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Chemistry Final Review A

Total questions: 58

Worksheet time: 15hrs 30mins

Name
Class
Date
1.

Which of the following represent(s) a chemical Change?

1) Rusting of an iron bridge.

2) melting of ice.

3) burning of a wooden stick.

4) boiling of water.

5) dissolving of sugar in water.

a)

1 and 3

b)

2 and 5

c)

1 to 4

d)

1,3 and 4

e)

2,3 and 5

2.

Which of the following properties of a metal are chemical properties?

1) It is hard.

2) it rusts in air.

3) Its density id 5.5 g/cm3

4) It reacts with a base

5) It is a good electrical conductor

a)

3 only

b)

1 and 2

c)

2 and 4

d)

1 and 3

e)

all of the above

3.

Assuming the numbers given are measurements, carry out the indicated arithmetic operation and give the answer with the correct number of significant figures.

2.36 x 102 + 5.4 x 103

a)

7.76 x 102

b)

7.76 x 103

c)

5.6 x103

d)

5.636x103

e)

5.64x103

4.

Oxygen boils at -297.3 F (Fahrenheit). What is this temperature in Kelvin?

a)

-195.8 K

b)

-47.2 K

c)

0 K

d)

90.2 K

e)

160.2 K

5.

How many protons, neutrons, and electrons are in the 14C atom?

a)

6 protons, 8 neutrons, 6 electrons.

b)

8 protons, 6 neutrons, 8 electrons

c)

6 protons, 8 neutrons, 8 electrons.

d)

14 protons, 14 neutrons, 14 electrons

e)

6 protons, 14 neutrons, 6 electrons.

6.

Give the name of the following compound: N2O3

a)

nitrogen oxide

b)

dinitrogen oxide

c)

dinitrogen trioxide

d)

nitrogen trioxide


e)

nitrogen oxygen

7.

An element has two naturally occurring isotopes with following masses and natural abundances:

Isotope Mass ( amu ) Abundances (%)

W 68.9257 60.12

X 70.9249 39.88

What is the identity of the element above?

a)

T1

b)

Zn

c)

Ni

d)

Ga

e)

Cu

8.

The correct formula for iron (II) chloride is:

a)

FeC1

b)

FeC12

c)

FeC13

d)

Fe2C1

e)

Fe2C12

9.

Alkaline earth metal cations carry a charge of what?

a)

2+

b)

1+

c)

0

d)

1-

e)

2-

10.

What is the net ionic equation for the reaction between aqueous sodium hydroxide (NaOH) and aqueous nitric acid (HNO3)?

a)

H+(aq) + NO3 (aq) + Na+ (aq) + OH (aq) → H2O(l) +Na+(aq) + NO3 (aq)

b)

H+(aq) + OH - (aq) → H2O(l)

c)

HNO3 (aq) + NaOH (aq) → NaNO3(aq)

d)

Na+(aq) + NO3 (aq)→NaNO3(aq)

e)

HNO3(aq)+OH (aq)→H2O(l) + NO3 (aq)

11.

Determine the initial volume needed to generate 2.50 L of 1.50 M HNO3 from 2.50 M HNO3 by dilution.

a)

2.50 L

b)

2.50 M

c)

1.50 M

d)

1.50 L

e)

0.9 mL

12.

Determine the simplest formula of the compound which has the composition 51.4 % C, 8.6% H, and 40.0% N by mass

a)

CHN

b)

C3H6N2

c)

C4H8N2

d)

C5H7N

e)

C6H10N

13.

Which of the following compounds is soluble in water?

a)

Ba(OH)2

b)

AgC1

c)

MgCO3

d)

CaF2

e)

PbSO4

14.

A Mixture of 10.0 g of NO and 14.0 g of NO2 results in the production of 8.52 g of N2O3.

What is the percentage yield?

NO(g) + NO2(g) → N2O3(l)

a)

36.9%

b)

60.2%

c)

71.4%

d)

85.6%

e)

100%

15.


A 20.00 mL sample of nitric acid, HNO3, requires 0.432 g of barium hydroxide, Ba (OH)2 for titration to the equivalence point. What is the concentration of the nitric acid?

2 HNO3(aq) + Ba (OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l)

a)

0.045 M

b)

0.126 M

c)

0.252 M

d)

0.510 M

e)

0.064 M

16.

The combustion of methane (CH4) produces carbon dioxide (CO2) and steam (H2O).

All of the following statements concerning this reaction are correct EXECPT

a)

one molecule of carbon dioxide is formed per one molecule of methane consumed.

b)

two molecules of oxygen are consumed per one molecule of methane consumed.

c)

two moles of steam are formed per two moles of oxygen consumed.

d)

the combined mass of reactants consumed equals the mass of products formed.

e)

one gram of carbon dioxide is formed per two grams of oxygen consumed.

17.

When A1(OH)3 reacts with sulfuric acid, the following reaction occurs:

2 Al(OH)3 + 3 H2SO4 → A12(SO4)3 + 6 H2O

If 0.45 x 103 g of A1(OH)3 is combined with 880g of H2SO4 how much aluminum sulfate can form?

a)

990 g

b)

790 g

c)

986 g

d)

791 g

e)

828 g

18.


Which of the following relationships are true for gases?

i) The volume of a gas is directly proportional to its pressure (at constant temperature).

ii) The pressure of a gas is inversely proportional to its temperature in kelvins (at constant volume).

iii) The number of moles of a gas is directly proportional to its volume (at constant pressure and temperature).

a)

i only

b)

ii only

c)

iii only

d)

i and ii

e)

ii and iii

19.

A mixture of He and O2 is placed in a 4.00 L flask at 32 degrees C. The partial pressure of the He is 3.0 atm and the partial pressure of the O2 is 2.0 atm. What is the mole fraction of O2?

a)

0.20

b)

0.30

c)

0,40

d)

0.50

e)

0.60

20.


At Constant temperature, 14.0 L of O2 at 2.70 atm is compressed to 1.75L. What is the final pressure of O2?

a)

0.110 atm

b)

0.142 atm

c)

7.06 atm

d)

21.6 atm

e)

27.8 atm

21.

Which of the followings are not generally true of gases?

1) Gas particles do not collide with each other.

2) Gases expand to fill the volume of a container.

3) Gases have lower densities than solids of liquids

4)Lighter gas particles tend to move faster at the same temperature.

5)At a fixed temperature, as pressure increases, average speed increases.

a)

1,2 and 4

b)

2, 3 and 4

c)

3, 4 and 5

d)

3 and 5

e)

1 and 5

22.

The ideal gas law begins to break down:

1) at high temperatures

2) at low temperatures

3) at high pressures

4) at low pressures

5) at low volume

a)

1 and 3

b)

1 and 4

c)

2 and 3

d)

2 and 4

e)

5

23.

A particular orbital has n = 3 and l =1. What must this orbital be?

a)

3s

b)

3p

c)

3d

d)

4s

e)

4p

24.

Write the ground state electron configuration for titanium.

a)

[ AR] 4s23d2

b)

[AR] 4s24p2

c)

[AR]3d4

d)

[AR] 3d24p2

e)

[Kr] 4s23d2

25.

How many valence electrons are in gallium?

a)

1

b)

2

c)

3

d)

4

e)

5

26.

Which of the following represents invalid set of quantum numbers?

a)

n = 3, l = 2, ml = -2

b)

n=2, l =1, ml = 0


c)

n=4, l = 3, ml = 2

d)

n = 2, l = 3, ml = 4

e)

n = 5, l = 0, ml = 0

27.

Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)

a)

has a filled valence shell of electrons.

b)

has two electrons per orbital, each with the same spins.

c)

has ml values greater than or equal to zero

d)

has two elecctrons per orbital, each with opposing spins.

e)

has the maximum number of unpaired electrons, all with the same spin.

28.


If hydrogen atom undergoes a transition from n = 1 (E = 4.17 x 10-19 J) to n = 3 (E=8.62 x 1019J), what is the wave length of the photo absorbed?

a)

4.46 x 10-7 m

b)

4.45 x 10-19 J

c)

6.72 x 10-16 s-1

d)

4.46 x 10-7 J

e)

4.45 x 10-19 m

29.


Select the element that is expected to have the most negative electron affinity

a)

K

b)

Te

c)

Cl

d)

Ca

e)

Ge

30.

Choose the compound below that should have the largest lattice energy


a)

KF

b)

NaF

c)

CaO

d)

MgS

e)

MgO

31.

Which of the following compounds illustrates sp3 hybridization?

a)

C2H4

b)

BeF2

c)

CCl4

d)

V2O5


e)

SO2

32.

What is the correct electron configuration of the potassium cation?

a)

1s22s22p63s23p64s2

b)

1s22s22p63s13p64s1

c)

1s22s22p63s23p6

d)

1s22s22p63s23p5

e)

1s22s22p63s23p4


33.


Which of the following molecules have a trigonal bipyramidal geometry?

BrF5 SF4 PCl5

a)

BrF5, SF4

b)

BrF5,SF4,PCl5

c)

SF4

d)

BrF5

e)

PCl5

34.

In assembling a Lewis Dot Diagram of CF2Cl2, there are ______ total electrons to use in the model.

a)

50

b)

48

c)

40

d)

32

35.

Choose the substance that corresponds to an n-type semiconductor

a)

Ge doped with P

b)

As doped with Si

c)

Si doped with A1

d)

Sn doped with Ga

e)

P doped with Ge

36.

What's the packing efficiency of the body - centered cubic structure?

a)

52%

b)

68%

c)

74%

d)

78.5%

e)

90.7%

37.

the isotopes of carbon are

a)

CO2; CO; CO32-

b)

diamond; graphite; fullerene

c)

12C; 13C; 14C;

d)

CO2; graphite; 12C

e)

C; Si; Ge; Sn; Pb

38.

Which type (s) of intermolecular forces need to be overcome to convert acetone [(CH3)2CO] from liquids to gases?

i. dispersion; ii. dipole-dipole; iii. H-bonding

a)

i only

b)

ii only

c)

iii only

d)

i and ii

e)

all of them

39.

Which of the following substances represents an excellent conductor of electricity?

a)

zinc

b)

silicon

c)

sucrose

d)

iodine

e)

argon

40.


In the calibration of a calorimeter, an electrical resistance heater supplies 100.0 J of heat and

a temperature increase of 0.850°C is observed. Then, 0.214 g of a particular fuel is burned in

this same calorimeter and the temperature increases by 4.23°C. Calculate the energy density

of this fuel, which is the amount of energy liberated per gram of fuel burned

a)

118 J/°C

b)

- 499 J

c)

499 J

d)

2.33 kJ/g

e)

-2.33 kJ/g

41.


Explain why the following is not a formation reaction.

4Na(s)+O(g)→2NaO(s)

a)

The standard state of oxygen is O(g).

b)

The equation is not balanced

c)

Two moles of the compound are formed

d)

Gases can only be on the product side.

e)


The product is not an element.

0 an

42.

Calculate ΔE for the system in which 16 J of work is done on a gas by the surroundings and

the gas releases 51 J of heat?

a)

-67 J

b)

-35 J

c)

+35 J

d)

+51 J

e)

+67 J

43.

For the reaction, how much energy is needed to generate 20 moles of NO(g)?

N(g)+O(g)→2 NO(g) ∆H = 180.5 kJ

a)

1.3 x104 kJ

b)

180.5 kJ

c)

1800 kJ

d)

9.7 x 103 kJ

e)

3.2x103 kJ

44.

Using these two equations,

C (graphite) + PbO(s)→Pb(s) + CO(g) ∆H°= 106.8 kJ

2C(graphite)+ O2(g)→2CO(g) ∆H°=-221.0 kJ

find the standard enthalpy change for the formation of 1 mol PbO(s) from lead metal and oxygen gas.

Pb(s) + ½ O (g)→PbO ∆H°= ?

a)

-217.3 kJ

b)

-262 kJ

c)

+262 kJ

d)

+327 kJ

e)

0.99 kJ

45.

Without doing a calculation, predict which of the following shows a

decrease in entropy?

a)

2 HNO3(l) + NO(g)→3NO2(g) + H2O(l)

b)

FeCl2(s) + H2(g) →Fe(s) +2HCl(g)

c)

CO(g)+2H2 (g) → CH3OH(l)

d)

2H2O(g) + →2H2(g) + O2(g)

e)

CH3OH(l) + 3/2 O2(g)→2H2O(g) + CO2(g)

46.

The sign of ∆Hrxn and ∆S rxn for several reactions are given. In which case is the reaction nonspontaneous at all temperatures?

a)

∆Hrxn < 0; ∆Srxn < 0

b)

∆Hrxn < 0; ∆Srxn > 0

c)

∆Hrxn > 0; ∆Srxn < 0

d)

∆Hrxn > 0; ∆Srxn > 0

e)

∆Hrxn = ∆Srxn

47.

Select the correct statement that corresponds to the second law of thermodynamics.

a)

he standard Gibbs free energy change, ΔGo, can be calculated from Gibbs free energies

of formation, ΔGfo

b)

The entropy of a perfect crystal of any pure substance approaches zero, as the

temperature approaches absolute zero (0 K)

c)

The entropy change for a reaction, ∆So, can be calculated from the standard molar

entropies of the reactants and products

d)

ΔEuniverse = ΔEsystem + ΔEsurroundings = 0

e)

In any spontaneous process, ΔSuniverse = ΔSsystem + ΔSsurroundings >0

48.

When magnesium sulfite decomposes, the solid transforms into magnesium oxide and sulfur dioxide.

MgSO3(s) → MgO(s) + SO2 (g)

At what temperature will this reaction be spontaneous according to Gibb's Energy?

ΔGfo in kJ/mol for: MgSO3(s) = −1172, MgO(s) = −569.6, SO2(g) = −300.2

ΔHfoin kJ/mol for: MgSO3(s) = −1068, MgO(s) = −601.8, SO2(g)) = −296.8

Soin J/mol K for: MgSO3(s) = 121, MgO(s) = 27, SO2(g) = 248.1

a)

temps

below −63.1 K

b)

temps below 179.5 K

c)

temps below 415.8 K

d)

temps above 415.8 K

e)

temps above 1100 K

49.

If a 5.0 L flask holds 0.125 moles of nitrogen at STP, what happens to the entropy of the

system upon heating the gas to 75 °C?

a)

The entropy is zero

b)

The entropy increases

c)

The entropy remains the same

d)

The entropy decreases.

e)

There is too little information to assess the change

50.

The randomness of a system may be described as its:

a)

enthalpy

b)

entropy

c)

kinetic energy

d)

Gibb's energy

e)

reaction rate constant

51.


In the first 10.0 s of the reaction, the concentration of B decreased from 0.50 M to 0.35 M.

What is the rate of the reaction in this time interval?

a)

2.3 M/s

b)

5.0 x 10-3 M/s

c)

0.13 M/s

d)

1.3 x 10-2 M/s

e)

4.3 x 10-3 M/s

52.

If the initial concentration of the reactant in a first-

order reaction A → products is 0.64 mol/L and the half-life is 30.0 s, how long would it take for the concentration of the reactant to drop

to 0.020 mol/L?

a)

30.0 s

b)

60.0 s

c)

90.0 s

d)

120.0 s

e)

150.0 s

53.

Consider the elementary step: 2A → C. What type of elementary step is this?

a)

unimolecular

b)

bimolecular

c)

termolecular

d)

all of the above

e)

none of the above

54.


If a reaction is first order with respect to [B], tripling the concentration of [B] will result in:

a)

a doubling of the rate

b)

a tripling of the rate

c)

a four-fold increase in rate

d)

an eight-fold increase in rate

e)

no change in the rate of reaction

55.

The decomposition of N2O5

in solution of carbon tetrachloride is a first-order reaction:

2 N2O5 →4 NO2 + O2

The rate constant at a given temperature is found to be 5.25 × 10-4 s-1..

If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 5 minutes have passed?

a)

0.000 M

b)

0.073 M

c)

0.146 M

d)

0.171 M

e)

0.199 M

56.

Consider the reaction: 2A + B → C, and a kinetics study on this reaction yielded:

[A] mol·L -1 [B] mol·L -1 Rate = mol·L-1⋅ s-1

0.100 0.200 5.03 × 10-3

0.050 0.200 1.27 × 10-3

0.050 0.100 1.25 × 10-3

a)

0.503 L· mol-1·s-1

b)

3.20 L· mol-1·s-1

c)

4.60 L· mol-1·s-1


d)

19.8 L· mol-1·s-1

e)

4.60 s-1

57.

Predict the order of vapor pressure for the following compounds

i. FCH2CH2 F;

ii. FCH2CH2OH;

iii) HOCH2CH2OH

a)

i > ii >iii

b)

i > iii >ii

c)

ii > i >iii

d)

ii > iii >i

e)

iii > ii >i

58.


What volume of O2, measured at 91.2 °C and 743 mm Hg, will be produced by the decomposition of 3.25 g KClO3? (R = 0.08206 L·atm/mol·K)

2 KClO3(s) → 2 KCl(s) + 3 O2(g)

a)

0.305 L

b)

1.22 L

c)

1.83 L

d)

24.0 L

e)

37.4 L

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