Free Printable C10 Mole Theory Test Review

1.

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)

2.

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)

3.

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)

4.

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)

5.

Use the Periodic Table from class.

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

(a)

6.

Use the Periodic Table from class.

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

(a)

7.

What is the molar mass of oxygen gas?

a)

15.9994 g/mol

b)

31.9988 g/mol

8.

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)

9.

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)

10.

A mole is the SI unit for

a)

mass of a substance

b)

amount of substance

c)

skin pigmentation

d)

length of a substance

11.

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

12.

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

13.

What are the units for molar mass?

a)

amu (atomic mass units)

b)

g (grams)

c)

mol (moles)

d)

g/mol (grams per mole)

14.

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

15.

Mark all that apply.

Which of the following are diatomic elements?

a)

hydrogen

b)

francium

c)

nitrogen

d)

oxygen

e)

chlorine

16.

Mark all that apply.

Which of the following are diatomic elements?

a)

iodine

b)

carbon

c)

bromine

d)

fluorine

e)

helium

17.

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)

18.

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)

19.

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)

20.

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)

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

21.

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)

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

22.

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

23.

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

24.

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

25.

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)

26.

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)

27.

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)

28.

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)

29.

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)

30.

Which type of particles are used for ionic compounds?

a)

atoms

b)

molecules

c)

formula units

31.

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

a)

atoms

b)

molecules

c)

formula units

32.

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

33.

Which type of particles are used for elements?

a)

atoms

b)

molecules

c)

formula units

34.

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

35.

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

36.

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

37.

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

38.

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

39.

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

40.

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

41.

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

(a)

42.

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

(a)

43.

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

Number only. No Units.

(a)

44.

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

Number only. No Units.

(a)

45.

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

(a)

46.

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)

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

47.

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)

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

48.

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

49.

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

50.

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

51.

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

52.

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

(No units. 3 significant figures)

(a)

53.

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

(No units. 3 significant figures)

(a)

54.

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

(No units. 3 significant figures)

(a)

55.

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

56.

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

(a)

57.

The SI unit for the amount of substance.

(a)

58.

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

(a)

59.

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

(a)

60.

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

C10 Mole Theory Test Review

Total questions: 60

Worksheet time: 41mins

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