Chemistry Fundamentals Multiple Choice Questions Quiz

1. PH is an important factor in

Consumer products

Swimming pools

Human blood

Soil in gardens and farms

All of the above

Test 5

Explanation

Test 5

2. One atomic mass unit is defined as

Exactly 1/14 the mass of a C-12 atom

Exactly 14 times the mass of a C-12 atom

Exactly 1/12 the mass of a C-12 atom

Exactly 12 times the mass of a C-12 atom

None of the above

Test 3

Explanation

Test 3

3. An acidic solution such as vinegar

Turns litmus paper blue

Turns litmus paper red

Has a salty taste

Feels slippery

Has a bitter taste

Test 5

Explanation

Test 5

4. Classify the following reaction: 2NaClO3 = 2NaCl + 3O2

Combustion

Synthesis

Decomposition

Single displacement

Double displacement

Test 2

Explanation

Test 2

5. Which of the following careers would involve a lot of work with solutions?

Chemistry teacher

Water quality analyst

Environmental chemist

Quality control technician

All of the above

Test 5

Explanation

Test 5

6. Which of the following is true for hydrochloric acid?

HCl = H + Cl (

It is a weak acid

HCl = H + Cl (>99%)

HCl = H + Cl (>50%)

HCl = H + Cl (

Test 5

Explanation

Test 5

7. An example of a binary compound is

NaOH

O2

H2S

CaCO3

Co

Test 1

Explanation

Test 1

8. A lab procedure involving the careful addition of an acid from a buret is called

Titration

Dilution

Endpoint

Standard

Distillation

Test 5

Explanation

Test 5

9. Hydroselenic acid is a very toxic substance. Its chemical formula is

HSe

H2SeO

H2Se

H2SeO3

H2SeO4

Test 2

Explanation

Test 2

10. An example of a binary compound is

NaOH

O2

H2S

CaCO3

Co

Test 2

Explanation

Test 2

11. Which of the following matches of group number and common name is incorrect?

Group 2 - Alkaline Earth Metals

Group 6 - Lanthanides

Group 1 - Alkali Metals

Group 17 - Halogens

Group 18 - Noble Gases

Test 1

Explanation

Test 1

12. Which of the following matches of group number and common name is incorrect?

Group 7 - Transition Metals

Group 2 - Alkali Earth Metals

Group 17 - Halogens

Group 2 - Actinides

Group 18 - Noble Gases

Test 1

Explanation

Test 1

13. Which of the following is a common source of water contamination?

Landfill leachate

Agricultural fertilizers and pesticides

Road salt runoff

Mining and mine tailings

All of the above

Test 4

Explanation

Test 4

14. The particle that has the smallest mass is the

Electron

Proton

Nucleus

Ion

Neutron

Test 1

Explanation

Test 1

15. An amphiprotic substance

Acts only like an acid

Acts like an acid or a base

Acts only like a base

Remains neutral

None of the above

Test 5

Explanation

Test 5

16. Classify the following reaction: Cl2 + ZnI2 = ZnCl2 + I2

Combustion

Synthesis

Decomposition

Single displacement

Double displacement

Test 2

Explanation

Test 2

17. Stainless steel is harder than pure iron because

It is an alloy

It is metallic

The electrons in it are free to move

All of the above

None of the above

Test 2

Explanation

Test 2

18. The IUPAC name for KMnO4 is

Krpyton manganese tetraoxide

Potassium manganate

Potassium permanganate

Potassium manganese oxide

Potassium monomanganese tetraoxide

Test 2

Explanation

Test 2

19. According to the Lewis model of the atom, the number of bonding electrons in a nitrogen atom is

1

2

3

5

7

Test 1

Explanation

Test 1

20. The person given credit for developing the first modern periodic table is

Dalton

Democritus

Thomson

Mendeleev

Chadwick

Test 1

Explanation

Test 1

21. Multivalent metals

Can form more than one ion, each with its own charge

Can exist in several different crystalline forms

Appear only in the representative metal groups

Contain more than one populated energy level

Form an ion whose charge is 2+ or greater

Test 1

Explanation

Test 1

22. The substance NH3 is a very important industrial chemical. It is used directly as a fertilizer and is also used to produce many other useful chemicals. The IUPAC name of this substance is

Hydrogen nitride

Ammonia

Hydrogen peroxide

Octane

Ammonium

Test 2

Explanation

Test 2

23. Which of the following expresses standard atmospheric pressure?

125 kPa

100 atm

1.00 atm

96.7 kPa

10.0 atm

Test 6

Explanation

Test 6

24. The total number of atoms represented in the formula Be(C2H3O2)2 is

4

8

15

22

29

Test 3

Explanation

Test 3

25. Which of the following is the most reactive element?

Helium

Radon

Francium

Hydrogen

Ununoctium

Test 1

Explanation

Test 1

26. What does the acronym SCUBA stand for?

Self contained underwater breathing apparatus

Self contained underwater breathing accessory

Self calibrated underwater breathing apparatus

Self calibrated underwater breathing accessory

Swimmer's calibrated underwater breathing apparatus

Test 6

Explanation

Test 6

27. Which of the following is NOT a property of acids?

They taste sour

They have a pH less than 7

They react with metals

They do not react with carbonates

They turn blue litmus red

Test 5

Explanation

Test 5

28. Carbon dioxide and water are produced when ethanol, C2H5OH, is burned in oxygen. The number of moles of CO2 that is produced when burning 6.0 mol of ethanol is

1.0

3.0

6.0

12.0

15.0

Test 3

Explanation

Test 3

29. A compound compoesd of sodium, sulfur, and oxygen would be named

Sodium peroxide

Sulfuric acid

Sodium sulfide

Sodium sulfate

Sodium hydroxide

Test 1

Explanation

Test 1

30. The reaction of silver nitrate with zinc would be classified as a

Combustion reaction

Synthesis reaction

Double displacement reaction

Decomposition reaction

Single displacement reaction

Test 2

Explanation

Test 2

31. Which of the following always indicates that a chemical reaction has taken place?

Production of a gas

Absorption of heat

Change in colour

Appearance of a new substance

Production of heat

Test 2

Explanation

Test 2

32. Welders use two types of compressed gasses to produce very high temperatures to cut or weld metals. What are the two gasses used by welders to accomplish this?

Oxygen and hydrogen

Methane and oxygen

Acetylene and oxygen

Propane and oxygen

Acetylene and hydrogen

Test 6

Explanation

Test 6

33. Which one of the following statements is a quantitative observation?

The freezing point of the clear and colourless solution was -40.5 degrees celsius

The reactant demonstrated a high degree of viscosity

The overall reaction was exothermic

The product was yellow in colour

A brown coloured gas evolved from the test tube

Test 3

Explanation

Test 3

34. Doubling the initial pressure while keeping the temperature constant causes the volume of a gas to go from 1000mL to

2000mL (double)

500mL (halved)

1000mL (constant)

About 900mL (slight decrease)

1100mL (slight increase)

Test 6

Explanation

Test 6

35. Determine the number of grams of HCl needed to react completely with 12.8g of aluminum, acording to the following equation: 2Al + 6HCl = 2AlCl3 + 3H2

51.9g

17.3g

34.6g

103.8g

38.4g

Test 3

Explanation

Test 3

36. The IUPAC name for P2I4 is

Phosphorus iodide

Diphosphorus tetraiodide

Tetraphosphorus diiodide

Phosphorus pentaiodide

Dipotassium tetraiodide

Test 2

Explanation

Test 2

37. According to the periodic law, chemical properties are repeated at a regular interval when

Elements are listed in order of their atomic radius

Elements are listed in order of their date of discovery

Families of elements are listed in order

Periods are arranged in order

Elements are arranged in order of increasing atomic number

Test 1

Explanation

Test 1

38. Which of the following is the correct net ionic equation for barium sulphate?

Ba(aq) + S(aq) = BaS(s)

B(aq) + SO3(aq) = BSO3(s)

Be(aq) + SO4(aq) = BeSO4(s)

Ba(aq) + SO4(aq) = BaSO4(s)

None of the above

Test 4

Explanation

Test 4

39. An isotope that has three times the mass of an atom of C-12 is most likely an atom of

Chlorine

Lithium

Calcium

Carbon

Fluorine

Test 3

Explanation

Test 3

40. Which of the following is the correct representation for a hydronium ion?

H

H3O

H2O

H4O

None of the above

Test 5

Explanation

Test 5

41. The kinetic molecular theory includes all of the following except

Molecules attract one another

Particles are small compared to the volume they occupy

Molecules move in straight line motion

Molecules collide elastically with one another

Molecules collide elastically with surrounding objects

Test 2

Explanation

Test 2

42. Hydrogen can be used as an alternative fuel for automobiles. Classify the following chemical reaction: 2H2 + O2 = 2H2O

Combustion reaction

Decomposition reaction

Single displacement

Double displacement

Simple decomposition

Test 2

Explanation

Test 2

43. Cola soft drinks have a sucrose concentration of 11g/100mL. What mass of sucrose is present in a 355mL can of Cola?

11g

39g

30g

22g

0.11g

Test 4

Explanation

Test 4

44. Which of the following is a practical use of radioisotopes?

Determining the age of old objects

Medical diagnosis

Production of electricity

All of the above

None of the above

Test 1

Explanation

Test 1

45. Which of hte following is NOT a property of bases?

They react with active metals

They taste bitter and feel slippery

They have a pH greater than 7

They turn red litmus blue

They neutralize acids

Test 5

Explanation

Test 5

46. Potassium chloride and oxygen gas are formed upon heating potassium chlorate. The following balanced equation shows this decomposition process: 2KClO3 = 2KCl + 3O2The number of moles of KClO3 required to produce 5.0 mol of oxygen is

1.0

2.0

3.0

3.3

5.0

Test 3

Explanation

Test 3

47. The properties of elements repeat periodically if they are arranged by

Atomic mass

Atomic charge

Atomic number

Number of neutrons

Number of electrons

Test 1

Explanation

Test 1

48. What is the formula for zinc chloride?

ZnCl

ZnCl2

Zn1Cl1

Zn1Cl2

Zn2Cl1

Test 2

Explanation

Test 2

49. If the molar mass of a hydrocarbon is 26.0g/mol, and its empirical formula is CH, its molecular formula is

CH

C2H2

C3H3

C4H4

C5H5

Test 3

Explanation

Test 3

50. Two atoms are isotopes if they have

Different atomic numbers

The same mass number, but different atomic numbers

The same number of protons and neutrons

The same number of electrons, but a different number of neutrons

The same atomic number, but a different mass number

Test 1

Explanation

Test 1

51. Which of the following metals would most likely oxidize if a clean metal surface is exposed to the atmosphere?

Aluminum

Iron

Gold

Silver

Zinc

Test 2

Explanation

Test 2

52. Which of the following is not a solution?

Oxygen in water

Tin in copper (bronze)

Sand in water

Sugar in water

Sea water

Test 4

Explanation

Test 4

53. A compound that ionizes in water to form hydroxide ions is

An acid

A salt

A base

Both A and B

Both B and C

Test 5

Explanation

Test 5

54. The formula for carbon tetrachloride is

C1Cl4

C4Cl4

C1Cl

CCl4

C4Cl1

Test 2

Explanation

Test 2

55. Tin and oxygen can combine to form two compounds of different combining proportions. Resulting formulas of these compounds include

Sn2O and SnO2

SnO and SnO2

SnO4 and SnO

SnO and SnO3

SnO2 and SnO4

Test 3

Explanation

Test 3

56. Nitric acid is classified as a strong acid because

It has high electrical conductivity

It ionizes about 50%

Ionizes more than 99%

Both A and C

It has a higher concentration than other acids

Test 5

Explanation

Test 5

57. At a fixed temperature and pressure, the average distance between molecules would be greater in a sample of

Air

Concrete

Sponge

NaCl

Liquid perfume

Test 6

Explanation

Test 6

58. A new element, dmytrium, has two isotopes, Dm-350 and Dm-375. The composition of dmytrium is 62.0% Dm-350 and 38.0% Dm-375 by mass. The relative atomic mass of this new element is

351 u

354 u

357 u

366 u

360 u

Test 3

Explanation

Test 3

59. The dissociation equation K3PO4(s) = 3K(aq) + PO4(aq) represents

Soluble potassium phosphate

Insoluble sodium phosphate

Soluble potassium carbonate

Soluble potassium phosphide

Soluble potassium phosphite

Test 4

Explanation

Test 4

60. If XF2 is the correct formula for a metallic fluoride, then the formula for the oxide of X is

X2O

XO

XO4

XO2

X2O2

Test 2

Explanation

Test 2

61. Which of the following formulas does not represent a molecular compound?

CO2

CoCl2

SO2

PCl5

HCl

Test 1

Explanation

Test 1

62. The IUPAC name for CaCl2 is

Calcium chloride

Calcium (II) chloride

Calcium dichloride

Calcium chlorate

Monocalcium dichloride

Test 1

Explanation

Test 1

63. Which of the following atoms is believed to contain three lone pairs of electrons?

H

Al

B

C

Cl

Test 1

Explanation

Test 1

64. One way to produce oxygen gas is via the decomposition of potassium chlorate, as shown in the equation KClO3 = KCl + O2. When properly balanced the sum of the coefficients is

3

6

7

10

11

Test 3

Explanation

Test 3

65. The SI symbol used for the atomic mass unit

Au

Atu

U

Atm

Am

Test 3

Explanation

Test 3

66. Which of the following best describes on mole of potassium sulfate, K2SO4?

It contains six atoms in total

It contains one sulfur atom

It has a mass of 174.3g

It contains 3.01 x 10^23 molecules

None of the above

Test 3

Explanation

Test 3

67. The element found in the periodic table in Group 4 and Period 6 is

Halfnium, Hf

Selenium, Se

Gadolinium, Gd

Chromium, Cr

Aluminum, Al

Test 1

Explanation

Test 1

68. The point during a titration at which a sharp colour change occurs is called the

Mixed point

End point

Neutralization point

Fixed point

Last point

Test 5

Explanation

Test 5

69. If the name of a chemical compound ends in "ide", the compound is

Acidic

Binary

Basic

An oxide

None of the above

Test 1

Explanation

Test 1

70. The atomic mass of barium is due to the number of

Neutrons and electrons in the nucleus

Electrons in the nucleus

Protons and neutrons in the nucleus

Protons and electrons in the atom

Protons in the nucleus

Test 1

Explanation

Test 1

71. A instrument used to measure gas pressure is a

Barometer

Thermometer

Calorimeter

Anemometer

Hygrometer

Test 6

Explanation

Test 6

72. Household ammonia has a pH of 12.5 and lye has a pH of 13.5. Which of the following is true?

Ammonia is ten times more basic than lye

Lye is two times more basic than ammonia

There is no significant difference in the acidities of ammonia and lye

Lye is ten times more basic than ammonia

Ammonia is less acidic than lye

Test 5

Explanation

Test 5

73. A metaloid in Period 3 is

Scandium

Aluminum

Germanium

Phosphorus

Silicon

Test 1

Explanation

Test 1

74. Which metal would not displace gold, Au, from a compound?

Copper, Cu

Potassium, K

Lithium, Li

Magnesium, Mg

None of the above

Test 2

Explanation

Test 2

75. What is the formula for copper(II) nitrite?

Cu2(NO3)

Cu(NO3)2

Cu(NO2)2

Cu2(NO2)

Cu(NO3)

Test 2

Explanation

Test 2

76. Oxygen and carbon dioxide have low solubilities in water because

They are big, bubbly gasses

They are non-polar molecules

They are polar molecules

Water is nonpolar

They want to stay in air

Test 4

Explanation

Test 4

77. Breathalyzers can determine blood alcohol content indirectly by

Aqueous dichromate ions (orange) + alcohol = chromium(III) ions (green)

Permanganate ions turning purple

Copper solutions turning pink

Water + Alcohol = Red

None of the above

Test 4

Explanation

Test 4

78. The element found in the periodic table in Group 6 and period 4 is

Halfnium, Hf

Selenium, Se

Lithium, Li,

Gadolinium, Gd

Chromium, Cr

Test 1

Explanation

Test 1

79. A solution that has a relatively large quantity of solute dissolved in the solvent is

Homogeneous

Dilute

Concentrated

Mixed

Saturated

Test 4

Explanation

Test 4

80. Intermolecular forces are

Forces among molecules

Covalent bonds

Ionic bonds

Forces within molecules

None of these

Test 4

Explanation

Test 4

81. Which of the following compounds is insoluble in water?

CaCl2

Al(NO3)3

PbBr2

Li2CO3

NH4OH

Test 4

Explanation

Test 4

82. Which of the following has a concentration of 2mol/L

2mol/1L

2mol/1000mL

5mol/2.5L

2mol/2L

A, B, and C only

Test 4

Explanation

Test 4

83. Screening, flotation, settling, and filtering out of solid particles in waste water occurs during the

Secondary treatment

Tertiary treatment

Primary treatment

Quaternary treatment

All of the above

Test 4

Explanation

Test 4

84. The contamination of Walkerton, Ontario's water supply in 2000 was caused by

Lead

Mercury

Pesticides

E.coli bacteria

Nitrates

Test 4

Explanation

Test 4

85. Converting 4.8 x 10^-2mol of ammonium hydroxide (NH4OH) into mass yields

0.6g

1.0g

1.3g

1.7g

2.2g

Test 3

Explanation

Test 3

86. The percentage of nitrogen, by mass, in nitric acid, HNO3, is

1.6%

11.1%

15.6%

22.2%

72.6%

Test 3

Explanation

Test 3

87. Why is it easier to remove an electron from potassium than it is to remove an electron from calcium?

Potassium has a higher electron affinity

Potassium has a higher ionization energy

Potassium has a lower nuclear charge

Calcium has a lower electron affinity

Calcium is a metal, but potassium is not

Test 1

Explanation

Test 1

88. The systematic IUPAC name for HBr(aq) is

Aqueous bromine

Aqueous hydrogen bromide

Hypobromic acid

Hydrobromic acid

Bromic acid

Test 1

Explanation

Test 1

89. Which of the following would not precipitate the CO3 ion?

Co

H

Mg

Ba

Pb

Test 4

Explanation

Test 4

90. A sample of a gas with a volume of 1L at 25 degrees celsius and a pressure of 101.325 kPa is subjected to an increase in pressure and a decrease in temperature. The volume of the gas will

Decrease

Increase

Remain the same

Become zero

Either increase or decrease, depending on the magnitude of the pressure and temperature changes

Test 6

Explanation

Test 6

91. Pure oxygen boils at -183 degrees celsius and freezes at -219 degrees celsius. What state will the oxygen be in if the temperature is brought to within 50K of absolute zero?

Solid

Liquid

Gas

Plasma

Solution

Test 6

Explanation

Test 6

92. The limiting reagent of a chemical reaction is

The reactant of a chemical process that is not consumed completely

The product of a chemical process that is consumed completely

The product of a chemical process that is not consumed completely

The reactant of a chemical process that is consumed completely

None of the above

Test 3

Explanation

Test 3

93. The concept of multiple covalent bonds is used to explain the molecular formula of

O2

NaCl

C2H6

F2

NaOH

Test 1

Explanation

Test 1

94. Which of the following contains 1mol of dissolved copper(II) nitrate?

500mL of a 0.5mol/L solution

750mL of a 0.75mol/L solution

500mL of a 2.0mol/L solution

1L of a 0.9mol/L solution

2L of a 0.4mol/L solutions

Test 4

Explanation

Test 4

95. A metallic element X forms a carbonate with the formula X(CO3)2. The corresponding fluoride compound of element X would have the formula

XF

XF2

X4F2

X4F

XF4

Test 1

Explanation

Test 1

96. The atomic number is the number of

Protons in the nucleus

Neutrons in the nucleus

Protons plus the number of neutrons in the nucleus

Electrons plus the number of protons in the nucleus

Electrons plus the number of neutrons in the nucleus

Test 1

Explanation

Test 1

97. The concentration of fluoride ions, F-, in municipal drinking water cannot exceed 1.5ppm. What is the maximum mass of fluoride ions that can be dissolved in 500mL of water?

0.75mg

1.5mg

750mg

0.003

3.0mg

Test 4

Explanation

Test 4

98. Which of the following laws states that volume and temperature (in Kelvin) of a gas are directly proportional at constant pressure and number of molecules?

Boyle's Law

Charles' Law

Dalton's Law

Avogadro's Law

Gay-Lussac's Law

Test 6

Explanation

Test 6

99. Determine the sum of all the reactant coefficients when the following equation is balanced: H3PO4 + BaCO3 = Ba3(PO4)2 + H2O + CO2

8

9

6

5

2

Test 3

Explanation

Test 3

100. The mass found in 0.10 mol of KHC4H4O6 is

4.6g

19g

23.7g

37.6g

55.8g

Test 3

Explanation

Test 3

101. A possible molecular formula for the compound CH2O is

C2H4O2

C3H6O3

C4H8O4

C10H20O10

All of the above

Test 3

Explanation

Test 3

102. Which of the following mixtures is homogeneous?

Orange juice from concentrate

Milk

Clay in water

Sand and rocks

Jello

Test 4

Explanation

Test 4

103. Blackberries have a [H+] = 4.0 x 10^-4 mol/L. What is their pH?

3.4

4.0

2.0

8.0

5.0

Test 5

Explanation

Test 5

104. How much more acidic is vinegar (pH = 2.0) than coffee (pH = 5.0)

3.0

1000

100

2.5

0.4

Test 5

Explanation

Test 5

105. Which of the following is the proper dot diagram for NaCl?

Refer to the test for this question

Option 2

Option 3

Option 4

Test 1

Explanation

Test 1

106. Which of the following combinations would result in the formation of a precipitate?

Acetic acid and potassium hydroxide solutions

Magnesium nitrate and sodium sulfide solutions

Sulfuric acid and barium hydroxide solutions

Sodium sulfate and copper(II) chloride solutions

Sodium chloride and ammonium nitrate solutions

Test 2

Explanation

Test 2

107. There are 3.01 x 10^23 atoms present in

0.5 mol of C

0.5 mol of Na

0.5 mol of Ar

None of the above

All of the above

Test 3

Explanation

Test 3

108. Converting 153.0g of Mg(CN)2 into moles yields approximately

0.98 mol

1.49 mol

2.53 mol

3.06 mol

2.00 mol

Test 3

Explanation

Test 3

109. Upon analysis in the lab, a compound is found to consist of 2.2% hydrogen, 26.7% carbon, and 71.1% oxygen. The empirical formula for this compound is

H2C2O4

HCO

HC2O

HCO2

HC2O2

Test 3

Explanation

Test 3

110. "The volume of a given mass of a gas varies directly as the absolute temperature if the pressure is kept constant" is a statement of

Boyle's Law

Charles' Law

Avogadro's Law

Dalton's Law

Gay Lussac's Law

Test 6

Explanation

Test 6

111. A certain gas was found to have a mass of 28.0g and occupy a volume of 22.4L at STP. What is the perssure of this gas?

1.00 atm

760 mm Hg

101.325 kPa

760 torr

All of the above

Test 6

Explanation

Test 6

112. Which of the following is not always conserved in a chemical reaction?

Total number of atoms

Total number of molecules

Mass

Energy

None of the above are conserved

Test 3

Explanation

Test 3

113. A nonmetal in Period 6 is

Astatine

Iodine

Polonium

Radon

Rubidum

Radon is a radioactive element that has no taste and no color. The actual contact with Radon does not create any harm. Radon is the only non-metal element of period 6 of the periodic table.

Explanation

Radon is a radioactive element that has no taste and no color. The actual contact with Radon does not create any harm. Radon is the only non-metal element of period 6 of the periodic table.

114. The empirical formula of a compound containing 92.3% carbon and 7.7% hydrogen, by mass, is

C20H20

C12H12

C6H6

CH4

CH

Test 3

Explanation

Test 3

115. The ratio of hydrogen to oxygen, by mass, in water is

2:1

1:2

1:16

1:8

16:1

Test 3

Explanation

Test 3

116. Determine the number of moles of chlorine, Cl2, that are required to form 2.50 mol of lithium chloride, LiCl, according to the following equation: 2LiI + Cl2 = 2LiCl + I2

2.00 mol

1.75 mol

1.50 mol

1.25 mol

1.00 mol

Test 3

Explanation

Test 3

117. The percentage composition of chlroine, by mass, in the compound K2PtCl4 is

47.0%

34.2%

18.9%

15.3%

11.3%

Test 3

Explanation

Test 3

118. An unkonwn gas has a density of 1.95g/L at STP. What is the molar mass of this gas knowing that the universal gas constant is 8.31 kPa L/mol K

22.4 g/mol

11.4 g/mol

43.7 g/mol

23.8 g/mol

140 g/mol

Test 6

Explanation

Test 6

119. A bottle contains 3L of 12mol/L H2SO4 solution. After half of the contents are usedup, the remaining solution has a concentration of

18mol/L

12mol/L

6mol/L

3mol/L

None of the above

Test 4

Explanation

Test 4

120. Which of the following processes occur during the tertiary treatment of wastewater?

Reverse osmosis

Steam distillation

Chemical precipitation

All of the above

None of the above

Test 4

Explanation

Test 4

121. Which of the following is the correct dissociation reaction for calcium hydroxide?

Ca(OH)2 = Ca + 2OH

CaOH = Ca + OH

Ca(OH)2 = 2Ca + OH

Ca(OH)3 = Ca + 3OH

Ca(OH)2 = 2Ca + 2OH

Test 5

Explanation

Test 5

122. Seawater has a pH of 8.0. What is the hydrogen ion concentration?

2 x 10^-8 mol/L

1 x 10^-8 mol/L

1 x 10^-4 mol/L

8 x 10^-1 mol/L

8.0 mol/L

Test 5

Explanation

Test 5

123. Air Canada air buses fly at altitudes around 10km which is

Near the top of the stratosphere

Near the top of the troposphere

Above the ozone layer

In the mesosphere

In the ozone layer

Test 6

Explanation

Test 6

124. A solution whose precise concentration is known is called a

Standard solution

Traditional solution

Dilute solution

Chemical solution

Concentrated solution

Test 4

Explanation

Test 4

125. A compound containing carbon, hydrogen, and chlorine is composed of 49.0% carbon and 2.74% hydrogen by mass; the remainder is chlorine. The empirical formula of the compound is

CHCl

C3H2Cl

C2H2Cl

C2H3Cl

C2H3Cl2

Test 3

Explanation

Test 3

126. How many moles of KClO3 are needed to form 2.8L of O2, measured at STP, according to the following reaction: 2KClO3 = 2KCl + 3O2

0.083 mol

0.17 mol

0.33 mol

0.25 mol

0.50 mol

Test 6

Explanation

Test 6

127. On which continent are hydrocarbon-based refrigerators not readily available to the mass market?

Europe

Asia

Africa

North America

Australia

Test 6

Explanation

Test 6

128. As the temperature of a solution increases, the solubility of salts ___ and the solubility of gases ___

Doesn't change, doesn't change

Increases, decreases

Increases, increases

Decrease, decreases

Decreases, increases

Test 4

Explanation

Test 4

129. The best explanation why sodium carbonate solutions are alkaline would be

Sodium ions react with water to produce hydroxide ions.

Sodium carbonate is almost the same as sodium hydroxide.

Carbonate ions react with water to produce hydroxide ions.

Sodium carbonate doesn't dissolve very well in water.

Carbonate ions neutralize the hydronium ions in the solution.

Test 5

Explanation

Test 5

130. Consider the following equation: HC2H3O2 + H2O = C2H3O2 + H3O

Which are the conjugate acid-base pairs?

HC2H3O and H2O

HC2H3O2 and C2H3O2

C2H3O2 and H3O

H2O and H3O

B and D only

Test 5

Explanation

Test 5

131. Based on the solubility rules, which of the following is insoluble?

CaCl2

Fe(NO3)3

LiBr

(NH4)2CO3

PbBr2

Test 4

Explanation

Test 4

132. What mass of pure hydrogen peroxide would be dissolved in 250mL of 6.0% W/V H2O2(aq)

12g

25g

6g

15g

2.5g

Test 4

Explanation

Test 4

133. Determine the number of moles of silver that are produced when 210g of silver nitrate are completely reacted as shown in the following reaction: Sn + 2AgNO3 = 2Ag + Sn(NO3)2

1.24mol

1.78mol

2.48mol

3.11mol

4.07mol

Test 3

Explanation

Test 3

134. Why does atomic radius decrease from left to right in a period?

Nuclear charge increases from left to right in a period

Nuclear charge decreases from left to right in a period

The number of energy levels increase from left to right in a period

The number of energy levels decreases from left to right in a period

The number of electrons decreases from left to right in a period

Test 1

Explanation

Test 1

135. The temperature of a gas remains constant while the volume of a given amount of gas is tripled. What will happen to the pressure reading compared to the initial temperature?

No change in pressure will be recorded

The final pressure will be three times that of the initial pressure

The final pressure will be one third greater than the initial pressure

The final pressure will be one third the value of the initial pressure

The final pressure will decrease by one third from the initial pressure

Test 6

Explanation

Test 6

136. The greenhouse effect is caused by

Infrared radiation

Ultraviolet radiation

Water

Carbon dioxide

All of the above

Test 2

Explanation

Test 2

137. Which of the following graphs represent the plot of volume versus temperature (in K) at constant pressure? (Refer to Test for this question)

A

B

C

D

E

Test 6

Explanation

Test 6

138. When diluting concentrated acids, always add

A small acid volume to a larger volume of water

A tiny volume of water to the acid

A large acid volume to a small amount of water

A 50-50 mixture of acid and water

None of the above

Test 4

Explanation

Test 4

139. A gas is collected at 298K and 101kPa and it occupies a volume of 200mL. What volume will the same gas occupy if the pressure is doubled and the temperature is raised to 596K?

50.0 mL

100mL

200mL

400mL

800mL

Test 6

Explanation

Test 6

140. According to Bronsted-Lowry an acid is

A substance that produces hydronium ions

A substance that produces hydroxide ions

A proton acceptor

A proton donor

Really just neutral

Test 5

Explanation

Test 5

141. A mixture of 0.2 mol Ar and 0.25 mol N2 is compressed at 298K from 10.0L to 1.00L. What is the change in pressure?

1114 kPa to 111.4 kPa

111.4 kPa to 1114 kPa

9.35 kPa to 93.5 kPa

93.5 kPa to 9.35 kPa

None of the above

Test 6

Explanation

Test 6

142. Secondary treatment of waste water involves

Distillation

Aeration and chlorination

Filtering

Large expenses

Reverse osmosis

Test 4

Explanation

Test 4

143. An underground formation of permeable rock that produces useful well water is a

Puddle

Reservoir

River

Pond

Aquifer

Test 4

Explanation

Test 4

144. Laughing gas, N2O, and tear gas, NH3, are released at the same time at an equal distance away from you. Particles of laughing gas and tear gas move by simple diffusion and each molecule has the same kinetic energy. The room is perfectly sealed with no prevalent air current. Would you laugh or cry first?

You would laugh first

You would cry first

You would laugh and cry at the same time

You would do neither because the gasses would neutralize each other before reaching you

This is impossible to determine because too many variables are not controlled

Test 6

Explanation

Test 6

145. The mass of a fixed quantity of a gas

Decreases as the density increases

Increases as the density increases

Increases when the volume increases at constant temperature

Decreases when the absolute temperature decreases at constant pressure

Remains at a constant value regardless of the changes in pressure and temperature

Test 6

Explanation

Test 6

146. Why does electron affinity increase from bottom to top in a chemical family?

Nuclear charge increases from bottom to top in a chemical family

Nuclear charge decrease from bottom to top in a chemical family

The number of energy levels increases from bottom to top in a chemical family

The number of energy levels decreases from bottom to top in a chemical family

The number of electrons increases from bottom to top in a chemical family

Test 1

Explanation

Test 1

147. Which measurement has the highest pressure?

3.0 mm Hg

3.0 atm

3.0 kPa

3.0 psi

3.0 tor

Test 6

Explanation

Test 6

148. A 100.0g sample of a compound is composed of 16.3g of carbon, 32.1g of chlorine, and 51.6g of fluorine. The empirical formula of the compound is

CCIF

CCIF3

C2Cl2F6

C3Cl2F6

C9Cl6F18

Test 3

Explanation

Test 3

149. Under conditions of constant temperature and amount of molecules, Boyle's law requires thati) P1V1 = P2V2ii) PV = Constantiii) P1/P2 = V1/V2

I) only

Ii) only

Iii) only

I), ii), and iii)

None of the above

Test 6

Explanation

Test 6

150. A sealed 4.0 L pickle jar is filled with O2 gas by the downward displacement of water. The jar is placed into the refrigerator. What will happen to the O2 gas?

The O2 molecules will move further apart

The gas will liquefy

The O2 molecuels will collide more frequently with the sides of the jar.

The translational motion of the O2 molecules will increase

The kinetic energy of the O2 molecules will be reduced

Test 6

Explanation

Test 6

151. Which of the following combinations of aqueous solutions would produce a precipitate?

Ammonium sulphide and zinc bromide

Potassium chloride and sodium nitrate

Iron(III) nitrate and potassium hydroxide

All of the above

A and C only

Test 4

Explanation

Test 4

152. Which term would best describe 40g of NH4Cl dissolved in 100mL of water at 30 degrees celsius?

Supsersaturated

Insoluble

Unsaturated

Saturated

Subsaturated

Test 4

Explanation

Test 4

153. What volume of water should be added to 500mL of a 1.0mol/L CuSO4 solution to dilute it to 0.5mol/L

500mL

1.0L

250mL

125mL

375mL

Test 4

Explanation

Test 4

154. What pressure would be exerted by a mixture of 1.4g of nitrogen gas and 4.8g of oxygen gas in a 0.2L container at 330K?

4.76 x 10^2 kPa

3.4 x 10^3 kPa

4.8 x 10^3 kPa

2.7 x 10^3 kPa

3.0 kPa

Test 6

Explanation

Test 6

155. Temperature is

The amount of heat in a sample

The average kinetic energy of the sample

The same as the enthalpy of the sample

The sum of the forces of collision with the termometer

All of the above

Test 6

Explanation

Test 6

156. Which of the following are true statements about the change of state from liquid to gas?

The density of the liquid is less than the density of the gas.

The liquid has a higher compressibility than the gas.

The distance between particles increases during evaporation

The chemical composition of the particles changes during evaporation.

None of the above

Test 6

Explanation

Test 6

157. The random motion of gas molecules is a significant part of the explanation for the

Low density of gasses

Transparency of gasses

High compressibility of gasses

Low reactivity of gasses

The reason why gasses always fill their containers over time

Test 6

Explanation

Test 6

158. Avogadro's principle states that at the same temperature and pressure,

All molecules in the gaseous state are the same size.

The volumes occupied by the same number of molecules are the same

The volumes occupied by equal numbers of molecules are proportional to their masses

Equal masses of all gasses contain the same number of molecules

Equal masses of gasses have equal volumes

Test 6

Explanation

Test 6

159. Which of the net ionic equation best represents the reaction between silver nitrate and potassium acetate?

2Ag(aq) + C2H3O2(aq) = AgC2H3O2(s)

Au(aq) + C2H4O2(aq) = AgC2H3O2(s)

Ag(aq) + C2H3O2(AQ) = AgC2H3O2(s)

Ag(aq) + C2H3O2^2-(aq) = AgC2H3O2(S)

Ag(aq) + C2C2H3O2^-(aq) = AgC2H3O2

Test 4

Explanation

Test 4

160. At what temperature does an ideal gas have zero kinetic energy?

0 degrees celsius

273 degrees celsius

273 K

-273 K

-273 degrees celsius

Test 6

Explanation

Test 6