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REVIEW TIME
DEFINE THE FOLLOWING: Atom, element, compound, mixture, proton, neutron, electron, atomic
number, Mass number, atomic mass, isotope, ion, ionic charge, cation, anion, polyatomic ions, diatomic
ions.
Write the Chemical Formula
(1) sodium nitrite
(2) copper (II)oxide
(3) sodium iodide
(4) sulfur dioxide
(5) hydrogen sulfide
(6) magnesium phosphate
(7) potassium hydrogen carbonate
(8) iron(III) chloride
(16) magnesium oxide
(17) potassium sulphate
(18) magnesium nitride
(19) sodium nitrate
(20) carbon tetrachloride
(21) potassium sulphite
(22) calcium chloride
(23) sodium sulphide
Write the names for the following Chemical Formulas
CaCl2
NH4OH
Mg(N03)2
CO2
NaNO3
Mg3(PO4)2
Na2SO4
NaI
Mg(OH)2
FeCl3
CO
NaHSO4
Write the correct Molecular formula for each.
Potassium Nitrate
Ammonium Phosphate
Hydrogen Hydroxide
Calcium Chlorate
Copper (II) Nitrate
Mg CO3
Al (C2H3O2) 3
Fe (NO3) 3
Ca CO3
Ca SO4
COMPLETE THE TABLE
Element
Symbol
Atomic #
Mass #
Protons
Neutrons
Hydrogen
2
12
Fe
79
State the LAW OF CONSERVATION OF MASS.
Balance the following equations:
1)
___ NaNO3 + ___ PbO → ___ Pb(NO3)2 + ___ Na2O
2)
___ AgI + ___ Fe2(CO3)3 → ___ FeI3 + ___ Ag2CO3
3)
___ C2H4O2 + ___ O2 → ___ CO2 + ___ H2O
4)
___ ZnSO4 + ___ Li2CO3 → ___ ZnCO3 + ___ Li2SO4
5)
___ V2O5 + ___ CaS → ___ CaO + ___ V2S5
6) Potassium bromide added to lithium iodide makes lithium bromide and potassium iodide.
7) When silver(I) nitrate is added to calcium chloride, calcium nitrate and silver(I) chloride are produced.
8) Potassium sulphate plus magnesium chloride forms magnesium sulphate and potassium chloride.
9) When iron(III)nitrate is added to sodium hydroxide, the result is iron(III) hydroxide and sodium nitrate.
LIST THE 5 Common types of reaction and give a chemical equation.
REVIEW TIME
DEFINE THE FOLLOWING: Atom, element, compound, mixture, proton, neutron, electron, atomic
number, Mass number, atomic mass, isotope, ion, ionic charge, cation, anion, polyatomic ions, diatomic
ions.
Write the Chemical Formula
(1) sodium nitrite
(2) copper (II)oxide
(3) sodium iodide
(4) sulfur dioxide
(5) hydrogen sulfide
(6) magnesium phosphate
(7) potassium hydrogen carbonate
(8) iron(III) chloride
(16) magnesium oxide
(17) potassium sulphate
(18) magnesium nitride
(19) sodium nitrate
(20) carbon tetrachloride
(21) potassium sulphite
(22) calcium chloride
(23) sodium sulphide
Write the names for the following Chemical Formulas
CaCl2
NH4OH
Mg(N03)2
CO2
NaNO3
Mg3(PO4)2
Na2SO4
NaI
Mg(OH)2
FeCl3
CO
NaHSO4
Write the correct Molecular formula for each.
Potassium Nitrate
Ammonium Phosphate
Hydrogen Hydroxide
Calcium Chlorate
Copper (II) Nitrate
Mg CO3
Al (C2H3O2) 3
Fe (NO3) 3
Ca CO3
Ca SO4
COMPLETE THE TABLE
Element
Symbol
Atomic #
Mass #
Protons
Neutrons
Hydrogen
2
12
Fe
79
State the LAW OF CONSERVATION OF MASS.
Balance the following equations:
1)
___ NaNO3 + ___ PbO → ___ Pb(NO3)2 + ___ Na2O
2)
___ AgI + ___ Fe2(CO3)3 → ___ FeI3 + ___ Ag2CO3
3)
___ C2H4O2 + ___ O2 → ___ CO2 + ___ H2O
4)
___ ZnSO4 + ___ Li2CO3 → ___ ZnCO3 + ___ Li2SO4
5)
___ V2O5 + ___ CaS → ___ CaO + ___ V2S5
6) Potassium bromide added to lithium iodide makes lithium bromide and potassium iodide.
7) When silver(I) nitrate is added to calcium chloride, calcium nitrate and silver(I) chloride are produced.
8) Potassium sulphate plus magnesium chloride forms magnesium sulphate and potassium chloride.
9) When iron(III)nitrate is added to sodium hydroxide, the result is iron(III) hydroxide and sodium nitrate.
LIST THE 5 Common types of reaction and give a chemical equation.
HOW MANY MOLES ARE THERE IN:
a) 13 g zinc
b) 15 g sulphur
c) 0.50 g gold
d) 5.0 g iron
WHAT IS THE MASS OF:
a) 3.0 mol copper
c) 2.3 x 10-3 mol magnesium
b) 0.044 mol sulphur
d) 2.0 mol sodium carbonate
HOW MANY MOLES ARE THERE IN:
a) 13 g zinc
b) 15 g sulphur
c) 0.50 g gold
d) 5.0 g iron
WHAT IS THE MASS OF:
a) 3.0 mol copper
c) 2.3 x 10-3 mol magnesium
b) 0.044 mol sulphur
d) 2.0 mol sodium carbonate
CALCULATE THE NUMBER OF MOLES IN 20 g OF:
a) sodium sulphide
b) copper (II) nitrate
c) copper (II) sulphate d) calcium carbonate
HOW MANY PARTICLES ARE THERE IN:
a) 12 grams of carbon b) 15 g of sodium chloride
c) 13 g of zinc
c) 140 g magnesium sulphate
STOICHIOMETERY
1. Methane is the main component of natural gas which we use as a fuel. When methane burns in air, the
following reaction takes place:
a)
b)
c)
d)
e)
f)
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
How many moles of oxygen are needed to react with 0.1 mole of CH4
How many moles of CO2 are produced from 0.1 moles of CH4
How many moles of water are produced from 0.1 moles of CH4
How many moles of carbon dioxide will be produced by 0.1 mole of oxygen gas?
How many moles of oxygen gas will react completely with 0.25 mole of methane gas
How many moles of water (gas) will be produced by 8.0 moles of oxygen gas?
2. Aluminium powder burns in oxygen to form aluminium oxide according to the following equation:
a)
b)
c)
4Al3+ (s) + 3O2 (g)
→ 2Al2O3 (s)
What amount, in moles, of aluminium is needed to form 1.2mol of Al2O3(s)?
What amount of oxygen gas is needed to react completely with 1.25 mol of aluminium?
Calculate the amount of Al2O3(s)¬ formed when 6.5mol of oxygen reacts completely with
aluminium.
3. Acetylene gas (C2H2) is produced in Australia by CIG by adding water to imported calcium carbide
(CaC2).
a)
b)
c)
CaC2 (s) + 2H2O (l)
→ C2H2(g) + Ca(OH)2 (aq)
What mass of acetylene is produced when 5.00g of calcium carbide is added to a pool of water?
What volume would this occupy at STP?
What mass of water would be consumed by 98kg of calcium carbide?
4. The combustion of petrol can be approximately represented by the equation:
2C8H18(g) + 25O2(g)
→
16CO2(g) + 18H2O(g)
a) What mass of oxygen is used up in the combustion of 1kg of petrol?
HOW MANY MOLES ARE THERE IN:
a) 13 g zinc
b) 15 g sulphur
c) 0.50 g gold
d) 5.0 g iron
WHAT IS THE MASS OF:
a) 3.0 mol copper
c) 2.3 x 10-3 mol magnesium
b) 0.044 mol sulphur
d) 2.0 mol sodium carbonate
HOW MANY MOLES ARE THERE IN:
a) 13 g zinc
b) 15 g sulphur
c) 0.50 g gold
d) 5.0 g iron
WHAT IS THE MASS OF:
a) 3.0 mol copper
c) 2.3 x 10-3 mol magnesium
b) 0.044 mol sulphur
d) 2.0 mol sodium carbonate
CALCULATE THE NUMBER OF MOLES IN 20 g OF:
a) sodium sulphide
b) copper (II) nitrate
c) copper (II) sulphate d) calcium carbonate
HOW MANY PARTICLES ARE THERE IN:
a) 12 grams of carbon b) 15 g of sodium chloride
c) 13 g of zinc
c) 140 g magnesium sulphate
STOICHIOMETERY
1) Methane is the main component of natural gas which we use as a fuel. When methane burns in air, the
following reaction takes place:
a)
b)
c)
d)
e)
f)
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
How many moles of oxygen are needed to react with 0.1 mole of CH4
How many moles of CO2 are produced from 0.1 moles of CH4
How many moles of water are produced from 0.1 moles of CH4
How many moles of carbon dioxide will be produced by 0.1 mole of oxygen gas?
How many moles of oxygen gas will react completely with 0.25 mole of methane gas
How many moles of water (gas) will be produced by 8.0 moles of oxygen gas?
2. Aluminium powder burns in oxygen to form aluminium oxide according to the following equation:
4Al3+ (s) + 3O2 (g)
→ 2Al2O3 (s)
a)
What amount, in moles, of aluminium is needed to form 1.2mol of Al2O3(s)?
b)
What amount of oxygen gas is needed to react completely with 1.25 mol of aluminium?
c)
Calculate the amount of Al2O3(s)¬ formed when 6.5mol of oxygen reacts completely with
aluminium.
3. Acetylene gas (C2H2) is produced in Australia by CIG by adding water to imported calcium carbide
(CaC2).
a)
b)
c)
CaC2 (s) + 2H2O (l)
→ C2H2(g) + Ca(OH)2 (aq)
What mass of acetylene is produced when 5.00g of calcium carbide is added to a pool of water?
What volume would this occupy at STP?
What mass of water would be consumed by 98kg of calcium carbide?
4. The combustion of petrol can be approximately represented by the equation:
2C8H18(g) + 25O2(g) → 16CO2(g) + 18H2O(g)
a) What mass of oxygen is used up in the combustion of 1kg of petrol?