1. The equation for the production of ammonia, NH3, is shown.
N2 (g) + 3H2 (g) 2NH3 (g)
Which mass of nitrogen is required to make 51 tonnes of ammonia?
A 21 tonnes
B 25.5 tonnes
C 42 tonnes
D 84 tonnes
2. Which symbol equation represents the reaction between aqueous sodium hydroxide and dilute
sulfuric acid?
3. What is the relative formula mass of magnesium bromide?
A 47
B 82
C 104
D 184
4. Magnesium burns in oxygen to form magnesium oxide.
The equation for the reaction is shown.
2Mg + O2 2MgO
Which mass of magnesium oxide is formed when 48 g of magnesium is burned?
A 20 g
B 40 g
C 80 g
D 160 g
5. What is the formula of iron(III) oxide?
A FeO
B Fe3O4
C FeO2
D Fe2O3
6. Calcium carbonate is heated. Calcium oxide and carbon dioxide gas are formed.
The equation for the reaction is shown.
CaCO3 CaO + CO2
225 kg of calcium carbonate is heated until there is no further change in mass.
The yield of calcium oxide is 85 kg.
What is the percentage yield?
A 37.8% B 47.2%
C 67.5%
D 85.0%
7. What is the empirical formula of a compound that contains 3.66 g of hydrogen, 37.8 g of
phosphorus and 58.5 g of oxygen?
A H6P2O6
B H4PO4
C H3PO3
D HPO
8. The structure of ethene is shown.
How many hydrogen atoms and how many carbon atoms are in one mole of ethene?
9. A compound of element X has the formula X2O and a relative formula mass of 144.
What is element X?
A copper, Cu
B gadolinium, Gd
C sulfur, S
D tellurium, Te
10. Compounds that contain nitrogen can be used as fertilisers.
Which compound contains the greatest proportion of nitrogen by mass?
A CH4N2O
B NH4Cl
C NH4NO3
D (NH4)2SO4
Q1. A 0.5 g sample of calcium carbonate is reacted with excess dilute hydrochloric acid.
CaCO3(s) + 2HCl(aq) CaCl2 (aq) + H2O(l) + CO2 (g)
Calculate volume of CO2 is produced at r.t.p.?
Q2. 0.048 g of magnesium was reacted with excess dilute hydrochloric acid at room temperature
and pressure. The hydrogen gas given off was collected.
a. Write a word and balanced symbol equation for the reaction taking place.
………………………………………………………………………………………………………………………………………
b. How many moles of magnesium were used?
……………………………………… moles
c. Using the equation you have written in your answer to a, calculate the number of moles of
hydrogen and hence the volume of this gas produced.
…………………………………………mole
…………………………………………dm3
d. Calculate the volume of a solution containing 0.1 mol dm−3 hydrochloric acid which would
be needed to react exactly with 0.048 g of magnesium.
……………………………………….dm3
0
