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HC06 Avogadro's Number Conversions

Total questions: 66

Worksheet time: 45mins

Name
Class
Date
1.

Which type of particles are used for ionic compounds?

a)

atoms

b)

molecules

c)

formula units

2.

Which type of particles are used for elements?

a)

atoms

b)

molecules

c)

formula units

3.

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

a)

atoms

b)

molecules

c)

formula units

4.

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

a)

atoms

b)

molecules

c)

formula units

5.

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

a)

atoms

b)

molecules

c)

formula units

6.

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

7.

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

8.

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

9.

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

10.

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

11.

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

NA

b)

Molar mass

c)

"Subscripts" of the chemical formula

12.

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

NA

b)

Molar mass

c)

Subscripts of the chemical formula

13.

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

NA

b)

Molar mass

c)

Subscripts of the chemical formula

14.

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

NA

b)

Molar mass

c)

Subscripts of the chemical formula

15.

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

NA

b)

Molar mass

c)

Subscripts of the chemical formula

16.

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

NA

b)

Molar mass

c)

Subscripts of the chemical formula

17.

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

(a)  

18.

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

(a)  

19.

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

Number only. No Units.

(a)  

20.

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

Number only. No Units.

(a)  

21.

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

(a)  

22.

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

Number only. No Units.

(a)  

23.

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

(a)  

24.

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

a)

1.22×1025 molecules CCl41 mol CCl46.022×1023 molecules CCl4\frac{1.22\times10^{25}\ molecules\ CCl_4}{ }\frac{1\ mol\ CCl_4}{6.022\times10^{23}\ molecules\ CCl_4}  

b)

1.22×1025 molecules CCl46.022×1023 mol CCl41 molecule CCl4\frac{1.22\times10^{25}\ molecules\ CCl_4}{ }\frac{6.022\times10^{23}\ mol\ CCl_4}{1\ molecule\ CCl_4}  

25.

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

a)

3.55 mol  CCl41 molecule CCl46.022×1023 mol CCl4\frac{3.55\ mol\ \ CCl_4}{ }\frac{1\ molecule\ CCl_4}{6.022\times10^{23}\ mol\ CCl_4}  

b)

3.55 mol CCl46.022×1023 molecules CCl41 mol CCl4\frac{3.55\ mol\ CCl_4}{ }\frac{6.022\times10^{23}\ molecules\ CCl_4}{1\ mol\ CCl_4}  

26.

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

27.

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

28.

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

29.

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

30.

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

31.

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

32.

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

33.

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

34.

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

35.

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

36.

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

(No units. 3 significant figures)

(a)  

37.

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

(No units. 3 significant figures)

(a)  

38.

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

(No units. 3 significant figures)

(a)  

39.

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

(No units. 3 significant figures)

(a)  

40.

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

(No units. 3 significant figures)

(a)  

41.

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

(No units. 3 significant figures)

(a)  

42.

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

(No units. 3 significant figures)

(a)  

43.

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

(No units. 3 significant figures)

(a)  

44.

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

(No units. 3 significant figures)

(a)  

45.

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

(No units. 3 significant figures)

(a)  

46.

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

47.

What is Avogadro's number?

a)

6.022×10236.022\times10^{23}  

b)

6.022×10226.022\times10^{22}  

c)

6.22×10246.22\times10^{24}  

d)

6.022×10246.022\times10^{24}  

e)

6.22×10236.22\times10^{23}  

48.

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

(a)  

49.

The SI unit for the amount of substance.

(a)  

50.

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

(a)  

51.

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

(a)  

52.

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

(a)  

53.

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

(a)  

54.

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
55.

Fill in the blank:

1 mol S = 6.022 x 1023 (a)   S

56.

Fill in the blank:

1 mol K = 6.022 x 1023 (a)   K

57.

Fill in the blank:

1 mol KCl = 6.022 x 1023 (a)   KCl

58.

Fill in the blank:

1 mol NaClO = 6.022 x 1023 (a)   NaClO

59.

Fill in the blank:

1 mol ClO2 = 6.022 x 1023 (a)   ClO2

60.

Fill in the blank:

1 mol C3H6 = 6.022 x 1023 (a)   C3H6

61.

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

(a)   mol C

62.

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

(a)   mol C

63.

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

(a)   mol O

64.

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

(a)   mol H

65.

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

(a)   mol H

66.

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

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