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J FORTUNE TUTORIAL CHEM 101 MOCK TEST 150 standard questions

Total questions: 150

Worksheet time: 5hrs 12mins

Name
Class
Date
1.

rate = k[A]

The rate constant in the rate law above is 0.5 L/mol·s. 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.

2.

Given the following rate law,

rate = k[A]2[B]

if [A] were doubled, what must happen to [B] to keep the rate constant?

a)

[B] must quadruple

b)

[B] must double

c)

[B] must be havled

d)

[B] must be quartered

3.

Consider this reaction:

2SO2(g) + O2(g) →\rightarrow   2SO3(g)

The rate of disappearance of SO2 is 1.6 gL-1 min-1. What is the rate of formation of SO3 in molL-1min-1? [Molar mass SO2: 64.0 gmol-1]

a)

0.035

b)

0.025

c)

0.120

d)

0.050

4.

The rate constant is doubles on the increasing temperature from 310K to 350K. What is the activation energy (in kJ mol-1) for this reaction?

a)

12.3

b)

15.6

c)

25.8

d)

29.2

5.

rate = k[A]

The rate constant in the rate law above is 0.5 1/s. 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.

6.
The reaction
2ClO2(aq) + 2OH-(aq) —> ClO3(aq) + ClO2-(aq) + H2O(l) was studied with the following results: 
Calculate the rate constant with proper units. 
a)
230 M/S
b)
230 M-S-
c)
230 M2-S-
d)
R=K[ClO2][OH-]
7.

A → products

The reactant A in the equation above was found to be first order. Which of the following integrated rate laws would correspond to this reaction?

a)

1/[A] = kt + 1/[A]o

b)

ln[A] = -kt + ln[A]o

c)

[A] = -kt + [A]o

8.
The molar solubility of PbI2 is 1.52 x 10-3 M. Calculate the value of Ksp for PbI2.
a)
3.51 x 10-9
b)
1.40 x 10-8
c)
4.62 x 10-6
d)
1.52 x 10-3
9.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
10.
Silver chromate, Ag2CrO4, has a Ksp of 8.96 x 10-12. Calculate the solubility in mol/L of silver chromate.
a)
1.31 x 10-4M
b)
1.65 x 10-4M
c)
2.25 x 10-12M
d)
2.08 x 10-4M
11.

The Ksp value for PbF2 is 4 x 10-8. Calculate the molar solubility of solid PbF2 in a 0.5M NaF solution.

a)

8 x 108

b)

1.6 x 107

c)

8 x 10-8

d)

1.6 x 10-7

12.
If a 8.50g ice cube at -10o C sits out on the counter, completely melts, and then warms to room temperature (25o C) how much energy did the ice cube absorb? Use C = 2.108 J/goC for ice, C = 4.184 J/goC for water, and Hf = 334 J/g.
a)
179.18 J
b)
2839 J
c)
889.1 J
d)
3907.3 J
13.

Oxygen gas is at a temperature of 40oC when it occupies a volume of 2.3 liters. To what temperature should it be raised to occupy a volume of 6.5 liters?

a)

611.84oC

b)

611.84 K

c)

880.33 K

d)

880.33oC

14.

The standard enthalpy of formation of NH3 is – 46 kJ mol–1. If the enthalpy of formation of H2 from its atoms is – 436 kJ mol–1 and that of N2 is –712 kJ mol–1, the average bond enthalpy of N—H bond in NH3 is

a)

– 1102 kJ mol–1

b)

– 964 kJ mol–1

c)

+ 352 kJ mol–1

d)

+ 1056 kJ mol–1

15.

For a reaction, A(g) → A(l); ∆H = –3RT. The correct statement for the reaction is

a)

|∆H| < |∆U|

b)

∆H = ∆U≠ 0

c)

|∆H| > |∆U|

d)

∆H = ∆U = 0

16.

6. The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?

a)

-85.6 kJ, spontaneous

b)

-18.3 kJ, not spontaneous

c)

+18.3 kJ, spontaneous

d)

+85.6 kJ, not spontaneous

17.

1. Given the following information, calculate ΔG0 for the reaction below at 250C: (K = 0C + 273)

SnCl4(l) + 2 H20(l) → SnO2(S) + 4HCl(g),

ΔH0=133.0 kJ and ΔS0 =401.5 J/K

a)

-252.6 kJ

b)

-13.4 kJ

c)

13.4 kJ

d)

252.6 kJ

18.

A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if ΔH is __________ and ΔS is __________.

a)

+, +

b)

-, -

c)

+, -

d)

-, +

e)

+, 0

19.

In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2 (g) + 3H2 (g) ->2NH3 (g)

∆G at 298 K for this reaction is -33.3 kJ/mol.

The value of ∆G at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is

a)

3.86 x103

b)

-1.8

c)

-40.5

d)

-7.25 x103

e)

-104.5

20.

The average bond enthalpies for O-O and O=O are 146 and 496 kJ/mol respectively. What is the enthalpy change, in kJ, for the reaction below?

H2O2(g) → H2O(g) + ½O2(g)

a)

-102

b)

+102

c)

+350

d)

+394

21.

Which of these would ALWAYS give a spontaneous process?

a)

ΔH is + ΔS is +\Delta H\ is\ +\ \Delta S\ is\ +  

b)

ΔH is − ΔS is −\Delta H\ is\ -\ \Delta S\ is\ -  

c)

ΔH is + ΔS is −\Delta H\ is\ +\ \Delta S\ is\ -  

d)

ΔH is − ΔS is +\Delta H\ is\ -\ \Delta S\ is\ +  

22.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

23.

Calculate the standard enthalpy change for the combustion of methane (CH4) given the following data: C(s) + 2H2(g) -> CH4(g) ΔH = -74.8 kJ/mol, O2(g) -> 2O(g) ΔH = 495 kJ/mol, CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) ΔH = -890.3 kJ/mol.

a)

-74.8 + 495 + (-890.3) = -469.1 kJ/mol

b)

-74.8 - 495 - 890.3 = -1460.1 kJ/mol

c)

-74.8 + 495 + 890.3 = 1311.5 kJ/mol

d)

-74.8 + 495 - 890.3 = -469.1 kJ/mol

24.

At what temperature would a given reaction become spontaneous if ΔH =+119kJ and ΔS=+263J/K.mol

a)

452 K

b)

2210 K

c)

382 K

d)

363 K

25.
How many particles are in 13.5 grams of Beryllium?
a)
1.5 particles
b)
9 particles
c)
4x1023 particles
d)
9x1023 particles
26.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
27.

For the reaction represented by the equation Pb(NO3)2+2KI → PbI2+2KNO3Pb\left(NO_3\right)_2+2KI\ \rightarrow\ PbI_2+2KNO_3  how many moles of lead iodide (PbI2)\left(PbI_2\right) are produced of 300 grams potassium iodide (KI)\left(KI\right)  when Pb(NO3)2Pb\left(NO_3\right)_2  is in excess?

a)

114.78 mol PbI2

b)

0.904 grams PbI2

c)

0.904 mol PbI2

d)

114.78 grams PbI2

28.

Lighting a match is an example of

a)

an endothermic reaction

b)

an endergonic reaction

c)

both an endothermic and an endergonic reaction

d)

both an exothermic and an exergonic reaction

29.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single diplacement
d)
Double displacement
30.

What colour is copper(II)carbonate

a)

white

b)

blue

c)

colourless

d)

green

31.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
32.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
33.
Find the percentage composition of  Mg in Mg3(PO4)2.
   

a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
34.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
35.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
36.
The relative atomic mass is the average mass of an atom compared to 
a)
the mass of a carbon-12 atom.
b)
1/12 the mass of a carbon-12 atom
c)
the mass of a hydrogen atom
d)
1/12 the mass of a hydrogen atom
37.

You begin with a solution of 400 grams of potassium chloride dissolved in 1250 mL of water. If the volume of water is increased by 33%, what is the final molarity of the solution?

a)

3.2 M

b)

4.3 M

c)

5400 M

d)

5.4 M

38.

How can the equilibrium constant (K) be used to predict the direction of a reaction?

a)

If K is greater than 1, the reaction will proceed to the right (towards products)

b)

If K is greater than 1, the reaction will proceed to the left (towards reactants)

c)

If K is less than 1, the reaction will proceed to the right (towards products)

d)

If K is less than 1, the reaction will proceed to the left (towards reactants)

39.
Which energy conversion shown below takes place in an electrochemical cell?
a)
Electrical to chemical
b)
Mechanical to chemical
c)
Mechanical to electrical
d)
Chemical to electrical
40.

As steady current of 10 amperes is passed through an aluminum-production cell for 15 minutes. Which of the following is the correct expressions for calculating the number of grams of aluminum produced? (1 faraday = 96,500 coulombs)

a)
b)
c)
d)
e)
41.

In the electroplating of nickel, 0.200 faraday of electrical charge is passed through a solution of NiSO4. What mass of nickel is deposited?

a)

2.94 g

b)

5.87 g

c)

11.7 g

d)

58.7 g

e)

294 g

42.

An electric current of 1.00 ampere is passed through an aqueous solution of Ni(NO3)2. How long will it take to plate out exactly 1.00 mol of nickel metal, assuming 100 percent current efficiency? (1 Faraday = 96,500 coulombs = 6.02 x 1023 electrons)

a)

386,000 sec

b)

193,000 sec

c)

96,500 sec

d)

48,200 sec

e)

24,100 sec

43.

Which statement is true for a spontaneous redox reaction carried out at standard-state conditions?

a)

E°red is always negative.

b)

E°cell is always positive.

c)

E°ox is always positive.

d)

E°red is always positive.

44.

According to Faraday's first law, the amount of substances produced or consumed at cathode or anode electrode is directly proportional to the

a)

voltage provided

b)

concentration of electrolyte

c)

quantity of electricity passed

d)

temperature of solution

45.

Calculate the equilibrium constant for the reaction between Sn metal and Zn2+ solution.

Sn + Zn2+ ⇋ Sn2+ + Zn

Sn2+ + 2 e- → Sn (s) E° = −0.141 V

Zn2+ + 2 e- → Zn (s) E° = −0.762 V

a)

1.01 x 10^21

b)

0.08 x 10^21

c)

0.08 x 10^-21

d)

1.01 x 10^-21

46.

Calculate the potential for the half-cell below for [SO3 2-] = 0.100 M, [S2O3] = 0.500 M and the pH = 10.50.

2 SO3 2- (aq) + 3 H2O (l) + 4 e- ⇋ S2O3 2- (aq) + 6 OH- (aq)

E° = −0.566 V

a)

0.123 V

b)

0.023 V

c)

-0.090 V

d)

-0.280 V

47.

Which of the following is the SI unit of molar conductivity.

a)

S m-1 mol-1

b)

S m mol-1

c)

S m2 mol-1

d)

S m2 mol-2

48.

Bonding in electrolyte is _____ and ______ in non electrolyte

a)

Covalent & ionic

b)

Dative & covalent

c)

Dative & ionic

d)

Electrovalent & covalent

49.

During ionisation ___ and _______ exhibit krypton and xenon structure respectively

a)

Rb + and Sr+

b)

Rb+ and Cs+

c)

Te- and Br-

d)

CS+ and Ba²+

50.

The modern concept of chemical bonding are base on?

a)

Attaining noble gas structure

b)

Energetic of reactions

c)

To become ion

d)

To form a product

51.

Ionic compounds are soluble in (a)   and covalent compounds are soluble in

52.

Energy in kg/mol in ionic is

a)

>>> 1000

b)

100-900

c)

20 -50

d)

Less than 20

53.

______ I use to make pie bond ?

a)

Hybridized orbital

b)

Unhybridized orbital

c)

Both

d)

None of the above

54.

Which force is responsible for liquefaction of non polar solvent

a)

London force

b)

Ionic bonds

c)

Covalent

d)

Van da waals

55.

Using Columbs law, Arrange ( NAI, NACl, NaF,NaBr) in increasing ionic character

a)

NAI, NACl, NaF, NaBr

b)

NaF, NACl,NaBr, NaI

c)

NABr, NaCl, NaF, NaI

d)

None of the above

56.

Ammonium ion (NH4+) is an example for

a)

Covalent compound

b)

Ionic compound

c)

Coordinate compound

d)

Metallic compound

57.

Which correctly describes the molecular polarity of water?

a)

nonpolar and symmetrical

b)

nonpolar and asymmetrical

c)

polar and symmetrical

d)

polar and asymmetrical

58.

In what year did Thomson discover electron

a)
1897
b)

1886

c)

1897

d)

1997

59.

What's the charge to mass of an electron

a)

1.16 * 10^11

b)

1.17 *10^ -11

c)

1.76*10^11

d)

1.78*10^13

60.

In ______, ______ assign the atomic number

a)
1924 Mosley
b)

1824 Mosley

c)

1910 Mosley

d)

1811 Mosley

61.

Wave nature of matter can only be account for

a)

Diffraction and reflection

b)

Diffraction and refraction

c)

Diffraction and polarisation

d)

Reflection and refraction

62.

Find lamda respectively

(a)  

63.

Energy level 2 to 5 are ____,_____,_____,____ and ______ respectively

a)
Balma, paschen,brachette, pfund
b)

Balma,Lyman, pfund, brachette

c)

Balma, Lyman, brachette, pfund

d)

Lyman, brachette, pfund, balma

64.

What are the six elements that doesn't exhibit isotope

a)

Fluorine, arsenic, Phosphorus, iodine, manganese, cobalt

b)

Fluorine, boron, manganese chromium,iodine , bromine

c)

Iodine, fluorine, manganese, bromine, chromium

d)

Fluorine, arsenic, manganese, chromium, iodine, boron

65.

2P⁶

"P" stands for _____

a)

Principal quantum numbers

b)

Azimuthal QN

c)

Spin QN

d)

Magnetic QN

66.

The smallest unit of an element that maintains the properties of that element

a)

proton

b)

atomic mass unit

c)

electron

d)

atom

67.
Place the following scientists in order, from earliest to latest: A) Enest Rutherford; B) J.J. Thomsonl C) John Dalton
a)
B, C, A
b)
C, A, B
c)
A, C, B
d)
C, B, A
68.
Discovered the nucleus
a)
Democritus
b)
Robert Millikan
c)
James Chadwick
d)
Ernest Rutherford
69.

Which of the following has the atomic models in the correct Chronological order?

a)

Solid sphere, Plum pudding, Nuclear, Planetary, Quantum Mechanic/Electron Cloud

b)

Solid sphere, Plum pudding, Nuclear, Quantum Mechanic/Electron Cloud, Planetary,

c)

Plum pudding, Nuclear, Planetary, Quantum Mechanic/Electron Cloud,Solid sphere

d)

Nuclear, Planetary, Solid sphere, Quantum Mechanic/Electron Cloud,Plum pudding,

70.

Which electron filling diagram rule/principle is broken if refer to the following diagram?

a)

Aufbau Principle

b)

Pauli Exclusion Principle

c)

Hund's Rule

d)

It's Correct!

71.

Which quantum number (n, l, ml, ms) determines the shape of an orbital?

a)

n

b)

l

c)

ml

d)

ms

72.

Which quantum number (n, l, ml, ms) determines the specific orbital of an electron?

a)

n

b)

l

c)

ml

d)

ms

73.

Which type of nuclear radiation can be stopped by a sheet of paper?

a)

Alpha

b)

Beta

c)

Gamma

74.

Which type of nuclear radiation can be stopped 60 cm of aluminum or 7 cm of lead?

a)

Alpha

b)

Beta

c)

Gamma

75.

When a substance undergoes beta decay

a)

The atomic number increases by 1

b)

The atomic number decreases by 2

c)

The atomic number does not change

76.

What will the values of x and y be?

a)

x=194, y =83

b)

x=194, y =84

c)

x=194, y =85

d)

I don't know. I should probably study this stuff more before the test.

77.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
78.

In beta becay…..

a)

A neutron becomes a proton and an electron

b)

A proton becomes a neutrons and an electron

c)

A electron becomes a protons and a neutron

d)

It's just a wave

79.

Compared with β-particles and γ-rays, α-particles

a)

are the only type of radiation to carry a charge.

b)

have the greatest ionising effect.

c)

have the greatest penetrating effect.

d)

have the smallest mass.

80.

Why are some radioactive sources stored in boxes made from lead?

a)

Lead absorbs emissions from the radioactive sources.

b)

Lead decreases the half-life of radioactive sources.

c)

Lead increases the half-life of radioactive sources.

d)

Lead repels emissions from the radioactive sources.

81.

A radioactive decay can be represented as shown.


The equation is incomplete.

In this decay, the nucleus changes by

a)

absorbing a neutron.

b)

absorbing a proton.

c)

emitting an α-particle.

d)

emitting a β-particle.

82.

Name a phenomenon that shows the wave properties of electrons.

a)

Reflection

b)

Refraction

c)

Dispersion

d)

Propagation

83.
What do you call the energy required to prevent the protons in the nucleus from repelling?
a)
nuclear energy
b)
binding energy
c)
radioacitve energy
d)
electromagnetic energy
84.

Which of the following statements is/are correct

regarding the binding energy of the nucleus.

I. It is equivalent to the mass defect

II. It is the energy that holds the nucleus

together

III. It is the energy required to remove a

proton from the nucleus

a)

I only

b)

II only

c)

III only

d)

I and II only

85.

Convert 5 Ci to Bq.

(a)  

86.
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 constant
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
87.

For the reaction...

SO2 + O2 ⇌ SO3

If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.

a)

left

b)

right

c)

left and right

d)

neither left nor right

88.

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

b)

H2

c)

N2 and H2

d)

NH3

89.
2SO2(g)+O2(g)⇌2SO3(g)
Removing O2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
increase pressure
d)
have no change
90.

2SO2(g)+O2(g)⇌2SO3(g)

Adding SO3(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase K

d)

have no change

91.
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.
92.
2SO2(g)+O2(g)⇌2SO3(g)
Adding SO2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
increase rate of reaction
d)
have no change
93.

For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 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

94.

In a .4 L solution at equilibrium

CaCO3CaCO_3  3 moles
CaOCaO  .5 moles
CO2CO_2  7 moles
balanced eq  CaCO3⟷CaO+CO2CaCO_3\longleftrightarrow CaO+CO_2  
What is the Keq



(a)  

95.

BaCl2+H2SO4 ⟷ BaSO4+2HClBaCl_{2_{ }}+H_2SO_4\ \longleftrightarrow\ BaSO_4+2HCl

 In a solution .96 L solution at equilibrium

BaCl2BaCl_2   .87 mole
H2SO4H_2SO_4  .1 mole

BaSO4BaSO_4   .5 mole

HClHCl   .5 mole
what is the Keq



(a)  

96.

The following reaction aA + bB produce cC + dD.

The realtion that determine the equilibirum constant, Kc is known as

a)

Law of active mass.

b)

Law of mass action.

c)

Law of chemical reactions.

d)

Law of conservation of mass.

97.

For the graph, choose the CORRECT statement.

a)

The rate of reaction slowly increase

b)

The systems never reach equilibrium

c)

At equilibrium, more NO2 is present than N2O4.

d)

At start of reaction, only NO2 was present.

98.

What does a value of Keq greater than 1 mean?

a)

more reactants than products exist at equilibrium

b)

more products than reactants exist at equilibrium

c)

the rate of the forward reaction is high at equilibrium

d)

the rate of the reverse reaction is high at equilibrium

99.

An equilibrium constant for the dissolving of a sparingly soluble ionic compound in water is called what?

a)

common ion

b)

solubility product constant

c)

heterogeneous equilibrium)

d)

Le Châtelier’s principle

e)

chemical equilibrium

100.

Consider the equilibrium: 2 NO2NO_2 (g) ⇌ N2O4N_2O_4 (g) + energy. The equilibrium will shift to the left as a result of

a)

adding a catalyst

b)

increasing the volume

c)

removing some N2O4N_2O_4

d)

decreasing the temperature

101.

An indication that an equilibrium system favours the products is a …

a)

large KcK_c

b)

positive ΔH

c)

very small value for KcK_c

d)

low activation energy

102.

Consider the equilibrium: PCl5PCl_5 (g) ⇌ PCl3PCl_3 (g) + Cl2Cl_2 (g).  A 1 L flask contains 0,02 mol PCl5PCl_5 , 0,05 mol PCl3PCl_3 and 0,05 mol Cl2Cl_2 at equilibrium. The value of KcK_c is …

a)

0,125

b)

2,50

c)

5,00

d)

8,00

103.

Of the following equilibria, only __ will shift to the left in response to a decrease in volume …

a)

4Fe(s) + 3 O2O_2 (g) ⇌ 2 Fe2O3Fe_2O_3 (s)

b)

H2H_2 (g) + Cl2Cl_2 (g) ⇌ 2HCl(g)

c)

2 SO3SO_3 (g) ⇌ 2 SO2SO_2 (g) + O2O_2 (g)

d)

2HI(g) ⇌ H2H_2 (g) + I2I_2 (g)

104.

What type of system must a chemical change at equilibrium be measured in?

a)

open system, where energy and particles can travel in and out of the system

b)

closed system, where only energy can travel in and out of a system

c)

isolated system, where neither energy nor particles are allowed to travel and out of a system

105.

For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 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

106.

When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00–liter flask, the reaction represented below occurs.

2SO2 (g) + O2 (g) ↔ 2SO3 (g)

After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO3. Based on these results, the equilibrium constant, Kc, for the reaction is

a)

20

b)

10

c)

6.7

d)

2.0

107.

For the following chemical equilibrium, Kp = 4.6 × 10-14 at 25 °C, find the value of Kc for this reaction at 25 °C.

2 Cl2(g) + 2 H2O(g) ⇔ 4 HCl(g) + O2(g)

a)

Kc = 2.2 × 10-14

b)

Kc = 4.6 × 10-14

c)

Kc = 9.4 × 10-14

d)

Kc = 1.9 × 10-15

e)

Kc = 1.1 × 10-12

108.

What is ΔH° for a reaction that has Kp = 1.456 at 273 K and Kp = 14.2 at 298 K?

a)

462 kJ/mol

b)

61.6 kJ/mol

c)

-462 kJ/mol

d)

-61.6 kJ/mol

e)

8.42 × 10-5 kJ/mol

109.

For a reaction Keq = 1.2 × 10-6 at T = 200 K. What is ΔG° for the reaction?

a)

-22.7 kJ/mol

b)

22.7 kJ/mol

c)

53.6 kJ/mol

d)

170 kJ/mol

e)

-53.6 kJ/mol

110.

Calculate the temperature for which Keq for a reaction is 1.04 × 103 where ΔH° = -83.2 kJ/mol and ΔS° = -246 J/mol ∙ K.

a)

0.307 K

b)

307 K

c)

274 K

d)

0.274 K

e)

cannot be determined without ΔG°

111.
Consider the following reaction :    
SO2 (g) +  NO2 (g) ↔ SO3 (g) + NO (g)  
had reached a state of equilibrium, was found to contain   0.40 M SO3 , 0.30 M NO, 0.15 M NO2 , and 0.20 M SO2. Calculate the equilibrium constant  for this reaction.
a)
4
b)
.42
c)
.25
d)
1
112.

A mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 1.00L stainless-steel flask at 430⁰C. The equilibrium constant Kc for the reaction H2 (g) + I2 ↔ 2HI (g) is 54.3 at this temperature. Calculate the concentrations of H2, I2 , and HI at equilibrium.

Use ICE Table

a)

[H2] = 0.107 M

[I2] = 0.107 M

[HI] = 0.768 M

b)

[H2] = 0.768 M

[I2] = 0.107 M

[HI] = 0.107 M

c)

[H2] = 0.107 M

[I2] = 0.768 M

[HI] = 0.107 M

d)

[H2] = 0.107 M

[I2] = 0.107 M

[HI] = 0.0768 M

113.

Calculate the pH of a solution with a hydrogen ion concentration of 1.5 x 10^-3 M.

a)

pH = 5.67

b)

pH = 2.82

c)

pH = 1.23

d)

pH = 1.43

114.

Oxygen molecules at temperature T have the same r.m.s. speed as helium molecules at 300 K. What is the temperature T ?

a)

106 K

b)

600 K

c)

850 K

d)

2400 K

115.

The volume of an ideal gas is V when its pressure is p. The r.m.s. speed of the gas molecules is proportional to

a)

pV

b)

p/V

c)

√pV

d)

√p/V

116.

The pressure of an ideal gas in a vessel is 1.5×105 Pa when the temperature is 350 K. What is the number of gas molecules per unit volume?

a)

1.7×1020 m-3

b)

1.4×1021 m-3

c)

1.2×1022 m-3

d)

3.1×1025 m-3

117.

What is an ideal gas?


I. obey all gas laws at all temperature and pressure

II. real gas near atmospheric pressure and room temperature

III. there is no forces of attraction or repulsion between molecules

a)

I only

b)

II only

c)

I, II

d)

I, II, III

118.

What is the approximate number of atoms in a cubic metre of an ideal monatomic gas at a temperature of 27⁰C and a pressure of 1x10⁵Pa.


[Boltzmann constant k = 1.38x10¯²³J K¯¹, R = 8.31 J K¯¹ mol¯¹]

a)

1 x 10²²

b)

6x10²³

c)

2 x 10²⁵

d)

3 x 10²⁶

119.

Which of the following is not an assumption of kinetic theory of gases?

a)

the total volume of the particles are negligible compare to the volume of container

b)

the number of particles are large

c)

the particles are moving with the same speed

d)

the collisions of particles are elastic

120.

The density of argon at a pressure of 1.00x10⁵Pa and at a temperature of 300 K is 1.60 kg m¯³. What is the root-mean-square speed of argon molecules at this temperature?

a)

216 m s¯¹

b)

250 m s¯¹

c)

306 m s¯¹

d)

433 m s¯¹

121.

The molecules of an ideal gas at thermodynamic (absolute) temperature T have a root-mean-square speed crms.


The gas is heated to temperature 2T.


What is the new root-mean-square speed of the molecules?

a)

2crms\sqrt{2c_{rms}}

b)

2crms\sqrt{2}c_{rms}

c)

2crms2c_{rms}

d)

4crms4c_{rms}

122.

The mean kinetic energy of CO2 gas molecules at temperature T is

a)

12kT\frac{1}{2}kT

b)

32kT\frac{3}{2}kT

c)

52kT\frac{5}{2}kT

d)

3kT

123.

A container having a volume of 1.0 m³ holds 5.0 moles of helium gas at 50°C. If the helium behaves like an ideal gas, the total energy of the system is

a)

2.0 × 10⁴J

b)

2.5 × 10⁴J

c)

1.7 × 10³J

d)

1.5 × 10³J

124.

A container having a volume of 1.0 m³ holds 5.0 moles of helium gas at 50°C. If the helium behaves like an ideal gas, the average kinetic energy per molecule is

a)

6.7 × 10−²¹ J

b)

1.0 × 10−²¹J

c)

1.0 × 10−²⁰J

d)

6.7 × 10−²¹ J

125.

Which statement below is NOT an assumption made in the molecular model of an ideal gas?

a)

The average separation between molecules is large compared with the dimensions of the molecules.

b)

The molecules undergo inelastic collisions with one another.

c)

The forces between molecules are short range

d)

The molecules obey Newton's laws of motion

126.

Boyle's Law shows the relationship between which two factors of a gas?

a)

volume and pressure

b)

temperature and pressure

c)

pressure and temperature

d)

volume and temperature

127.
Charles's law shows the relationship between which two factors of a gas ?
a)
volume and temperature 
b)
volume and pressure 
c)
pressure and volume
d)
volume and mass
128.
Consider the following conditions: (1) low temperature, (2) low density, (3) temperature near the freezing temperature, (4) temperature above the condensation temperature, and (5) high density. Under which of these conditions does a real gas behave as an ideal gas?
a)
1 and 2 only
b)
1 and 5 only
c)
2 and 3 only
d)
2 and 4 only
e)
A real gas can never behave as an ideal gas.
129.

The equation of state of an ideal gas is given by

a)

pV=mRT, here R is characteristic gas constant

b)

pV=nRT, here R is universal gas constant

c)

pV=NKT

d)

all of the mentioned

130.

The Van Der Waal's equation of states for a Real Gas is aV2\frac{a}{V^2}^{ }

a)

PV = RT

b)

(P+ aV2\frac{a}{V^2}^{ } )(V-b) = RT

c)

(P- aV2\frac{a}{V^2}^{ } )(V-b)=RT

d)

(P- aV2\frac{a}{V^2}^{ } )(V+b)=RT

131.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
132.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
133.
Real gases deviate from ideal gas behavior because real gas particles have
a)
volume and some attraction for each other
b)
no volume and no attraction for each other
c)
no volume but some attraction for each other
d)
volume but no attraction for each other
134.

Given an atmospheric pressure of 1.85 atm, what would be the pressure in mmHg?

a)

1406 mmHg

b)

0.00243 mmHg

c)

187 mmHg

d)

27.2 mmHg

135.

Which equation represents Dalton's Law?

a)

E = mc2

b)

PV = nRT

c)

P1 / T1 = P2 / T2

d)

Ptotal = P1 + P2 + P3

136.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
137.

If a gas has the same temperature throughout, which gas molecule has the highest average velocity?

a)

O2

b)

H2O

c)

H2

d)

Xe

138.

A mixture of 4.5% H2, 76% O2, and 19.5% N2 has a total pressure of 2.3 atm. What is the partial pressure of each of the gases?

a)

PH2 = 0.10 atm

P02 = 1.7 atm

PN2 = 0.45 atm

b)

PH2 = 2.3 atm

P02 = 0 atm

PN2 = 0 atm

c)

PH2 = 0.32 atm

P02 = 2.4 atm

PN2 = 3.1 atm

139.
Which of the following gases will effuse most slowly under the same physical conditions?
Don't forget to check for diatomics!
a)
Hydrogen
b)
Chlorine
c)
Ammonia (NH3)
d)
Bromine
140.
An unknown gas diffuses 0.25 times as fast as helium gas (He). What is the molecular mass of the unknown gas? 
a)
64 g/mol
b)
16 g/mol
c)
32 g/mol
d)
4 g/mol
141.

If the He in Problem 3 takes 20 sec to effuse, how long will the NH3 take

a)

5 seconds

b)

10 seconds

c)

20 seconds

d)

40 seconds

142.
In order to calculate the rate of effusion of a gas, you must compare it to that of another gas and
a)
take the square root of the molar mass of the lighter gas divided by the square root of the molar mass of the heavier gas.
b)
take the square root of the molar mass of the heavier gas.
c)
take the square root of the molar mass of the lighter gas.
d)
take the square root of the molar mass of the heavier gas divided by the square root of the molar mass of the lighter gas.
143.

The density of argon at a pressure of 1.00x10⁵Pa and at a temperature of 300 K is 1.60 kg m¯³. What is the root-mean-square speed of argon molecules at this temperature?

a)

216 m s¯¹

b)

250 m s¯¹

c)

306 m s¯¹

d)

433 m s¯¹

144.
BaCl2
a)
soluble
b)
insoluble
145.
NH4NO3
a)
soluble
b)
insoluble
146.
AgCl
a)
soluble
b)
insoluble
147.

Ions that do not take part in a chemical reaction are called:

a)

Precipitates

b)

Spectators

c)

Net Ionic equation

d)

Solubles

148.

CH3OH(g) → CO(g) + 2H2(g)  

The reaction mixture contains 6.30 mol of CO(g) at equilibrium at 327°C. Calculate the number of moles of H2(g)  in the tank. 

a)

12.6 mol H2

b)

1 mol H2

c)

2 mol H2

d)

36 mol H2

149.

The temperature of an ideal gas is raised from 135K to 270K, while the pressure remains constant. Which  statement correctly identifies what happens to the volume?

a)

Remains the same

b)

Doubles in size

c)

Shrinks to ½ the original volume

d)

 Increases by a factor of 10

150.

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

a)

A

b)

B

c)

C

d)

D

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