Category: Chemistry

Set 6 – Moles & Reacting Masses from Equations

1

1 / 12

What mass of oxygen is required for complete combustion of 1 tonne of methane?

2 / 12

What mass of zinc will displace 5.4g of silver from silver nitrate solution?

3 / 12

What mass of

CO2

could be obtained by heating 5g of calcium carbonate?

4 / 12

Given this equation,

2Al+Fe2O3=>Al2O3+2Fe

what mass of aluminium would react completely with 320g of iron (lll) oxide?

5 / 12

Given this equation,

4Na+ O2=>2Na2O

what mass of O2 is required to react with 23g of sodium?

6 / 12

Given this equation,

2CO+O2=>2CO2

what mass of CO will react with 32g of oxygen?

7 / 12

Given this equation,

Zn+S=>ZnS

what mass of zinc will combine with 32g of sulphur?

8 / 12

Balance this equation:

P4+O2=>P4O10

Using the balanced equation, how many moles of oxygen molecules are required to react with 1 mole of phosphorous molecules?

9 / 12

Balance this equation:

K+S=>K2S

Using the balanced equation, how many moles of potassium atoms are required to react with 1 mole of sulphur atoms?

10 / 12

How many moles of NO2 can be made by full decomposition of 1 mole of Pb(NO3)2 if the equation for this reaction is:

2Pb(NO3)2 => 2PbO + 4NO2 + O2

11 / 12

The correctly balanced form of the equation

Al + Cl2=>AlCl3

is:

12 / 12

Given the equation,

3NaOH +H3PO4 =>Na3PO4+3H2O

How many moles of NaOH are required to react with 1 mole of H3PO4?

 

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Set 5 – Balancing Equations

2

Moles Set 5 - Balancing Equations

1 / 14

Cu + HNO3 => Cu(NO3)2 + NO + H2O

2 / 14

NH3 + O2 => NO + H2O

3 / 14

C4H10 + O2 => CO2 + H2O

4 / 14

KClO3 => KClO4 + KCl

5 / 14

Br2 + KOH => KBrO3 + KBr + H2O

6 / 14

Na2O2 + H2O => NaOH + O2

7 / 14

MnO2 + HCl => MnCl2 + H2O + Cl2

8 / 14

P4O10+ H2O => H3PO4

9 / 14

(NH4)2SO4 + NaOH => Na2SO4 + NH3 + H2O

10 / 14

NaHCO3 => Na2CO3 + CO2 + H2O

11 / 14

K + Cl2 = KCl

12 / 14

Mg + N2 => Mg3N2

13 / 14

ZnS + O2 = >ZnO + SO2

14 / 14

Fe + H2O => Fe3O4 + H2

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Set 4 – Moles from Compounds

0

Moles Set 4 - Moles of Compounds

1 / 10

How many moles of HNO3 are contained in 189g of the compound?

2 / 10

How many moles of CO2 are contained in 33.0g of the compound?

3 / 10

The mass of 0.500 moles of iron (II) sulphide is:

4 / 10

The mass of 2.00 moles of lead (II) nitrate is:

5 / 10

The mass of 0.250 moles of LiOH is:

6 / 10

The mass of 3.00 moles of Na2CO3 is:

7 / 10

The mass of 1.00 mole of KCN is

8 / 10

The mass of 1.00 mole of MgSO4 is:

9 / 10

The formula mass of (NH4)2SO4 is:

10 / 10

The formula mass of KNO3 is:

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Set 3 – Formulae

0

Moles Set 3 - Formulae

1 / 40

A compound with empirical formula CH2 has a relative molecular mass of 84. Which of the following is the molecular formula of the compound?

2 / 40

Combustion of 7.8g of potassium produced 14.2g of an oxide. Which of the following is the simplest formula of the oxide of potassium formed?

3 / 40

In a certain compound 15.5g of phosphorus combine with 20g of oxygen. What is the simplest formula of the compound?

4 / 40

232g of an oxide of iron contains 168g of iron combined with 64g of oxygen. The empirical formula is.

5 / 40

A sample of a compound containing copper and sulfur only was found to contain 127g of copper and 64g of sulfur. What is the empirical formula of the compound?

6 / 40

The empirical formula of a compound:

7 / 40

CuSO4

8 / 40

CuS

9 / 40

Cu2O

10 / 40

Fe(OH)2

11 / 40

ICl

12 / 40

Ca3N2

13 / 40

Ca(NO3)2

14 / 40

(NH4)2S04

15 / 40

NaHSO4

16 / 40

BaCO3

17 / 40

SO3

18 / 40

P2O5

19 / 40

ZnCl2

20 / 40

Work out the names of each of the following compounds from their formula. Use the data sheet Names & Formulae of Some Common Ions

Formulae are Case Sensitive.

Remember to use regular numbers in formulae e.g. H2O not H2O

HBr

21 / 40

nitrogen (v) oxide

22 / 40

silicon (IV) fluoride

23 / 40

phosphorus (III) chloride

24 / 40

sulfur (VI) fluoride

25 / 40

sulfur dichloride

26 / 40

zinc oxide

27 / 40

sodium sulfide

28 / 40

calcium fluoride

29 / 40

magnesium nitride

30 / 40

silver nitrate

31 / 40

barium hydroxide

32 / 40

potassium carbonate

33 / 40

calcium hydrogencarbonate

34 / 40

ammonium chloride

35 / 40

cobalt (II) nitrate

36 / 40

iron (III) sulfate

37 / 40

Work out the formula of each of the following molecular compounds.

Use a Periodic Table

hydrogen iodide

38 / 40

carbon disulfide

39 / 40

nitrogen trifluoride

40 / 40

Work out the formula of each of the following ionic compounds. Use the data sheet ‘Names & Formulae of Some Common Ions’

Use upper case letter I for roman numerals e.g. (II)

Formulae are Case Sensitive.

Use regular numbers in formulae e.g. H2O not H2O

lithium bromide

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Set 2 – Moles of Elements

4

Moles Set 2 - Moles of Elements

1 / 26

0.100mol of X atoms has a mass of 15.2g. The element is a mixture of two isotopes in equal amounts. One of these is 151X. What is the mass number of the other isotope?

2 / 26

1.00mol of Y2 molecules weighs 14 times as much as 1 mole of hydrogen molecules. What is the relative atomic mass of Y?

3 / 26

Calculate the volume in cm3 of 0.100 mole of osmium atoms (density of Os = 22.5gcm-3) Osmium is the most dense of all the elements

4 / 26

Calculate the volume in cm3 of 0.500 mole of lithium atoms (density of Li = 0.534gcm-3) Lithium is the least dense of all the metallic elements (hint: look at the units!)

5 / 26

Calculate the number of moles of aluminium atoms in a 10.0cm3 block of aluminium (density of Al = 2.70gcm-3

6 / 26

Calculate the number of moles of fluorine molecules (F2) in 9.00g of fluorine

7 / 26

Calculate the number of moles of bromine molecules (Br2) in 4.00g of bromine

8 / 26

Calculate the number of moles of nitrogen molecules (N2) in 28.0g of nitrogen

9 / 26

Calculate the number of moles of nitrogen atoms in 28.0g of nitrogen

10 / 26

Calculate the number of moles of phosphorus atoms in 3.10g of phosphorus

11 / 26

Calculate the number of moles of chlorine atoms in 142g of chlorine

12 / 26

Calculate the number of moles of iron atoms in 55.8g of iron

13 / 26

Calculate the mass of oxygen having the same number of molecules as 7.10g of chlorine

14 / 26

Calculate the mass of silver containing the same number of atoms as 1.20g of magnesium

15 / 26

Calculate the mass of silicon that contains the same number of atoms as 10.0g of calcium

16 / 26

Calculate the mass of 6.02 x1022molecules of iodine (I2)

17 / 26

Calculate the mass of 2.01 x1023atoms of carbon

18 / 26

Calculate the mass of 6.02 x1023atoms of oxygen

19 / 26

Calculate the mass of 3.00 mol of phosphorus (P4) molecules

20 / 26

Calculate the mass of 1.00 mol of bromine (Br2) molecules

21 / 26

Calculate the mass of 0.00200 mol of sodium atoms

22 / 26

Calculate the mass of 0.750 mol of titanium atoms

23 / 26

Calculate the mass of 0.100 mol of lead atoms

24 / 26

Calculate the mass of 0.500 mol of sulfur atoms

25 / 26

Calculate the mass of 2.00 mol of argon atoms

26 / 26

Calculate the mass of 1.00 mole of zinc atoms

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Set 1 – Ar & Mr

2

Moles Set 1 - Ar & Mr

1 / 20

Calculate the relative molecular mass (formula mass) of copper (II) sulfate pentahydrate CuSO4 ●5H2O

2 / 20

Calculate the relative molecular mass (formula mass) of iron (III) bromide, FeBr3

3 / 20

Calculate the relative molecular mass (formula mass) of lithium carbonate, Li2CO3

4 / 20

Calculate the relative molecular mass (formula mass) of silver sulphate, Ag2SO4

5 / 20

Calculate the relative molecular mass (formula mass) of calcium nitrate, Ca(NO3)2

6 / 20

Calculate the relative molecular mass (formula mass) of nitrogen dioxide, NO2

7 / 20

Calculate the relative molecular mass (formula mass) of zinc hydroxide, Zn(OH)2

8 / 20

Calculate the relative molecular mass (formula mass) of sodium iodide, Nal

 

9 / 20

Calculate the relative molecular mass (formula mass) of ethene C2H4

10 / 20

Calculate the relative atomic mass (to one decimal place) of element, C if element C is a mixture of two isotopes, 85C and 87C, with the abundances 72.15% and 27.85% respectively.

11 / 20

Calculate the relative atomic mass (to one decimal place) of element, B if element B is a mixture of two isotopes, 10B and 11B. There is one atom of 10B to every four atoms of 11B.

12 / 20

Calculate the relative atomic mass (to one decimal place) of element, A, if element A is an almost equal mixture of two isotopes, 79A and 81A.

13 / 20

How many carbon-12 atoms would have the same mass as 6 Br atoms? Enter a whole number.

 

14 / 20

How many carbon-12 atoms would have the same mass as 3 Si atoms? Enter a whole number.

15 / 20

How many carbon-12 atoms would have the same mass as 1 Ag atom? Enter a whole number.

16 / 20

Neon (accurate relative atomic mass = 20.18) is made up of three isotopes: Ne-20, Ne-21 and Ne-22.

One of these makes up 90.92% of the element. Which one?

17 / 20

Identify the element (write the symbol) if an atom of Z is one-third of the mass of a 12C atom.

18 / 20

Identify the element (write the symbol) if an atom of Y is twice as heavy as an atom of carbon-12.

19 / 20

The atomic mass of an element is:

20 / 20

Identify the element (write the symbol) if an atom of X is four times as heavy as an atom of carbon-12.

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Moles from Masses 5

0

Moles from Masses - 5

1 / 10

1. Calculate the number of moles of ethane if you have 6.00 g of ethane

C=12.0 H=1.0

2 / 10

2. Calculate the number of moles of propene if you have 105 g of propene

C=12.0 H=1.0

3 / 10

3. Calculate the number of moles of ammonia if you have 100 g of ammonia

N=14.0 H=1.0

4 / 10

4. Calculate the number of moles of hydrogen if you have 6.00 g of hydrogen

H=1.0

5 / 10

5. Calculate the number of moles of aluminium oxide if you have 25.5 g of aluminium oxide

Al=27.0 O=16.0

6 / 10

Calculate the number of moles of phosphorus (V) oxide (P6. 4O10) if you have 80.0 g of phosphorus (V) oxide (P6. 4O10)

P=31.0 O=16.0

7 / 10

7. Calculate the number of moles of lithium hydroxide if you have 80.0 g of lithium hydroxide

Li=6.9 O=16.0 H=1.0

8 / 10

8. Calculate the number of moles of ammonium nitrate if you have 29.0 g of ammonium nitrate

N=14.0 O=16.0 H=1.0

9 / 10

9. Calculate the number of moles of potassium hydrogen carbonate if you have 9.00 g of potassium hydrogen carbonate

K=39.1 H=1.0 C=12.0 O=16.0

10 / 10

10. Calculate the number of moles of iron (II) sulfate heptahydrate if you have 50.0 g of iron (II) sulfate heptahydrate

S=32.1 Fe=55.8 O=16.0 H=1.0

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Moles from Masses 4

0

Moles from Masses - 4

1 / 10

1. Calculate the number of moles of copper (II) sulfate pentahydrate if you have 150 g of copper (II) sulfate pentahydrate

S=32.1 Cu=63.5 O=16.0 H=1.0

2 / 10

2. Calculate the number of moles of anydrous copper (II) sulfate if you have 12.0 g of anydrous copper (II) sulfate

S=32.1 Cu=63.5 O=16.0

3 / 10

3. Calculate the number of moles of barium nitrate if you have 130 g of barium nitrate

Ba=137.3 N=14.0 O=16.0

4 / 10

4. Calculate the number of moles of aluminium sulfate if you have 100 g of aluminium sulfate

S=32.1 Al=27.0 O=16.0

5 / 10

5. Calculate the number of moles of magnesium hydroxide if you have 62.0 g of magnesium hydroxide

H=1.0 C=12.0 O=16.0

6 / 10

Calculate the number of moles of white phosphorous (P6. 4) if you have 12.4 g of white phosphorous (P6. 4)

P=31.0

7 / 10

7. Calculate the number of moles of iodine if you have 12.7 g of iodine

I=126.9

8 / 10

8. Calculate the number of moles of fluorine if you have 76.0 g of fluorine

F=19.0

9 / 10

9. Calculate the number of moles of chlorine if you have 15.8 g of chlorine

Cl=35.5

10 / 10

10. Calculate the number of moles of nitrogen if you have 7.00 g of nitrogen

N=14.0

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Moles from Masses 3

0

Moles from Masses - 3

1 / 10

1. Calculate the number of moles of glucose if you have 36.0 g of glucose

H=1.00 C=12.0 O=16.0

2 / 10

2. Calculate the number of moles of calcium carbonate if you have 60.0 g of calcium carbonate

Ca=40.1 C=12.0 O=16.0

3 / 10

3. Calculate the number of moles of oxygen if you have 64.0 g of oxygen

O=16.0

4 / 10

4. Calculate the number of moles of sodium if you have 34.5 g of sodium

Na=23.0

5 / 10

Calculate the number of moles of NH5. 3 if you have 4.75 g of NH5. 3

N=14.0 H=1.0

6 / 10

Calculate the number of moles of P6. 2O5 if you have 105 g of P6. 2O5

P=31.0 O=16.0

7 / 10

Calculate the number of moles of Ba(NO7. 3)2 if you have 326 g of Ba(NO7. 3)2

Ba=137.3 N=14.0 O=16.0

8 / 10

Calculate the number of moles of NH8. 4NO3 if you have 32.0 g of NH8. 4NO3

N=14.0 O=16.0 H=1.0

9 / 10

Calculate the number of moles of KHCO9. 3 if you have 25.0 g of KHCO9. 3

K=39.1 H=1.0 C=12.0 O=16.0

10 / 10

Calculate the number of moles of FeSO10. 4 . 7H2O if you have 45.6 g of FeSO10. 4 . 7H2O

S=32.1 Fe=55.8 O=16.0 H=1.0

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Moles from Masses 2

0

Moles from Masses - 2

1 / 10

Calculate the number of moles of CuSO1. 4 if you have 479 g of CuSO1. 4

S=32.1 Cu=63.5 O=16.0

2 / 10

Calculate the number of moles of CuSO2. 4 . 5H2O if you have 24.9 g of CuSO2. 4 . 5H2O

S=32.1 Cu=63.5 O=16.0 H=1.0

3 / 10

Calculate the number of moles of I3. 2 if you have 127 g of I3. 2

I=126.9

4 / 10

Calculate the number of moles of Cl4. 2 if you have 355 g of Cl4. 2

Cl=35.5

5 / 10

Calculate the number of moles of N5. 2 if you have 28.0 g of N5. 2

N=14.0

6 / 10

Calculate the number of moles of F6. 2 if you have 9.50 g of F6. 2

F=19.0

7 / 10

Calculate the number of moles of C7. 6H12O7. 6 if you have 3.60 g of C7. 6H12O7. 6

H=1.0 C=12.0 O=16.0

8 / 10

Calculate the number of moles of Mg(OH)8. 2 if you have 87.5 g of Mg(OH)8. 2

Mg=24.3 H=1.00 O=16.0

9 / 10

Calculate the number of moles of CaCO9. 3 if you have 7.00 g of CaCO9. 3

Ca=40.0 C=12.0 O=16.0

10 / 10

Calculate the number of moles of Al10. 2(SO4)3 if you have 17.1 g of Al10. 2(SO4)3

 

S=32.1 Al=27.0 O=16.0

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