Chemical Formulas, Reactions, and Mole Concept Review
Part A. Formulas and Chemical Reactions.
Write complete balanced equations including phase subscripts. Classify each.
1. Lead and phosphorus powders are added and react.
2. Calcium metal reacts with fluorine gas.
3. Methane (CH4) is decomposed.
4. Iron (III) bromide is decomposed to isolate bromine.
5. Propane C3H8 (l) is burned as a fuel.
6. A solution of lead (II) nitrate is added to the solution of sodium carbonate.
7. Magnesium is added to hydrochloric acid.
8. Iron (II) acetate solution is added to a solution of barium chloride.
9. Iron ore (iron (III) oxide) is reacted with carbon to refine iron. Carbon dioxide gas is
produced.
10. Potassium is added to water. The resulting chemical solution is basic and the gas
produced “pops” with a lit splint.
11. A solution of nickel (III) nitrate is added to a solution of phosphoric acid.
Part B. Mole Calculations
1. How many atoms of oxygen are there in 105.3 g of glucose (C6H12O6)?
2. What volume would 16.2 g of nitrogen gas occupy at STP?
3. How many atoms would 2.35 L of neon have?
4. If a sample of disulphur hexabromide had 6.99 x 1023 atoms of bromine what mass
would the sample have?
5. Find the total number of atoms in 7.67 g of sodium phosphide.
6. How many carbon atoms in 60.5 g of ethanol (CH3CH2OH)?
7. How many molecules in
a) 7.56 g of bromine gas?.
b) 88.55 g of carbon monoxide gas?.
c) 18.6 L of chlorine gas (at STP)?
d) 1.56 x 103 L of methane gas at STP?
8. What volume, at STP, would
a) 6.85 x 1022 molecules of sulphur dioxide take up.
b) 68.7 g of helium take up.
Chemical Formulas, Reactions, and Mole Concept Review
Part A. Formulas and Chemical Reactions.
Write complete balanced equations including phase subscripts. Classify each.
1. Lead and phosphorus powders are added and react.
synthesis
6 Pb (s) + P4 (s)  2 Pb3P2 (s)
2. Calcium metal reacts with fluorine gas.
synthesis
Ca (s) + F2 (g)
3. Methane (CH4) is decomposed.

CaF2 (s)
decomposition
CH4 (g)  C(s) + 2 H2 (g)
4. Iron (III) bromide is decomposed to isolate bromine.
decomposition
2 FeBr3 (s)
5. Propane C3H8 (l) is burned as a fuel.

3 Br2 (l) + 2 Fe (s)
combustion
C3H8 (l) + 5 O2 (g) 
3 CO2 (g) + 4 H2O (g)
6. A solution of lead (II) nitrate is added to the solution of sodium carbonate.
double replacement Pb(NO3)2 (aq) + Na2CO3 (aq) 2 NaNO3(aq) + PbCO3 (s)
7. Magnesium is added to hydrochloric acid.
single replacement
Mg (s) +2 HCl (aq) 
MgCl2 (aq) + H2 (g)
8. Iron (II) acetate solution is added to a solution of barium chloride.
double replacement Fe(CH3COO)2 (aq) + BaCl2(aq) FeCl2(aq) + Ba(CH3COO)2 (aq)
9. Iron ore (iron (III) oxide) is reacted with carbon to refine iron. Carbon dioxide gas is
produced.
single replacement
2 Fe2O3 (s) + 3 C (s) 
3 CO2(g) + 4 Fe (s)
10. Potassium is added to water. The resulting chemical solution is basic and the gas
produced “pops” with a lit splint.
single replacement
2 K (s) + 2 HOH(l) 
2 KOH (aq) + H2 (g)
11. A solution of nickel (III) nitrate is added to a solution of phosphoric acid.
double replacement
Ni(NO3)3 (aq) + H3PO4 (aq)

3 HNO3 (aq) + NiPO4 (s)
Part B. Mole Calculations
1. How many atoms of oxygen are there in 105.3 g of glucose (C6H12O6)?
2.114 x 1024 atoms O
2. What volume would 16.2 g of nitrogen gas occupy at STP?
13.0 L N2
3. How many atoms would 2.35 L of neon have?
6.32 x 1022 atoms Ne
4. If a sample of disulphur hexabromide had 6.99 x 1023 atoms of bromine what mass
would the sample have?
105 g S2Br6
5. Find the total number of atoms in 7.67 g of sodium phosphide.
1.85 x 1023 atoms
6. How many carbon atoms in 60.5 g of ethanol (CH3CH2OH)?
1.58 x 1024 atoms C
7. How many molecules in
a) 7.56 g of bromine gas?.
2.85 x 1022 molecules Br2
b) 88.55 g of carbon monoxide gas?.
1.903 x 1024 molecules CO
c) 18.6 L of chlorine gas (at STP)?
5.00 x 1023 molecules Cl2
d) 1.56 x 103 L of methane gas at STP?
4.19 x 1025 molecules CH4
8. What volume, at STP, would
a) 6.85 x 1022 molecules of sulphur dioxide take up.
b) 68.7 g of helium take up.
2.55 L SO3
385 L He