Free Printable CHem

1.

1. (3 points) Choose the response that includes all the items listed below that are mixtures. i. steel; ii. gasoline; iii. graphite; iv. purified table sugar; v. fat-free milk.

a)

i, iii

b)

i, ii, v

c)

iv only

d)

iii, iv

e)

all of them are mixtures

2.

(3 points) Which of the following is an element?

a)

fire

b)

oxygen

c)

water

d)

air

e)

metal

3.

3. (3 points) Which one of the following represents a chemical change?

a)

condensation of steam

b)

grinding coffee beans into powders

c)

dissolving sugar in water

d)

melting gold

e)

souring of milk

4.

4. (3 points) Rank the following values: (1) 286; (2) 2.21 × 105 ; (3) 3.72 × 10−3 ; (4) 6.20 × 102 .

a)

(3) > (2) > (1) > (4)

b)

(1) > (2) > (4) > (3)

c)

(2) > (4) > (1) > (3)

d)

(3) > (1) > (2) > (4)

e)

(3) > (1) > (4) > (2)

5.

5. (3 points) Identify the extensive properties. i. volume; ii. density; iii. mass; iv. temperature; v. color

a)

i, iii

b)

i, iii, iv

c)

iv only

d)

iii, iv

e)

all of them are not pure

6.

6. (3 points) Convert 36.5 ◦C to the temperature in Fahrenheit.

a)

−36.5 F

b)

2.5 F

c)

97.7 F

d)

309.6 F

e)

236.6 F

7.

7. (3 points) Express the number 0.0000415 in scientific notation.

a)

0.0000415 is already written in scientific notation

b)

4.15 × 10^5

c)

41.5 × 10^4

d)

41.5 × 10^−4

e)

4.15 × 10^−5

8.

8. (3 points) What is the SI based unit for temperature?

a)

Fahrenheit

b)

Celsius

c)

Gram

d)

Kelvin

e)

Liter

9.

9. (3 points) A graduated cylinder initially contains 48.6 mL of water. When the jewelry is submerged in the graduated cylinder, the total volume increases to 61.4 mL. What is the volume of this jewelry?

a)

110.0 mL

b)

48.6 mL

c)

61.4 mL

d)

12.8 mL

e)

38.6 mL

10.

10. (3 points) A piece of wood cubic has an edge length of 6.43 cm. The mass is 130.145 g. What is the density of the wood?

a)

2.04 g/cm^3

b)

0.0494 g/cm^3

c)

20.2 g/cm^3

d)

4.90 × 10^−4 g/cm^3

e)

0.490 g/cm^3

11.

11.(3 points) Which of the following numbers can be treated as an exact number?

a)

There are 5 eggs in a basket.

b)

The mass of a dozen eggs is weighed to be 720 g.

c)

The number of gallons of gasoline needed to fill an automobile gas tank.

d)

The time required to drive from San Francisco to Kansas City at an average speed of 53 mi/h.

e)

The mass of a textbook.

12.

12. (3 points) Which of the following measurements has the most significant figures?

a)

2 × 10^18 m

b)

38.7 g

c)

9.741 50 × 10^−4 J

d)

0.000 140 0 g

e)

17.0 kg

13.

13. (3 points) The conversion factor between g and mg is

a)

1 g = 1 × 10^6 mg

b)

1 g = 1 × 10^3 mg

c)

1 g = 1 × 10^−3 mg

d)

1 g = 1 × 10^−6 mg

e)

1 g = 1 × 10^−9 mg

14.

14. (3 points) Considering the results of the archery contest shown in this figure, which statement is correct?

a)

Archer X is most precise.

b)

Archer X is most accurate.

c)

Archer W is most precise.

d)

Archer Y is not accurate but precise.

e)

Archer Z is not accurate but precise.

15.

15. (3 points) Perform the calculation and report the answer with the correct number of significant figures.

42.7 + 0.259

a)

42.959

b)

42.96

c)

43.0

d)

43

e)

4.3 × 10^1

16.

16. (3 points) The elements in the last column of the periodic table are known as

a)

metalloids

b)

metals

c)

halogen

d)

nonmetals

e)

noble gases

17.

17. (3 points) An anion is defined as

a)

a stable atom.

b)

a group of stable atoms.

c)

an atom or group of atoms with a net positive charge.

d)

a charged atom or group of atoms with a net negative charge.

e)

a metal atom

18.

18. (3 points) What is the number of electrons in the atom ^13 C?

a)

4

b)

5

c)

6

d)

7

e)

13

19.

19. (3 points) Which of the following must be molecular formula rather than empirical formula?

a)

$N_2O_4$

b)

$CH_2O$

c)

$CH_4O$

d)

CH

e)

$NO_2$

20.

20. (3 points) How many protons and electrons are present in one $Na^+$ ion?

a)

11 p, 9 e

b)

11 p, 10 e

c)

11 p, 11 e

d)

10 p, 11 e

e)

10 p, 9 e

21.

21. (3 points) Which is the correct formula for iron(III) sulfate?

a)

$FeSO_4$

b)

$Fe_2SO_4$

c)

$FeSO_3$

d)

$Fe_2(SO_4)_3$

e)

$Fe_2(SO_3)_3$

22.

22. (3 points) The correct name for $HBrO_2$ is

a)

hypobromous acid

b)

bromous acid

c)

bromic acid

d)

hydrobromic acid

e)

hydrogen bromide

23.

23. (3 points) Which of the following is the formula for iron(II) hydroxide?

a)

$FeH_2$

b)

$Fe_2O_3$

c)

$HFeO_3$

d)

$Fe(OH)_2$

e)

$Fe(OH)_3$

24.

24. (3 points) The correct name for $CaCl_2$ · 2 $H_2O$ is

a)

Calcium chlorite hydrate

b)

Calcium chlorite dihydrate

c)

Calcium chloride dihydrate

d)

Calcium hypochlorous acid

e)

Calcium chlorate dihydrate

25.

25. (3 points) For the following pair of ions, write the formula of the compound they will form.

a)

$NH_4SO_4$

b)

$NH_4(SO_4)_2$

c)

$N_2H_8SO_4$

d)

$NH_4S_2O_8$

e)

$(NH_4)_2SO_4$

26.

26. (3 points) What ions can be found in compound $KClO_4$ ?

a)

K+ and Cl– and $O_2$

b)

K + and Cl– and O2 –

c)

K + and $ClO^4$ –

d)

K + and $ClO_4$ –

e)

K + and ClO–

27.

27. (3 points) Using the periodic table, identify the lightest, i.e., smallest mass number, member of alkaline earth metals

a)

Li

b)

H

c)

Be

d)

He

e)

F

28.

28. (3 points) What are α particles which can be found in α radiation?

a)

electrons

b)

He nuclei

c)

photons

d)

protons

e)

neutrons

29.

29. (3 points) Write the symbol of the following ion: the ion with 54 electrons, 53 protons, and 74 neutrons.

a)

^127 v53 I^–

b)

^127 v74 W^–

c)

^74 v53 I^–

d)

^128 v54 Xe^+

e)

^74 v54Xe^+

30.

30. (3 points) Which statement of Dalton’s atomic theory is not accurate from a modern perspective?

a)

Elements are composed of extremely small particles called atoms.

b)

All atoms of a given element are identical, having the same size, mass, and chemical properties.

c)

The atoms of one element are different from the atoms of all other elements.

d)

Compounds are composed of atoms of more than one element. In any compound, the ratio of the numbers of atoms of any two of the elements present is either an integer or a simple fraction.

e)

A chemical reaction involves only the separation, combination, or rearrangement of atoms; it does not result in their creation or destruction.

31.

31. (3 points) What is the mass of 7.98 × $10^{22}$ Mg atoms?

a)

0.133 g

b)

1 g

c)

3.22 g

d)

6.02 × $10^{23}$ g

e)

7.54 g

32.

32. (3 points) When balanced with smallest set of whole numbers, the coefficient of H2 in the following equation is Na + H2O −−→ NaOH + H2

a)

1

b)

2

c)

3

d)

4

e)

5

33.

33. (3 points) What is the mass of 1.33 mol aluminum oxide?

a)

136 g

b)

102 g

c)

57.2 g

d)

6.02 × 10^23 g

e)

8.01 × 10^23 g

34.

34. (3 points) How many atoms are there in 34.15 g Fe?

a)

0.612

b)

1.64

c)

3.68 × 10^23

d)

6.02 × 10^23

e)

9.84 × 10^23

35.

a)

58.4 g

b)

40.1 g

c)

36.5 g

d)

25.0 g

e)

15.6 g

36.

36. (3 points) The mass of three moles of molecular hydrogen (H2) is

a)

1.01 g

b)

2.02 g

c)

3.02 g

d)

4.03 g

e)

6.04 g

37.

37. (3 points) Calculate the molar mass of menthol $C_{12}H_{17}NO$ .

a)

191 g/mol

b)

161 g/mol

c)

31 g/mol

d)

4 g/mol

e)

1 g/mol

38.

38. (3 points) What is the mass of 1.50 moles of $C_{10}H_{20}O$ ?

a)

1.5 g

b)

156 g

c)

234 g

d)

6.02 × $10^{23}$ g

e)

9.03 × $10^{23}$ g

39.

39. (3 points) An organic compound is 38.66% C, 9.73% H, and 51.61% O by mass. What is the empirical formula of this compound?

a)

$CH_8O$

b)

$CH_6O$

c)

$CH_3O$

d)

$C_2H_6O$

e)

$C_3H_6O$

40.

40. (3 points) What is the mass percent of C in organic compound $C_{13}H_{18}O_2$ ?

a)

8.7%

b)

15.5%

c)

39.4%

d)

75.7%

e)

100%

41.

41. (3 points) Identify the major ionic species present in an aqueous solution of $K_2SO_4$

a)

K + , S+ , O2 –

b)

K^+ , SOv4^2 –

c)

Kv2 + , SOv4^2 –

d)

Kv2^+ , S^2 – , Ov4

e)

K^+ , S^6+,

Ov4^2 –

42.

42. (3 points) Based on the solubility rules, which one of the following compounds should be insoluble in water?

a)

$Na_3PO_4$

b)

$(NH_4)_2CO_3$

c)

AgCl

d)

$Ca(NO_3)_2$

e)

$K_2SO_4$

43.

43. (3 points) What is the chemical formula of the salt produced by the neutralization of bromic acid with calcium hydroxide?

a)

$CaBr_2$

b)

CaO

c)

$CaBr_2O$

d)

$Ca(BrO_3)_2$

e)

$Ca_2BrH$

44.

44. (3 points) Which of the following compounds is a weak electrolyte?

a)

$AgNO_3$

b)

NaF

c)

$HClO_3$

d)

$CH_3COOH$

e)

NaCl

45.

45. (3 points) Which of the following compounds is a weak acid?

a)

$HClO_3$

b)

HF

c)

HBr

d)

HCl

e)

$H_2SO_4$

46.

46. (3 points) Which of the following represents the correct net ionic form of the reaction between hydrochloric acid and sodium hydroxide.

a)

Cl– (aq) + Na+ (aq) −−→ NaCl(s)

b)

H + (aq) + OH– (aq) −−→ H2O(l)

c)

H + (aq) + Cl – (aq) + Na+ (aq) + OH– (aq) −−→ NaCl(aq) + H2O(l)

d)

HCl(aq) + NaOH(aq) −−→ H + (aq) + Cl – (aq) + Na+ (aq) + OH– (aq)

e)

HCl(aq) + NaOH(aq) −−→ Na+ (aq) + Cl – (aq) + H2O(l)

47.

47. (3 points) The oxidation number of C in $Na_2C_2O_4$ is

a)

-1

b)

+2

c)

+3

d)

+4

e)

None of above

48.

48. (3 points) Which of the following represents a disproportionation reaction?

a)

2 NaN3(s) −−→ 2 Na(s) + 3 N2(g)

b)

3 NO2(g) + H2O(l) −−→ 2 HNO3(aq) + NO(g)

c)

Fe2O3(s) + 2 Al(s) −−→ 2 Fe(s) + Al2O3(s)

d)

2 P(s) + 3 Cl2(g) −−→ 2 PCl3(g)

e)

. 2 ZnS(s) + 3 O2(g) −−→ 2 ZnO(s) + 2 SO2(g)

49.

49. (3 points) In the following redox reaction

a)

H is oxidized and H is reduced

b)

O is oxidized and O is reduced

c)

N is oxidized and N is reduced

d)

N is oxidized and O is reduced

e)

O is oxidized and N is reduced

50.

50. (3 points) What mass of $Na_2CO_3$ is needed to prepare 100 mL of a solution having a sodium ion concentration of 1.00 M?

a)

14.3 g

b)

28.6 g

c)

106 g

d)

10.6 g

e)

5.30 g

51.

51. (3 points) The pressure of a gas sample was measured to be 0.364 atm. What is an equivalent statement of that pressure?

a)

364 mmHg

b)

760 mmHg

c)

36.9 kPa

d)

101 kPa

e)

1.01 × 10^5 kPa

52.

52. (3 points) Calculate the volume of 1.42 mole ideal gas at 78.6 ◦C and 101 kPa.?

a)

411 L

b)

91.9 L

c)

41.1 L

d)

9.19 L

e)

0.411 L

53.

53. (3 points) A 2.50 L volume of hydrogen measured at −196 ◦C is warmed to 100 ◦C. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.

a)

0.516 L

b)

−1.28 L

c)

1.28 L

d)

4.90 L

e)

12.1 L

54.

54. (3 points) In a container there are 0.468 mol of nitrogen and 0.110 mol of oxygen. The overall pressure is 760 mmHg. Calculate the partial pressure of oxygen.

a)

0.11 atm

b)

0.190 atm

c)

0.810 atm

d)

145 atm

e)

615 atm

55.

55. (3 points) Which one of these gases is ”lighter-than-air” (means lower density)?

a)

$Cl_2$

b)

$SO_2$

c)

$PH_3$

d)

$NO_2$

e)

Ne

56.

56. (3 points) Two moles of chlorine gas at 25 ◦C are heated to 100 ◦C while the volume is not changed. The density of the gas

a)

increase

b)

decrease

c)

remains the same

d)

depends on the pressure

e)

Not enough information is given to correctly answer the question.

57.

57. (3 points) What is the density of dinitrogen monoxide at a temperature of 325 K and a pressure of 113.0 kPa?

a)

186 kg/m3

b)

1.84 kg/m3

c)

1.86 × 10^5 kg/m3

d)

1.84 × 10^5 kg/m3

e)

11.5 kg/m3

58.

58. (3 points) Sometimes leaving a bicycle in the sun on a hot day will cause a blowout. Why?

a)

Sunlight causes chemical reaction of the air in the tire

b)

The bicycle is too old.

c)

The volume of the tire decreases under sunshine.

d)

The pressure of the air in the tire increases at elevated temperatures.

e)

The moles of gas increase at higher temperature

59.

59. (3 points) Which of these properties is not a general characteristic of gases?

a)

Colorless

b)

High compressibility

c)

Relatively large distances between molecules

d)

Formation of homogeneous mixtures regardless of the nature of gases

e)

Under the same pressure and temperature, the density of a gas is correlated with its molar mass

60.

60. (3 points) Which statement is false?

a)

The average speed of molecules from samples of different “ideal” gases is not the same at the same temperature.

b)

The molecules of an ideal gas are relatively far apart.

c)

At the same temperature, two types of ideal gas molecules have the same average kinetic energy regardless their different molar masses.

d)

Molecules of a gas undergo many collisions with each other and the container walls.

e)

Molecules of greater mass have a higher average speed than those of less mass at the same temperature.

61.

61. (3 points) If ∆rxnH−◦ = −54.74 kJ mol−1 for a chemical reaction, which of the following statement is true?

a)

The reaction is endothermic

b)

The reaction is exothermic.

c)

The reaction cannot occur.

d)

The reaction causes an explosion.

e)

The reaction needs a supply of oxygen.

62.

62. (3 points) Which of the following is a state function?

a)

enthalpy

b)

heat

c)

specific heat

d)

mechanical work

e)

electric work

63.

63. (3 points) An endothermic reaction causes the surroundings to

a)

warm up.

b)

become acidic

c)

expand

d)

decrease in temperature

e)

release $CO_2$

64.

64. (3 points) Which of the following processes is endothermic?

a)

C + Ov2 −−→ COv2

b)

H2O(g) −−→ H2O(l)

c)

MgClv2(s) −−→ Mg(s) + Clv2(g)

d)

H2O(l) −−→ H2O(s)

e)

2 C + O2 −−→ 2 CO

65.

65. (3 points) Which of the following processes always results in a decrease in the internal energy of a system?

a)

The system gains heat and has work done on it by the surroundings.

b)

The system loses heat and does work on the surroundings.

c)

The system gains heat and does work on the surroundings.

d)

The system loses heat and has work done on it by the surroundings.

e)

None of these is always true.

66.

66. (3 points) When 18.5 g of HgO(s) is decomposed to form Hg(l) and O2(g), 7.75 kJ of heat is absorbed at standard-state conditions. What is the standard enthalpy of formation (∆fH−◦ ) of HgO(s)?

a)

−90.7 kJ/mol

b)

−7.75 kJ/mol

c)

0.419 kJ/mol

d)

27.9 kJ/mol

e)

181 kJ/mol

67.

67. (3 points) Consider the following data when these two metals are placed in contact, which of the following will take place?

a)

Heat will flow from Al to Cu because Al has a larger specific heat.

b)

Heat will flow from Cu to Al because Cu has a larger mass.

c)

Heat will flow from Cu to Al because Cu has a larger heat capacity.

d)

Heat will flow from Cu to Al because Cu is at a higher temperature.

e)

No heat will flow in either direction.

68.

68. (3 points) At constant pressure, in which of the reactions is work done by the system on the surroundings?

a)

Hg(l) −−→ Hg(g)

b)

3 $O_2$ (g) −−→

$2O_3$ (g)

c)

H2(g) + F2(g) −−→ 2 HF(g)

d)

HCl(aq) + NaOH(aq) −−→ NaCl(aq) + H2O(l)

e)

2 H2(g) + O2(g) −−→ 2 H2O(l)

69.

69. (3 points) Which of the following standard enthalpy of formation values is not zero under standard-state conditions?

a)

Na(s)

b)

Ne(g)

c)

$CH_4$ (g)

d)

$H_2(g)$

e)

Hg(l)

70.

70. (3 points) Which of the statements of heat capacity and specific heat is correct?

a)

heat capacity is the heat required to increase the temperature of one mole of a substance by 1 ◦C.

b)

specific heat is the heat required to increase the temperature of one mole of a substance by 1 ◦C.

c)

heat capacity is the heat required to increase the temperature of 1 g of a substance by 1 ◦C.

d)

mole heat capacity is the heat required to increase the temperature of 1 g of a substance by 1 ◦C.

e)

specific heat is the heat required to increase the temperature of 1 g of a substance by 1 ◦C.

71.

71. (3 points) Knowing the reaction enthalpy of the following two reactions, calculate the standard molar enthalpy of formation for SbCl5(s).

a)

−234 kJ/mol

b)

−394 kJ/mol

c)

214 kJ/mol

d)

394 kJ/mol

e)

−708 kJ/mol

72.

72. (3 points) Given the thermochemical equation

a)

99 kJ/mol

b)

−99 kJ/mol

c)

198 kJ/mol

d)

−198 kJ/mol

e)

396 kJ/mol

73.

13. (3 points) Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. Determine the enthalpy change when 27 g of aluminum is produced by this method. (CO: ∆fH−◦ = −110.5 kJ mol−1 ; Alv2Ov3: ∆fH−◦ = −1669.8 kJ mol−1 )

a)

1338 kJ

b)

669 kJ

c)

334 kJ

d)

310 kJ

e)

1504 kJ

74.

74. (3 points) Given the following thermal reaction equation, what information can you get?

a)

Regardless of the state of the reactants and products, i.e., gas, liquid or solid, the reaction enthalpy is always the same.

b)

Every 5 mol of oxygen consumption would require 907 kJ heat from the surroundings to the system.

c)

Every 5 mol of oxygen consumption would release 907 kJ heat from the system to the surroundings.

d)

The reaction is endothermic.

e)

All statements above are incorrect.

75.

75. (3 points) Which statement is correct?

a)

If a reaction release heat to the surroundings, the enthalpy of reaction has a positive value.

b)

The enthalpy changes of reverse reactions have the same absolute value but different signs (one is positive the other must be negative).

c)

If you multiply both sides of a reaction equation by a factor 2, the value of enthalpy change remains the same.

d)

The enthalpy change of the reaction between hydrogen and oxygen does not depends on the state of the reactants and products (i.e., gas, liquid, solid).

e)

The standard enthalpy of formation of any pure element is 0.

76.

76. (3 points) One photon of which kind of electromagnetic wave of the following has the lowest energy?

a)

infrared

b)

ultrablue

c)

microwave

d)

x-ray

e)

visible light

77.

77. (3 points) Calculate the frequency of visible light having a wavelength of 486 nm

a)

6.17 × 10^14 s ^−1

b)

2.06 × 10^14 s ^−1

c)

2.06 × 10^6 s ^−1

d)

4.86 × 10^−7 s^−1

e)

1.20 × 10^−15 s^−1

78.

78. (3 points) What is the energy of a mole of photons associated with visible light of wavelength 486 nm?

a)

2.46 × 10^5 J

b)

1.24 × 10^4 J

c)

2.46 × 10^−4 J

d)

6.46 × 10^−16 J

e)

6.46 × 10^−25 J

79.

79. (3 points) Calculate the energy required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level.

a)

2.07 × 10^−32 kJ

b)

2.25 × 10^−21 kJ

c)

2.04 × 10^−21 kJ

d)

3.27 × 10^−20 kJ

e)

2.19 × 10^2 kJ

80.

80. (3 points) Calculate the wavelength of a neutron that has a velocity of 250 m/s. (The mass of a neutron = 1.675 × 10^−24 g)

a)

1.0 × 10^−4 m

b)

1.6 × 10^−7 m

c)

1.6 × 10^−9 m

d)

1.6 × 10^−11 m

e)

1.6 × 10^−10 m

81.

81. (3 points) Which one of the following sets of quantum numbers is not possible?

a)

n = 4, l = 3, ml = −2, ms = +1/2

b)

n = 4, l = 1, ml = 1, ms = −1/2

c)

n = 3, l = 1, ml = 1, ms = +1/2

d)

n = 2, l = 2, ml = −2, ms = −1/2

e)

n = 2, l = 0, ml = 0, ms = +1/2

82.

82. (3 points) What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 4, l = 3, ml = −2, ms = −1/2

a)

0

b)

1

c)

2

d)

6

e)

10

83.

83. (3 points) Electrons in an orbital with l = 2 are in a/an

a)

p orbital

b)

d orbital

c)

s orbital

d)

g orbital

e)

f orbital

84.

84. (3 points) The number of orbitals in a d subshell is

a)

1

b)

2

c)

5

d)

3

e)

7

85.

85. (3 points) The orbital diagram for a ground-state oxygen atom is

a)

1s ↑↓ 2s ↑ 2p ↑ ↑ ↑

b)

1s ↑↓ 2s ↑↓ 2p ↑↓ ↑↓--

c)

1s ↑↓ 2s ↑↓ 2p ↑↓ ↑ ↑

d)

1s ↑↓ 2s ↑↓ 2p ↑ ↑ ↑

e)

1s ↑↓ 2s ↑↓ 2p ↑↓ ↑↓ ↑

86.

86. (3 points) The electron configuration of a ground-state Na atom is

a)

1s^1

b)

1s^2 2s^1

c)

1s^2 2s^2 3s^1

d)

1s^2 2s^2 2p^3 3s^1

e)

1s^2 2s^2 2p^6 3s^1

87.

87. (3 points) An electron in an atom is in the n = 3 quantum level. Choose the possible values of l and ml that it can have.

a)

l = 2 ml = 2

b)

l = 3 ml = 3

c)

l = 1 ml = 2

d)

l = 0 ml = −1

e)

l = 3 ml = 0

88.

88. (3 points) Which orbital is the highest in energy in a many-electron atom?

a)

2p

b)

3s

c)

3p

d)

3d

e)

4s

89.

89. (3 points) How many electrons could be held in the second shell of an atom?

a)

2

b)

4

c)

6

d)

8

e)

10

90.

90. (3 points) The number of orbitals in an s subshell is

a)

1

b)

3

c)

4

d)

5

e)

6

CHem

Total questions: 90

Worksheet time: 45mins

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