Free Printable CH07a Mole Theory Test Review Sans %M and Empirical formula

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Worksheets

CH07a Mole Theory Test Review Sans %M and Empirical formula

Total questions: 147

Worksheet time: 2hrs 45mins

Name

Class

Date

1.

To convert from moles to grams, you should multiply by ....

a)

b)

c)

d)

2.

To convert from grams to moles, you should multiply by ....

a)

b)

c)

d)

3.

0.50 moles of carbon (C) is equal to how many grams?

a)

6.0 grams

b)

12.0 grams

c)

8.0 grams

d)

14.0 grams

4.

36 g of beryllium (Be) contains how many moles?

a)

0.25 mol

b)

4.0 mol

c)

45 mol

d)

320 mol

5.

What is the mass of 2.50 mol of oxygen gas (O₂)?

a)

40.0 g

b)

80.0 g

c)

16.0 g

d)

32.0 g

6.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 20.0 g sample of XY?

(3 significant figures, include units)

(a)

7.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 5.00 g sample of XY?

(3 significant figures, include units)

(a)

8.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 4.00 g sample of XY?

(3 significant figures, include units)

(a)

9.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 3.00 g sample of XY?

(3 significant figures, include units)

(a)

10.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 2.00 g sample of XY?

(3 significant figures, include units)

(a)

11.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 2.50 g sample of XY?

(3 significant figures, include units)

(a)

12.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 2.20 g sample of XY?

(3 significant figures, include units)

(a)

13.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 2.44 g sample of XY?

(3 significant figures, include units)

(a)

14.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 7.11 g sample of XY?

(3 significant figures, include units)

(a)

15.

Compound XY has a molar mass of 10.0 g/mol.

How many moles are in a 5.82 g sample of XY?

(3 significant figures, include units)

(a)

16.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 1.78 mol sample of XY?

(3 significant figures, include units)

(a)

17.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 2.00 mol sample of XY?

(3 significant figures, include units)

(a)

18.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 3.00 mol sample of XY?

(3 significant figures, include units)

(a)

19.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 4.00 mol sample of XY?

(3 significant figures, include units)

(a)

20.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 8.00 mol sample of XY?

(3 significant figures, include units)

(a)

21.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 5.00 mol sample of XY?

(3 significant figures, include units)

(a)

22.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 0.123 mol sample of XY?

(3 significant figures, include units)

(a)

23.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 0.681 mol sample of XY?

(3 significant figures, include units)

(a)

24.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 1.09 mol sample of XY?

(3 significant figures, include units)

(a)

25.

Compound XY has a molar mass of 10.0 g/mol.

What is the mass of a 1.22 mol sample of XY?

(3 significant figures, include units)

(a)

26.

What is the correct dimensional analysis for calculating the mass of 4.32 mol O₂?

a)

$\ \frac{4.32\ mol\ O_2}{ }\frac{31.9988\ g\ O_2}{1\ mol\ O_2}$

b)

$\ \frac{4.32\ mol\ O_2}{ }\frac{1\ g\ O_2}{31.9988\ mol\ O_2}$

27.

What is the correct dimensional analysis for calculating the number of moles in 4.32 g O₂?

a)

$\frac{4.32\ g\ O_2}{ }\ \frac{1\ mol\ O_2}{31.9988\ g\ O_2}=$

b)

$\frac{4.32\ g\ O_2}{ }\ \frac{31.9988\ mol\ O_2}{1\ g\ O_2}=$

28.

In the problem, "Calculate the number of atoms of C that are in 2.00 g C." what mole conversion factors would be used? (mark all that apply)

a)

Avogadro's number

b)

molar mass

c)

"subscripts"

d)

molar volume

29.

In the problem, "Calculate the number of moles of C that are in 2.00 g C." what mole conversion factors would be used? (mark all that apply)

a)

Avogadro's number

b)

molar mass

c)

"subscripts"

d)

molar volume

30.

In the problem, "Calculate the mass of 2.00 mol C." what mole conversion factors would be used? (mark all that apply)

a)

Avogadro's number

b)

molar mass

c)

"subscripts"

d)

molar volume

31.

Which type of particles are used for ionic compounds?

a)

atoms

b)

molecules

c)

formula units

32.

Which type of particles are used for elements?

a)

atoms

b)

molecules

c)

formula units

33.

Which type of particles are used for covalent (molecular) compounds?

a)

atoms

b)

molecules

c)

formula units

34.

Which type of particles are used for compounds that contain only nonmetals?

a)

atoms

b)

molecules

c)

formula units

35.

Which type of particles are used for compounds that contain a metal or NH₄?

a)

atoms

b)

molecules

c)

formula units

36.

How many moles of chlorine are in exactly 1 mol of P₂Cl₅

a)

2 atoms

b)

5 atoms

c)

2 moles

d)

5 moles

e)

6.022 x 10²³ moles

37.

How many moles of phosphorus are in exactly 1 mol of P₂Cl₅

a)

2 atoms

b)

5 atoms

c)

2 moles

d)

5 moles

e)

6.022 x 10²³ moles

38.

How many atoms of phosphorus are in exactly 1 molecule of P₂Cl₅

a)

2 atoms

b)

5 atoms

c)

2 moles

d)

5 moles

e)

6.022 x 10²³ molecules

39.

How many atoms of chlorine are in exactly 1 molecule of P₂Cl₅

a)

2 atoms

b)

5 atoms

c)

2 moles

d)

5 moles

e)

6.022 x 10²³ molecules

40.

How many molecules of diphosphorus pentachloride are in exactly 1 mole of P₂Cl₅?

a)

2 atoms

b)

5 atoms

c)

2 moles

d)

5 moles

e)

6.022 x 10²³ molecules

41.

What would be used to solve the following problem - "How many moles of magnesium are in 5.6x10⁴⁴ atoms of magnesium?" Mark all that apply

a)

Avogadro's number

N_A

b)

Molar mass

c)

"Subscripts" of the chemical formula

42.

What would be used to solve the following problem - "How many moles of chlorine, Cl, are in 2.16x10²⁴ molecules of magnesium chloride, MgCl₂?" Mark all that apply

a)

Avogadro's number

N_A

b)

Molar mass

c)

Subscripts of the chemical formula

43.

What would be used to solve the following problem - "How many atoms of chlorine, Cl, are in 3.7x10²⁵ molecules of magnesium chloride, MgCl₂?" Mark all that apply

a)

Avogadro's number

N_A

b)

Molar mass

c)

Subscripts of the chemical formula

44.

What would be used to solve the following problem - "How many moles of chlorine, Cl, are in 1.54 moles of magnesium chloride, MgCl₂?" Mark all that apply

a)

Avogadro's number

N_A

b)

Molar mass

c)

Subscripts of the chemical formula

45.

What would be used to solve the following problem - "How many atoms of chlorine, Cl, are in 2.99 moles of magnesium chloride, MgCl₂?" Mark all that apply

a)

Avogadro's number

N_A

b)

Molar mass

c)

Subscripts of the chemical formula

46.

What would be used to solve the following problem - "How many molecules of magnesium chloride, MgCl₂, are in 2.99 moles of magnesium chloride, MgCl₂?" Mark all that apply

a)

Avogadro's number

N_A

b)

Molar mass

c)

Subscripts of the chemical formula

47.

A sample contains 1.1 mol ethane (C₂H₆) how many moles of carbon does it contain? (enter the number only)

(a)

48.

A sample contains 1.1 mol ethane (C₂H₆) how many moles of hydrogen does it contain? (enter the number only)

(a)

49.

How many phosphate ions are in 11 formula units of calcium phosphate, Ca₃(PO₄)₂?

Number only. No Units.

(a)

50.

How many calcium ions are in 11 formula units of calcium phosphate, Ca₃(PO₄)₂?

Number only. No Units.

(a)

51.

How many ions in total are in 11 formula units of calcium phosphate, Ca₃(PO₄)₂

(a)

52.

How many phosphorus atoms are in 11 formula units of calcium phosphate, Ca₃(PO₄)₂?

Number only. No Units.

(a)

53.

How many oxygen atoms are in 11 formula units of calcium phosphate, Ca₃(PO₄)₂? Number only. No Units.

(a)

54.

What is the correct dimensional analysis for "How many moles of carbon tetrachloride are in 1.22x10²⁵ molecules of CCl₄?"

a)

$\frac{1.22\times10^{25}\ molecules\ CCl_4}{ }\frac{1\ mol\ CCl_4}{6.022\times10^{23}\ molecules\ CCl_4}$

b)

$\frac{1.22\times10^{25}\ molecules\ CCl_4}{ }\frac{6.022\times10^{23}\ mol\ CCl_4}{1\ molecule\ CCl_4}$

55.

What is the correct dimensional analysis for "How many molecules of carbon tetrachloride are in 3.15 mol of CCl₄?"

a)

$\frac{3.55\ mol\ \ CCl_4}{ }\frac{1\ molecule\ CCl_4}{6.022\times10^{23}\ mol\ CCl_4}$

b)

$\frac{3.55\ mol\ CCl_4}{ }\frac{6.022\times10^{23}\ molecules\ CCl_4}{1\ mol\ CCl_4}$

56.

How many atoms of S are in 0.250 mol S

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

57.

How many atoms of S are in 0.500 mol S

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

58.

How many atoms of S are in 1.50 mol S

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

59.

How many atoms of S are in 2.00 mol S

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

60.

How many atoms of S are in 1.00 mol SO₂

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

61.

How many atoms of O are in 1.00 mol SO₂

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

62.

How many atoms of O are in 0.500 mol SO₂

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

63.

How many atoms of S are in 0.500 mol SO₂

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

64.

How many atoms of S are in 0.250 mol SO₂

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

65.

How many atoms of O are in 0.250 mol SO₂

a)

1.506 x 10²³ S atoms

b)

3.011 x 10²³ S atoms

c)

9.033 x 10²³ S atoms

d)

6.022 x 10²³ S atoms

e)

1.204 x 10²⁴ S atoms

66.

How many moles of BaCl₂ are in 3.45 x 10²⁴ formula units of BaCl₂?

(No units. 3 significant figures)

(a)

67.

How many moles of Cl are in 1.23 x 10²⁴ formula units of BaCl₂?

(No units. 3 significant figures)

(a)

68.

How many moles of Na₂SO₄ are in 7.89 x 10²³ formula units of Na₂SO₄?

(No units. 3 significant figures)

(a)

69.

How many moles of Na are in 6.78 x 10²³ formula units of Na₂SO₄?

(No units. 3 significant figures)

(a)

70.

How many moles of S are in 6.78 x 10²³ formula units of Na₂SO₄?

(No units. 3 significant figures)

(a)

71.

How many moles of O are in 6.78 x 10²³ formula units of Na₂SO₄?

(No units. 3 significant figures)

(a)

72.

How many moles of C₂H₆ are in 2.11 x 10²⁴ molecules of C₂H₆?

(No units. 3 significant figures)

(a)

73.

How many moles of C are in 2.11 x 10²⁴ molecules of C₂H₆?

(No units. 3 significant figures)

(a)

74.

How many moles of H are in 1.05 x 10²³ molecules of C₂H₆?

(No units. 3 significant figures)

(a)

75.

How many moles of C₂H₆ are in 1.05 x 10²³ molecules of C₂H₆?

(No units. 3 significant figures)

(a)

76.

How are you supposed to put Avogadro's number in a TI85 calculator?

a)

6.022x10E23

b)

6.022*10^23

c)

6.022*e23

d)

6.022*E23

e)

6.022E23

77.

What is Avogadro's number?

a)

$6.022\times10^{23}$

b)

$6.022\times10^{22}$

c)

$6.22\times10^{24}$

d)

$6.022\times10^{24}$

e)

$6.22\times10^{23}$

78.

Which isotope is used for the definition of the mole and the amu? Record your answer using hyphen notation.

(a)

79.

The SI unit for the amount of substance.

(a)

80.

The amount of substance that contains the same number of entities (particles) as there are atoms in exactly 12 grams of carbon-12.

(a)

81.

The amount of substance that will contain 6.022 x 10²³ particles of that substance.

(a)

82.

What exact mass of carbon-12 will contain a mole of carbon-12 atoms?

(a)

83.

What exact mass of carbon-12 will contain 6.022x10²³ carbon-12 atoms?

(a)

84.

1 mol CO = 6.022 x 10²³ (a) CO

1 mol Mg = 6.022 x 10²³ (b) Mg

1 mol LiBr = 6.022 x 10²³ (c) LiBr

Choose from the below words

molecules

atoms

formula units

ions

elements

compounds

particles

85.

Fill in the blank:

1 mol S = 6.022 x 10²³ (a) S

86.

Fill in the blank:

1 mol K = 6.022 x 10²³ (a) K

87.

Fill in the blank:

1 mol KCl = 6.022 x 10²³ (a) KCl

88.

Fill in the blank:

1 mol NaClO = 6.022 x 10²³ (a) NaClO

89.

Fill in the blank:

1 mol ClO₂ = 6.022 x 10²³ (a) ClO₂

90.

Fill in the blank:

1 mol C₃H₆ = 6.022 x 10²³ (a) C₃H₆

91.

How many moles of carbon are in 2 mol of C₄H₁₀?

(a) mol C

92.

How many moles of carbon are in 0.5 mol of C₆H₁₄?

(a) mol C

93.

How many moles of oxygen are in 5 mol of C₆H₁₃OH?

(a) mol O

94.

How many moles of hydrogen are in 0.5 mol of C₄H₁₀?

(a) mol H

95.

How many moles of hydrogen are in 0.5 mol of C₆H₁₄?

(a) mol H

96.

Complete the following

6.022 x 10²³ atoms Sr = (a)

6.022 x 10²³ molecules CO₂ = (b)

6.022 x 10²³ FU Fe₂(CO₃)₃ = (c)

Choose from the below words

1 mol Sr

1 mol carbon dioxide

1 mol Iron (III) carbonate

6.022 mol Sr

0.5 mol CO

6.022 mol Iron (III) carbonate

97.

Element X has a molar mass of 10.01 g/mol and element Y has a molar mass of 5.05 g/mol.

What is the molar mass of the compound,

XY?

(include units of g/mol in the answer)

(a)

98.

Element X has a molar mass of 10.01 g/mol and element Y has a molar mass of 5.05 g/mol.

What is the molar mass of the compound,

X₂Y?

(include units of g/mol in the answer)

(a)

99.

Element X: MM_X= 10.01 g/mol

Element Y: MM_Y = 5.05 g/mol.

What is the molar mass of the compound,

XY₂?

(include units of g/mol in the answer)

(a)

100.

Element X: MM_X= 10.01 g/mol

Element Y: MM_Y = 5.05 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

XYW₂?

(include units of g/mol in the answer)

(a)

101.

Element X: MM_X= 10.01 g/mol

Element Y: MM_Y = 5.05 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

X(YW₃)₂?

(include units in the answer)

(a)

102.

Element X: MM_X= 10.01 g/mol

Element Y: MM_Y = 5.05 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

(XY₄)₂W?

(include units in the answer)

(a)

103.

Use the Periodic Table from class.

What is the molar mass of the element, oxygen (O)? (include units)

(a)

104.

Use the Periodic Table from class.

What is the molar mass of the element, hydrogen (H)? (include units)

(a)

105.

Use the Periodic Table from class.

What is the molar mass of the element, carbon (C)? (include units)

(a)

106.

Use the Periodic Table from class.

What is the molar mass of the element, sulfur (S)? (include units)

(a)

107.

Which hydrocarbon has a molar mass of 30.070 g/mol?

a)

C₂H₄

b)

C₂H₆

c)

C₃H₆

d)

C₃H₈

e)

C₃H₄

108.

Which hydrocarbon has a molar mass of 28.054 g/mol?

a)

C₂H₄

b)

C₂H₆

c)

C₃H₆

d)

C₃H₈

e)

C₃H₄

109.

Which hydrocarbon has a molar mass of 40.065 g/mol?

a)

C₂H₄

b)

C₂H₆

c)

C₃H₆

d)

C₃H₈

e)

C₃H₄

110.

Which hydrocarbon has a molar mass of 42.081 g/mol?

a)

C₂H₄

b)

C₂H₆

c)

C₃H₆

d)

C₃H₈

e)

C₃H₄

111.

Which hydrocarbon has a molar mass of 44.097 g/mol?

a)

C₂H₄

b)

C₂H₆

c)

C₃H₆

d)

C₃H₈

e)

C₃H₄

112.

What is the molar mass of oxygen gas?

a)

15.9994 g/mol

b)

31.9988 g/mol

113.

What is the molar mass of hydrogen gas?

a)

1.00794 g/mol

b)

2.01588 g/mol

114.

What is the molar mass of nitrogen gas?

a)

14.00674 g/mol

b)

28.01348 g/mol

115.

What is the molar mass of neon gas?

a)

20.1797 g/mol

b)

40.3595 g/mol

116.

What is the molar mass of helium gas?

a)

4.003 g/mol

b)

8.006 g/mol

117.

What is the molar mass of chlorine gas?

a)

35.4527 g/mol

b)

70.9054 g/mol

118.

What is the molar mass of krypton gas?

a)

83.80 g/mol

b)

167.60 g/mol

119.

Use the provided molar masses:

MM_C = 12.0 g/mol

MM_O = 16.0 g/mol

MM_H = 1.0 g/mol

What is the molar mass of carbon monoxide?

$CO$

Be sure to include units and correct number of significant figures.

(a)

120.

Use the provided molar masses:

MM_C = 12.0 g/mol

MM_O = 16.0 g/mol

MM_H = 1.0 g/mol

What is the molar mass of carbon dioxide

$CO_2$

Be sure to include units and correct number of significant figures.

(a)

121.

Use the provided molar masses:

MM_C = 12.0 g/mol

MM_O = 16.0 g/mol

MM_H = 1.0 g/mol

What is the molar mass of the carbonate ion?

$CO_3^{\ \ \ \ 2-}$

Be sure to include units and correct number of significant figures.

(a)

122.

Use the provided molar masses:

MM_C = 12.0 g/mol

MM_O = 16.0 g/mol

MM_H = 1.0 g/mol

What is the molar mass of the bicarbonate ion?

$HCO_3^{\ \ \ \ -}$

Be sure to include units and correct number of significant figures.

(a)

123.

Use the provided molar masses:

MM_C = 12.0 g/mol

MM_O = 16.0 g/mol

MM_H = 1.0 g/mol

What is the molar mass of the oxalate ion?

$C_2O_4^{\ \ \ \ 2-}$

Be sure to include units and correct number of significant figures.

(a)

124.

Use the provided molar masses:

MM_C = 12.0 g/mol

MM_O = 16.0 g/mol

MM_H = 1.0 g/mol

What is the molar mass of the acetate ion?

$C_2H_3O_2^{\ \ \ \ -}$

Be sure to include units and correct number of significant figures.

(a)

125.

Use the provided molar masses:

MM_C = 12.0 g/mol

MM_O = 16.0 g/mol

MM_H = 1.0 g/mol

What is the molar mass of methanol?

$CH_3OH$

Be sure to include units and correct number of significant figures.

(a)

126.

A mole is the SI unit for

a)

mass of a substance

b)

amount of substance

c)

skin pigmentation

d)

length of a substance

127.

What is the mass of one mole of a substance called?

a)

Avogadro's Mass

b)

Molar Mass

c)

Molal Mass

d)

Molex Mass

e)

Avocado's Mass

128.

What is the molar mass of an element equal to?

a)

the element's average atomic mass in units of grams per mole.

b)

the sum of the average atomic masses of all the atoms in the formula in units of grams per mole

c)

Mass ÷ Avogadro's number

d)

Mass × Avogadro's number

129.

What are the units for molar mass?

a)

amu (atomic mass units)

b)

g (grams)

c)

mol (moles)

d)

g/mol (grams per mole)

130.

What is the molar mass of a compound equal to?

a)

the element's average atomic mass in units of grams per mole.

b)

the sum of the average atomic masses of all the atoms in the formula in units of grams per mole

c)

Mass ÷ Avogadro's number

d)

Mass × Avogadro's number

131.

What is the approximate molar mass of the following?

sodium peroxide, Na₂O₂

a)

78 g/mol

b)

39 g/mol

c)

54 g/mol

d)

27 g/mol

132.

What is the approximate molar mass of the following?

calcium phosphate, Ca₃(PO₄)₂

a)

310 g/mol

b)

496 g/mol

c)

430 g/mol

d)

87 g/mol

133.

How do you calculate the molar mass of lithium sulfide, Li₂S?

a)

Atomic mass of lithium added to the atomic mass of sulfur

b)

(atomic mass of lithium x 2) added to the atomic mass of sulfur

c)

atomic mass of lithium added to the (atomic mass of sulfur x 2)

d)

(atomic mass of lithium ÷ 2) added to atomic mass of sulfur

134.

Mark all that apply.

Which of the following are diatomic elements?

a)

hydrogen

b)

francium

c)

nitrogen

d)

oxygen

e)

chlorine

135.

Mark all that apply.

Which of the following are diatomic elements?

a)

iodine

b)

carbon

c)

bromine

d)

fluorine

e)

helium

136.

What is the molar mass of table salt (NaCl)?

a)

116.886 g/mol

b)

35.453 g/mol

c)

22.990 g/mol

d)

58.443 g/mol

137.

The molar mass of an element is equal to its...

a)

Atomic mass

b)

Atomic number

c)

Oxidation number

d)

Valence electrons

138.

What is the Molar Mass of Potassium Sulfide?..... :-) You get to figure out the formula.

a)

110.262 g/mol

b)

71.164 g/mol

c)

174.258 g/mol

d)

158.259 g/mol

139.

What is the mass of one mole of aluminum chloride (remember to determine the correct formula first)?

a)

62.435g

b)

116.399g

c)

133.341g

d)

97.888g

140.

What is the molar mass of sodium hydroxide (remember to determine the correct formula first)?

a)

39.997 g/mol

b)

38.989 g/mol

c)

23.998 g/mol

d)

57.004 g/mol

e)

77.978 g/mol

141.

Element X: MM_X= 10.01 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

X₂W?

(include units in the answer)

(a)

142.

Element X: MM_X= 10.01 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

X₃W?

(include units in the answer)

(a)

143.

Element X: MM_X= 10.01 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

XW₂?

(include units in the answer)

(a)

144.

Element X: MM_X= 10.01 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

X₃W₂?

(include units in the answer)

(a)

145.

Element X: MM_X= 10.01 g/mol

Element W: MM_W = 3.03 g/mol

What is the molar mass of the compound,

X₂W₃?

(include units in the answer)

(a)

146.

How would the following molar mass of water be written as a conversions factor?

18.02 g/mol

a)

1 g = 18.02 mol

b)

1 mol = 18.02 g

c)

1 g = 1 mol

d)

18.02 g = 18.02 mol

147.

How would the following molar mass of sodium chloride be written as a conversions factor?

58.44 g/mol

a)

1 g = 58.44 mol

b)

1 mol = 58.44 g

c)

1 g = 1 mol

d)

58.44 g = 58.44 mol

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