SO3 , and 0.30 mol L-1 NO, 0.15 mol L-1NO2 , and 0.20 mol L-1 SO2. Calculate the equilibrium constant for this reaction. 

a)
4
b)
.42
c)
.25
d)
1
73.

What is the equilibrium expression for: Fe3O4(s) + 4H2(g) ⇌ 3Fe(s) + 4H2O(g) Kc =

a)
[Fe]3 [H2O]4  / [Fe3O4] [H2]4
b)
[Fe3O4] [H2]4 /  [Fe]3 [H2O]4
c)
[H2O]4 / [H2]4
d)
[Fe] [H2O] / [Fe3O4] [H2]
74.

Around what time does the reaction reach equilibrium?

a)

25 min

b)

70 min

c)

45 min

d)

80 min

75.

A mixture of gases is allowed to reach equilibrium at 700oC in a 12.0 L flask. At equilibrium, the

mixture contains 0.208 M SO2, 1.12×10-6 M O2 and 0.725 M SO3.

2SO2(g) + O2(g) ⇌ 2SO3 (g)

What is the equilibrium constant, Kc?

a)

9.22 x 10-8

b)

3.11 x 106

c)

1.08 x 107

d)

4.56 x 108

76.

The reaction of carbon and carbon dioxide reached equilibrium according to the equation,

C(s) + CO2(g) ⇌ 2CO (g)

Kc = 0.122 at 1100 K

What is the value of Kp for this reaction?

a)

0.035 atm

b)

0.12 atm

c)

11 atm

d)

945 atm

77.

Which is the correct statement for a chemical equilibrium?

a)

The rate of the forward reaction is the same as that of the reverse reaction.

b)

The total concentration of product equals that of reactants.

c)

The rate constant of forward reaction equals that of the reverse reaction.

d)

The product of equilibrium concentration of products and reactants equals to the Kc value.

78.

In which the of the following equilibrium systems will the product concentration increase by using

higher pressure?

a)

N2O4(g) ⇌ 2NO2(g)

b)

O2(g) + C(s) ⇌ 2CO(g)

c)

SbCl5(g) ⇌ SbCl3(g) + Cl2(g)

d)

2SO2(g) + O2(g) ⇌ 2SO3(g)

79.

At 2000K, the equilibrium constant KC for the reaction

N2 (g) + O2 (g) ⇌ 2NO (g)

is 4.0 x 10-4. Determine the concentration of NO at equilibrium if given the concentration of N2 and O2

at equilibrium is 0.25M and 0.33M, respectively.

a)

1.7 x 10-5 M

b)

5.7 X 10-3 M

c)

3.3 X 10-5 M

d)

6.8 X 10-3 M

80.

Which equilibrium is NOT affected by the change of total pressure of the system?

a)

NH4Cl(s) ⇌ NH3(g) + HCl(g)

b)

PCl5(g) ⇌ PCl3(g) + Cl (g)

c)

6H2O(l)+ 6CO2(g) ⇌ C6H12O6(s) + 6O2 (g)

d)

2PbS (s) + 3O2 (g) ⇌ 2PbO(s) + 2SO2 (g)

81.

The endothermic reaction

2NO(g) + Br2(g) ⇌ 2NOBr(g)

Has an equilibrium constant, KP= 116.6 at 25oC

Which of the statement below is NOT true?

a)

the equilibrium constant KP for reverse reaction is 8.58 x 10-3

b)

removing Br2 from the reaction vessel decrease the KP value

c)

the equilibrium constant KC is 116.6 RT

d)

KP increase as temperature increased

82.

The equilibrium constant KC for the reaction

N2O4(g) ⇌ 2NO2(g)

is 0.212 at 100 oC. what is the value of KP?

a)

14.28

b)

1.74

c)

198.62

d)

6.49

83.

Consider the following reaction:

2NaHCO3(s) ⇌ Na2CO3(s) + CO2(g) + H2O(g) ; Kp = 0.23

A sample of NaHCO3 is placed in an evacuated flask and is allowed to achieve equilibrium at 373 K.

What is the total gas pressure at equilibrium?

a)

0.12 atm

b)

0.24 atm

c)

0.48 atm

d)

0.96 atm

84.

Hydrogen and carbon dioxide react according to the equation.

H2(g) + CO2(g) ⇌ CO(g) + H2O(g)

When 4.0 mol of hydrogen and 0.9 mol of carbon dioxide were used for this reaction, 0.1 mol of CO2 was found in the equilibrium mixture. Calculate Kc for the reaction.

a)

0.4

b)

0.8

c)

2.0

d)

2.4

85.

The equilibrium constant, Kp, for the reaction,

N2(g) + O2(g) ⇌ 2NO(g)

is 1.3×10-15 at 298 K and 5.5×10-2 at 2000 K. This means that

a)

the forward reaction is exothermic.

b)

more product is formed as temperature is increased.

c)

the value of Kp depends on the amount of nitrogen used.

d)

the value of Kp increases as the pressure exerted on the system increases

86.

Calculate Kc for the reaction at 827 K when KP = 1.78 x 103 atm,

2CO2(g) ⇌ 2CO(g) + O2(g)

a)

1.22 x 107

b)

1.21 x 105

c)

2.62 x 101

d)

2.59 x 10-1

87.

Which of the following statements is/are true regarding the following equilibrium?

N2(g) + 3Cl2(g) ⇌ 2NCl3(g) Kp = 1.12×102 at T K


Tick 1 (or more) CORRECT answer(s)

a)

The Kp value for the reverse reaction is 8.93 ×10-3.

b)

The forward and reverse reaction rates are the same.

c)

The equilibrium shifts to the right when more NCl3 is added.

88.

In the Haber process, the equilibrium between H2, N2 and NH3 is shown;

N2(g) +3H2(g) ⇌ 2NH3(g) ; ΔH= -ve

What are the ideal conditions needed to obtain the maximum yield of NH3?

a)

low pressure, low temperature

b)

low pressure, high temperature

c)

high pressure, low temperature

d)

high pressure, high temperature

89.

After the adding the C, the system that has achieved an equilibrium is

3C(s) + 3H2(g) ⇌ CH4(g) + C2H2(g)

a)

shift to the right

b)

the volume of the container is decreased

c)

no further changes occur

d)

Kc decreases

90.
Find the Kc for
2NOBr(g) + Cl2(g) ↔ 2NO(g) + 2BrCl(g)
 if 
2NOBr(g) ↔ 2NO(g) + Br2(g)
has a Kc = 0.014
Br2(g) + Cl2(g) ↔ 2BrCl(g)
has a Kc = 7.2
a)
0.10
b)
10
c)
1.0 x 10-3
d)
1.0 x 10-2
91.

For the following reaction:

H2(g) + Cl2 (g) ↔ 2HCl(g),

calculate the concentration of HCl when KC= 2.3x10-5, [H2]= 0.0056mol, [Cl2]= 0.0048mol.

a)

6.2 x 10-10 M

b)

2.5 x 10-5 M

c)

1.1 M

d)

1.2 M

92.
Which picture shows how a catalyst would change the rate? 
a)
Option 3
b)
Option 2
c)
Option 1
93.

What letter represents the activation energy?

a)

A

b)

B

c)

C

d)

D

94.

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

a)

A

b)

B

c)

C

d)

D

95.

Which of the following represent the rate of reaction as
A  →\rightarrow  Product ?

a)

rate = Δ[A]Δtrate\ =\ \frac{\Delta\left[A\right]}{\Delta t}  

b)

rate = −Δ[A]Δtrate\ =\ -\frac{\Delta\left[A\right]}{\Delta t}  

c)

rate = Δ tΔ[A]rate\ =\ \frac{\Delta\ t}{\Delta\left[A\right]}  

d)

rate = −Δ tΔ[A]rate\ =\ -\frac{\Delta\ t}{\Delta\left[A\right]}  

96.

What two trials would you use to find the order for B?

a)

trials 1 and 2

b)

trials 1 and 3

c)

trails 2 and 3

97.

The first order rate constant for the decomposition of 0.5 M compound A at 100oC is 0.03 min-1. Calculate the half-life of A.

a)

1.5 min

b)

8.3 min

c)

23.1 min

d)

66.7 min

98.

What is the unit for rate constant,K if rate law:

Rate = K [A]2

a)

s-1

b)

M s-1

c)

M-1 s-1

d)

M-2 s-1

99.

The rate expression for the reaction

X(g) + 2Y(g) → 3Z(g) is

rate = k [Y]2

By which factor will the rate of reaction increase when the concentrations of X and Y are both increased by a factor of 3?

a)

6

b)

9

c)

18

d)

27

100.

A --> product

The rate constant for above reaction is 0.5 s-1 . If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

a)

0.7 s

b)

1.4 s

c)

2.8 s

d)

There is not enough information given.

101.

The reaction A + 2B → products was found to have the rate law, k = k[A][B]2. Predict by what factor the rate of reaction will increase when the concentration of B is doubled and the concentration of A remained uncanged

a)

2

b)

4

c)

6

d)

8

102.

For second order reaction, the initial concentration of reactant A is 0.24 M. If the rate constant is 8.1 x 10-2 M-1 s-1, what is the concentration of A after 29 seconds?

a)

0.02 M

b)

0.15 M

c)

0.30 M

d)

0.45 M

103.
Determine the order of reaction with respect to concentration of A
a)
zero
b)
1st
c)
2nd
d)
3rd
104.
Consider the following rate law: Rate = k[A]n[B]m
How are the exponents n and m determined?
a)
by using balanced chemical equation
b)
By using the subscripts for the formulas
c)
By educated guess
d)
By experiment 
105.
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]
106.

For the reaction below, which of the following is the correct differential rate equation?


NH3(g) + O2(g) → NO(g) + H2O(g)

a)

rate = −d[NH3]dt=−d[O2]dt=d[NO]dt=d[H2O]dtrate\ =\ -\frac{\text{d}\left[NH_3\right]}{\text{d}t}=-\frac{\text{d}\left[O_2\right]}{\text{d}t}=\frac{\text{d}\left[NO\right]}{\text{d}t}=\frac{\text{d}\left[H_2O\right]}{\text{d}t}

b)

rate = −12d[NH3]dt=−13d[O2]dt=14d[NO]dt=12d[H2O]dtrate\ =\ -\frac{1}{2}\frac{\text{d}\left[NH_3\right]}{\text{d}t}=-\frac{1}{3}\frac{\text{d}\left[O_2\right]}{\text{d}t}=\frac{1}{4}\frac{\text{d}\left[NO\right]}{\text{d}t}=\frac{1}{2}\frac{\text{d}\left[H_2O\right]}{\text{d}t}

c)

rate = d[NH3]dt=d[O2]dt=−d[NO]dt=−d[H2O]dtrate\ =\ \frac{\text{d}\left[NH_3\right]}{\text{d}t}=\frac{\text{d}\left[O_2\right]}{\text{d}t}=-\frac{\text{d}\left[NO\right]}{\text{d}t}=-\frac{\text{d}\left[H_2O\right]}{\text{d}t}

d)

rate = −14d[NH3]dt=−15d[O2]dt=14d[NO]dt=16d[H2O]dtrate\ =\ -\frac{1}{4}\frac{\text{d}\left[NH_3\right]}{\text{d}t}=-\frac{1}{5}\frac{\text{d}\left[O_2\right]}{\text{d}t}=\frac{1}{4}\frac{\text{d}\left[NO\right]}{\text{d}t}=\frac{1}{6}\frac{\text{d}\left[H_2O\right]}{\text{d}t}

107.

Which of the following is a unit of rate of reaction?

a)

s-1

b)

Ms-1

c)

M

d)

M-1s-1

108.

Determine the overall order of the reaction:


rate = k[A][B]0[D]

a)

First order

b)

Zero order

c)

Second order

d)

Third order

109.

Determine the rate of formation of CO2 if the rate of deflation of O2 gas is 0.15 Ms-1.

a)

0.15 Ms-1

b)

0.30 Ms-1

c)

0.10 Ms-1

d)

0.225 Ms-1

110.

One of the most common and important classes of catalysts are in living things, and are called ___

a)

synovial fluids

b)

amino acids

c)

hormones

d)

enzymes

111.

In the nitric oxide reaction, doubling the hydrogen doubled the rate so the reaction is ___

a)

first order, with respect to hydrogen

b)

first order, overall

c)

second order, with respect to hydrogen

d)

second order, overall

112.

The rate law describes the relationship between the initial concentrations of the reactants and ___

a)

the final concentration of products

b)

the rate at which they react

c)

their kinetic energy

d)

the equilibrium constant

113.

what is the order of reaction if

k= 2.3 X 10 -5 lit mol-1 sec-1

a)

3

b)

2

c)

1

d)

0

114.

Consider the Arrhenius equation given below and mark the correct option :

k=Ae−Ea​/RT.

a)

b)

c)

d)

115.

Given the hypothetical reaction A + B --> AB, ΔH = -50 kJ

If the activation energy for the forward reaction is 75 kJ, the activation energy for the reverse reaction is

a)

90 kJ

b)

-75 kJ

c)

25 kJ

d)

125 kJ

116.

State the equation shown in diagram below

a)

Activation energy

b)

Arrhenius equation

c)

Rate equation

d)

Arrhenius Constant

117.

Consider the reaction and its rate law given below.

2 A (g) + B(g) --> 2 C(g)

Rate = k[A][B]

At the beginning of one trial of this reaction, [A] = 3.0 M and [B] = 1.0 M. The observed rate for the formation of C is 0.36 mol L-1 s-1.

The numerical value of k, the rate constant is closest to

a)

0.040

b)

0.12

c)

108

d)

6.0

118.
The following data were measured for the reaction BF3(g) + NH3(g) —> F3BNH3(g)
What is the rate law for the reaction? 
a)
R=K[NH3]
b)
R=K[BF3]2[NH3]
c)
R=K[BF3][NH3]
d)
R=K[BF3][NH3]2

Similar Resources on Wayground

Periodic Table of the Elements Symbols

118 questions

Periodic Table of the Elements Symbols

quiz

Worksheet

•

7th Grade - University

Balancing Chemical Equations

120 questions

Balancing Chemical Equations

quiz

Worksheet

•

10th - 12th Grade

CH05 Periodic Trends

116 questions

CH05 Periodic Trends

quiz

Worksheet

•

10th - 11th Grade

Chemistry Final Review

117 questions

Chemistry Final Review

quiz

Worksheet

•

10th - 12th Grade

Test #1 Review

113 questions

Test #1 Review

quiz

Worksheet

•

10th - 12th Grade

Exam I: CHMY 141 Spring 2020

119 questions

Exam I: CHMY 141 Spring 2020

quiz

Worksheet

•

10th Grade - University

Mock Milestones Atoms

120 questions

Mock Milestones Atoms

quiz

Worksheet

•

7th - 12th Grade

The ENTIRE Periodic Table of Elements + Their Atomic Symbols

118 questions

The ENTIRE Periodic Table of Elements + Their Atomic Symbols

quiz

Worksheet

•

10th Grade - University