HERE'S SOME PRACTICE QUESTIONS
Chapter 5.3
Find the relative molecular mass (Mr) of
1. Zinc Suldife
ZnS
2. Titanium Dioxide
TiO2
3. Sodium Sulfate
Na2So4
4. Aluminium Oxide
Al2O3
5. Lead Nitrate
Pb (NO3)2
Chapter 5.4
1. 64g of copper reacts with 16g of oxygen to give copper(II) oxide.
a) What mass of copper will react with 32g of oxygen?
b) What mass of oxygen will react with 32g of copper?
c) How much copper and oxygen will give 8g of copper(II) oxide?
2. If 54g of magnesium oxide is produced when 36g of magnesium reacts with 18g of oxygen,
a)What is the amount of magnesium oxide produced
when there is 36g of oxygen?
b)Find the amount of magnesium needed to react with 28g of oxygen.
c)What is the percentage of magnesium in magnesium oxide in (2b)
Chapter 6.1
1. How many particles are there in 1 mole?
2. Calculate the moles of oxygen atoms in 64g of oxygen
3. Calculate the mass of 3 moles of sulphur dioxide, SO2.
Chapter 6.2
1) Find the masses,
a) 0.35 mole of Pb(OH)2 =
b) 1.42 mole of K2Cr2O7 =
c) 0.76 mole of C3H7OH =
2) Find the no. of moles,
a) 39.61g of BaSO4 is =
b) 7.5 g of Li2O =
c) 126.28g of AgCi =
3) Sodium reacts with chlorine and forms sodium chloride. What is the mass of chlorine needed to react with 11.5 g of sodium?
Chapter 6.3
1) Find the volume (dm^3) of these questions;
a) 22g of CO2 =
b) 1.5 mole of CI2 =
c) 0.005 mole of H2 =
2) Hydrogen reacts with oxygen to form water.
a) What is the balanced ratio for this equation?
b) What is the volume of Hydrogen when reacting with 24dm^3 of oxygen?
3) Magnesium chloride reacts with flourine and gives magnesium flouride and chlorine. ( MgCI2 + F2 --> MgF2 + CI2 )
To produce 1.2dm^3 of CI2, what is the mass of MgCI2 required?
Chapter 6.4
1) 0.5dm^3 of 1.7M H2SO4
a) How many moles are there in 0.5dm^3?
b) What is the concentration?
2) In 1.7 dm^3 of 0.55M HCI, what is the number of moles?
3) 0.73dm^3 of 1.5M H2SO4 was added to 0.5dm^3 of water. What is the new concentration?
Chapter 6.5
1. What is the empirical formula of a compound
containing 60.0% sulfur and 40.0% oxygen by mass?
2. A compound is found to contain 23.3% magnesium,
30.7% sulfur and 46.0% oxygen. What is the empirical
formula of this compound?
3. What is the empirical formula for a compound
containing 38.8% carbon, 16.2% hydrogen
and 45.1% nitrogen?
Chapter 6.6
1. If the compound 7.19% phosphorus; 92.81% bromine has a molar
mass of 431g/mol, what is the molecular formula?
2. If the compound 30.4% nitrogen; 69.6% oxygen has a molar
mass of 92g/mol, what is the molecular formula?
3. A compound with the following composition has
a molar mass of 60.10g/mol: 39.97% carbon;
13.41% hydrogen; 46.62% nitrogen.
Find the molecular formula.
Chapter 6.7
1. For the balanced equation shown below, if
the reaction of 20.7 grams of CaCO3 produces
6.81 grams of CaO, what is the percent yield?
2. For the balanced equation shown below, if
the reaction of 0.112 grams of H2 produces
0.745 grams of H2O, what is the percent yield?
3. For the balanced equation shown below, if the
reaction of 40.8 grams of C6H6O3 produces a
39.0% yield, how many grams of H2O would be
produced ?
