| 1 | 2 | 3 | 4 | 5 | 6 |
| 7 | 8 | 9 |
Question 1
This question is about the extraction of metals from their oxides. X is an unknown metal which can be extracted from its oxide by reduction with hydrogen. The equation for the reaction is: H2 + XO âž” X + H2O (You may need a periodic table) |
a) | The sum of the relative formula masses of the reactants is 81.5. Calculate the relative atomic mass of X.
|
b) | Identify the unknown metal using the periodic table.
|
c) | Carbon can also be used to reduce iron oxide. Balance the chemical equation below.
|
d) | Calculate the relative formula mass of carbon dioxide, CO2.
|
|
Question 2
A student is investigating the neutralisation reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH). The diagram below shows the apparatus used for the titration. |
a) | State the name of the piece of apparatus labelled A.
|
b) | The student opens the tap and allows the sulfuric acid to drain into the conical flask. The tap is closed when the student observes a permanent colour change of the indicator. The student then reads the burette to obtain a value for the titre and records it in a table. State the value shown on the burette below for titration 5.
|
c) | The student uses concordant results to calculate the mean titre. Concordant results are those within 0.1 cm3 of each other. Calculate the mean titre of the students results.
|
d) | The volume of the 0.2 mol/dm3 sodium hydroxide in the conical flask is 30 cm3. Calculate the concentration of the sulfuric acid used.
|
|
Question 3
A student neutralises 25 cm3 of hydrochloric acid by titrating sodium hydroxide solution into it. The hydrochloric acid concentration is 0.2 mol/dm3. |
a) | Describe how the student can obtain an accurate value for the volume of sodium hydroxide needed to neutralise the hydrochloric acid.
|
b) | The table below shows the student's results. Calculate the mean volume of sodium hydroxide added to the hydrochloric acid. Concordant results are results which are within 0.1 cm3 of each other.
|
c) | Calculate the concentration of sodium hydroxide used to neutralise the acid.
|
|
Question 4
This question is about the relative formula mass of iron Chloride, FeCl3. |
a) | Iron chloride is formed by reacting iron with chlorine gas. Complete the balanced symbol equation for the reaction between iron and chlorine to form iron chloride.
|
b) | The relative formulas masses of chlorine and iron are 35.5 and 56 respectively. Calculate the relative formula mass of iron chloride.
|
c) | A student has a sample of 3.8 g of iron chloride. Calculate the number of moles of iron chloride in the sample.
|
|
Question 5
This question is about the concentration of ethanoic acid. |
a) | The relative formula of ethanoic acid is CH3COOH. Calculate the relative formula mass of ethanoic acid. (You may need a periodic table) A 58 B 60 C 48 D 29
|
b) | A student has 20 cm3 of ethanoic acid solution. The solution contains 4 g of ethanoic acid. Calculate the concentration of the ethanoic acid solution in mol/dm3.
|
|
Question 6
A student is investigating the reaction between magnesium ribbon and hydrochloric acid. The balanced equation for the reaction is Mg + 2HCl âž” MgCl2 + H2 |
a) | The mass of the magnesium ribbon is 0.13 g. Calculate the number of moles of magnesium used. (You may need a periodic table)
|
b) | The magnesium ribbon is dropped into a conical flask containing 0.1 mol/dm3 hydrochloric acid. Calculate the minimum volume of acid to completely react with the 0.13 g sample of magnesium.
|
c) | The label on the hydrochloric acid was wrong and the actual concentration of the acid is half the stated value. Describe and explain what the student would observe when they add the magnesium ribbon to the acid.
|
|
Question 7
This question is about pentene, C5H10. |
Which of the following is the empirical formula of pentene? A CH B CH2 C C5H10 D (CH2)3
|
b) |
c) | Calculate the number of moles in a 200 g sample of pentene. Give your answer to 2 decimal places.
|
|
Question 8
This question is about the empirical formula of group 1 metals. (You may need a periodic table) |
a) | Potassium reacts with oxygen in the air to form potassium oxide on the metal's surface. 1.17 g of potassium reacts with 0.24 g of oxygen. Calculate the empirical formula of potassium oxide.
|
b) | Complete the balanced symbol equation below to show the reaction between potassium and oxygen to form potassium oxide.
|
c) | A student wants to react 4 g of potassium with 3 g of oxygen. |
c) i) | Which is the limiting reactant in the reaction above?
|
c) ii) | Calculate the mass of the potassium oxide produced. Give your answer in grams, to 2 decimal places.
|
|
Question 9
A student heats calcium carbonate (CaCO3) to form calcium oxide (CaO) and carbon dioxide (CO2). |
a) | Write a balanced symbol equation for the reaction.
|
b) | The student is demonstrating the conservation of mass. Explain what is meant by the conservation of mass.
|
c) | Calculate the relative formula mass of calcium carbonate, calcium oxide, and carbon dioxide. (You may need a periodic table)
|
d) | 1.5 g of calcium carbonate is heated in a crucible. Calculate the mass of calcium oxide and carbon dioxide produced.
|
|
| 1 | 2 | 3 | 4 | 5 | 6 |
| 7 | 8 | 9 |