Figure 1 shows a list of particles.
ethene molecule nanoparticle sodium atom starch molecule
Figure 1
In the spaces below, write the names of these particles in order of increasing particle size.
(2)
Explain a possible risk associated with nanoparticulate materials.
(2)
Explain the advantage of using catalysts made of nanoparticles rather than larger particles.
(2)
The concentration of a solution can be calculated using the equation
A student dissolved 9.25 g of ammonium chloride in water and made up the
Use the equation to calculate the concentration of this solution in gdm−3.
concentration =........ g dm
(2)
Dissolving ammonium chloride in water is an endothermic process. Figure 2 shows part of the reaction profile for this process.
Explain how Figure 2 shows that dissolving ammonium chloride in water is an endothermic process.
(2)
Complete the reaction profile in Figure 2 and label the activation energy.
(2)
A student used the equipment in Figure 3 to investigate whether electricity can pass through solid ammonium chloride and through ammonium chloride solution.
If an electrical current flows in the circuit, the lamp will light up.
Figure 4 shows the results of the investigation.
Explain the results of the investigation.
(3)
Diesel oil is a mixture of hydrocarbons that can be obtained from crude oil.
State the name of the process used to separate diesel oil from crude oil.
(1)
Diesel oil contains alkanes. These alkanes are part of an homologous series.
Which statement about compounds in this homologous series is true?
(1)
When fuels such as diesel oil are burned, the high temperatures produced can cause nitrogen and oxygen in the air to form the pollutant nitrogen dioxide.
Complete the balanced equation for the reaction.
(2)
Explain how the greenhouse effect is caused by the gases produced by the complete combustion of diesel oil.
(3)
This question is about polymers.
State a problem with recycling polymers.
(1)
Describe a problem associated with the disposal of polymers.
(2)
Poly(chloroethene) is a polymer made from chloroethene. A molecule of chloroethene is shown in Figure 5.
On Figure 5, draw a circle around the functional group in this molecule.
(1)
Draw a section of a poly(chloroethene) molecule containing three repeating units, showing all bonds.
(3)
What type of polymer is poly(chloroethene)?
(1)
Calculate the relative formula mass of a poly(chloroethene) molecule made from 2850 chloroethene molecules, C2H3Cl.
(relative atomic masses: H = 1.00, C = 12.0, C l = 35.5)
Give your answer to three significant figures.
Show your working.
relative formula mass =........
(3)
This question is about potassium and zinc.
Which of the following temperatures is most likely to be the melting point of potassium?
(1)
Explain how the electronic configuration of an atom of potassium is related to its position in the periodic table.
(2)
Potassium reacts with oxygen to form potassium oxide.
Describe the test to show that a gas is oxygen.
(2)
Potassium oxide is ionic.
Write the electronic configurations for the ions in potassium oxide, K2O.
(2)
Figure 6 shows two gas syringes connected by a glass tube.
Inside the glass tube there are some pieces of zinc. Zinc reacts with oxygen at a temperature of over 225 °C. Not all the oxygen reacts at once, the oxygen reacts only when in contact with the zinc.
Devise a plan to find the volume of oxygen contained in a known volume of air, using the apparatus shown in Figure 6.
(4)
This question is about the rate of reaction between calcium carbonate and dilute hydrochloric acid.
The word equation for this reaction is
calcium carbonate + hydrochloric acid 
calcium chloride + water + carbon dioxide
Which of the following is the formula for calcium carbonate?
(1)
Some pieces of calcium carbonate were added to dilute hydrochloric acid in a conical flask and the volume of carbon dioxide produced was measured.
Complete the diagram in Figure 7 to show the apparatus to collect the gas produced and measure its volume.
(2)
The reaction between calcium carbonate and dilute hydrochloric acid was investigated at different temperatures.
State what could be used to keep the temperature of the conical flask and its contents at a temperature of 45 °C throughout the reaction.
(1)
Figure 8 shows a graph of volume of gas collected in this investigation.
Draw a tangent at 100 seconds on Figure 8. Use this tangent to calculate the rate of reaction at this time.
rate of reaction =........ cm3
(2)
The temperature of the acid was kept at 45 °C.
State one other variable that needs to be controlled during this investigation.
(1)
Explain, in terms of particles, how decreasing the temperature affects the rate of this reaction.
(3)
A technician was asked to find the concentration of potassium ions in a dilute solution using a flame photometer.
The technician first produced a calibration curve using solutions with known concentrations of potassium ions. Figure 9 contains the data for the calibration curve.
| concentration of potassium ions in mol dm–3 | display reading |
| 0.025 | 180 |
| 0.050 | 280 |
| 0.100 | 440 |
| 0.200 | 580 |
| 0.500 | 900 |
Use the information in Figure 9 to plot the calibration curve on the grid below.
(3)
The technician then obtained a reading of 360 for a dilute solution containing potassium ions.
Use the calibration curve to find the concentration of the potassium ions in this solution.
(1)
In the test for chloride ions, silver nitrate solution is added to a solution containing chloride ions. A white precipitate forms.
Write the ionic equation for this reaction.
(2)
*(c) A student was given a container of ammonium iron(II) sulfate, (NH4)2Fe(SO4)2. The student was also given a dilute solution of sodium hydroxide and access to other laboratory reagents.
Describe the tests the student should carry out to identify the ions in the ammonium iron(II) sulfate, including appropriate equations for the reactions involved.
(6)
This question is about some of the elements in group 7 of the periodic table.
Which row in the table correctly shows the colours and physical states of the elements at room temperature?
(1)
The compound phosphorus oxychloride has the formula POCl3.
Calculate the percentage by mass of chlorine in phosphorus oxychloride.
(relative atomic masses: O = 16.0, P = 31.0, C l = 35.5)
percentage by mass of chlorine =........
(2)
When iron reacts with chlorine, iron chloride is formed.
Two possible equations for this reaction are
A Fe + Cl2 
FeCl2 B 2Fe + 3Cl2 2FeCl3
In an experiment, 8.40 g iron reacts with chlorine to form 19.05 g iron chloride.
Show, using a calculation, which reaction, A or B, is taking place.
You must show your working.
(relative atomic masses: C l = 35.5, Fe = 56.0)
(3)
*(d) Group 1 metals react with the elements from group 7 to form salts.
Some examples of these reactions are shown in Figure 10.
You will find the position of these elements in their groups on the periodic table.
Explain, in terms of their electronic configurations and the relative reactivity of these elements, which of the reactions shown in Figure 10 would be the most violent.
(6)
Pentadecane, C15H32, is a hydrocarbon and is used as a fuel.
The incomplete combustion of pentadecane produces carbon monoxide. Carbon monoxide is a toxic gas.
Explain why the incomplete combustion of pentadecane can produce carbon monoxide as one of the products.
(2)
Explain how carbon monoxide behaves as a toxic gas.
(2)
1 mole of pentadecane can be cracked to form 1 mole of octane, C8H18, and 1 mole of propene, C3H6, and 2 moles of another product.
Complete the balanced equation for this reaction by adding the formula of the missing product.
(1)
Figure 11 shows the reaction of propene, C3H6, with water.
H H H
Figure 11
Figure 12 shows some bond energies.
Use the bond energies in Figure 12 to calculate the energy change of the reaction in Figure 11.
energy change of reaction =........ kJ
(4)
Methane gas, CH4, was burned using the apparatus shown in Figure 13.
Explain why water droplets form on the bottom of the beaker of cold water.
(2)
Propanol, C3H7OH, can undergo reactions to form compounds Y and Z shown in Figure 14.
Figure 14
What happens to propanol when it forms compound Y ?
(1)
Compound Y can also be formed in the following reaction
C H C H
Explain how bromine water can be used to distinguish between compound X and compound Y.
(3)
Compound Z is a carboxylic acid.
Which of the following shows the functional group of a carboxylic acid?
(1)
Compound Z is an acid and turns litmus and universal indicator papers red. Compound Z also shows other acidic properties.
Devise an experiment that would show another acidic property of compound Z.
(2)
The balanced equation for the production of ethanol from the carbohydrate sucrose is
sucrose
Calculate the minimum mass of sucrose needed to produce 26.9 g of ethanol.
(relative formula masses: C2H5OH = 46, C12H22O11 = 342)
minimum mass of sucrose =........
(2)
Calculate the total number of atoms in 10.0 g of sucrose, C12H22O11.
(relative formula mass: C12H22O11 = 342; Avogadro constant = 6.02 × 1023)
number of atoms =........
(2)
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