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1. This question is about gases found in clean, dry air and gases found in polluted air.
(a) Name one gas found in clean, dry air which contributes to global warming. [1]
(b) State the percentage of nitrogen in clean, dry air. [1]
(c) Name the substance used to remove sulfur dioxide in flue gas desulfurisation. [1]
(d) Nitrogen dioxide, NO$_2$, is formed in car engines. Name the equipment in a car exhaust used to remove the NO$_2$ formed in car engines. [1]
(e) All gases diffuse.
(i) Choose from the list of formulae the gas which diffuses most quickly. Draw a circle around your answer. CO, CO$_2$, CH$_4$, NO$_2$, SO$_2$ [1]
(ii) Explain your answer to (i). [1]
(f) State one adverse effect of carbon monoxide on human health. [1]
(g) Carbon dioxide, CO$_2$, is a reactant in photosynthesis. Name the two products of photosynthesis. [2]
(h) Complete the dot-and-cross diagram for a molecule of CO$_2$. Show outer shell electrons only. [2]
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2. Lithium, sodium, and potassium are Group I elements.
(a) Name the type of bonding in these elements. [1]
(b) Sodium reacts with cold water to form hydrogen gas and a solution of a strong alkali.
(i) State the test for hydrogen gas. Test... Positive result... [1]
(ii) Suggest the pH of a solution of a strong alkali. pH = ... [1]
(iii) Name a substance which can be used to confirm the pH of a solution of a strong alkali. [1]
(iv) Write the symbol equation for the reaction between sodium and cold water. Include state symbols. [3]
(c) Lithium has two naturally occurring types of atoms, $^6$Li and $^7$Li.
(i) State the name given to atoms of the same element with different nucleon numbers. [1]
(ii) Complete Table 2.1 to show the number of protons, neutrons and electrons in the atom and ion of lithium shown. [Table_1] [3]
(iii) Calculate the relative atomic mass of lithium to one decimal place. [2]
(d) Potassium oxide, K$_2$O, is an ionic compound. Complete to show the electronic configurations of the ions in potassium oxide. Show the charges on the ions. [3]
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593
593
3. The Haber process is used to manufacture ammonia.
(a) State the main source of each gas used in the Haber process. Nitrogen... Hydrogen... [2]
(b) The equation for the Haber process is shown. $$N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \quad \Delta H = -92 \text{ kJ/mol}$$ The reaction is reversible. The forward reaction is exothermic.
(i) State what is meant by the symbol $\Delta H$. [1]
(ii) $\Delta H$ for the forward reaction is $-92$ kJ/mol. State why this value shows that the forward reaction is exothermic. [1]
(iii) State the typical conditions and name the catalyst used in the Haber process. Temperature... °C Pressure... kPa Catalyst... [3]
(iv) Complete to show the effect, if any, when the typical conditions in the Haber process are changed. Use only the words increases, decreases or no change. [Table_2] [4]
(v) Explain in terms of collision theory why increasing the temperature increases the rate of the reaction. [3]
(c) Ammonia reacts with an acid to form ammonium sulfate, (NH$_4$)$_2$SO$_4$.
(i) State the formula of the acid used. [1]
(ii) State one use of ammonium sulfate. [1]
(iii) Calculate the percentage composition by mass of nitrogen in (NH$_4$)$_2$SO$_4$. [2]
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522
4. Copper is element 29 in the Periodic Table.
(a) Brass contains copper.
(i) Name the other metal in brass. [1]
(ii) State the term given to a mixture of a metal with another element. [1]
(b) Copper can be stretched into wires. Copper wires conduct electricity.
(i) Name the property of metals which means that they can be stretched into wires. [1]
(ii) Name the particles responsible for the conduction of electricity in solid copper. [1]
(c) Copper is a transition element. Some physical and chemical properties of transition elements are shown.
Physical properties: high density, high strength.
Chemical properties: form coloured compounds, have ions with variable oxidation numbers.
(i) State one other physical property of transition elements. [1]
(ii) State one other chemical property of transition elements. [1]
(d) Hydrated copper(II) sulfate is a coloured compound. It exists as hydrated crystals which contain water molecules.
(i) State the term given to water molecules present in hydrated crystals. [1]
(ii) State the colour of hydrated copper(II) sulfate crystals. [1]
(iii) Write the formula of hydrated copper(II) sulfate. [2]
(e) Copper(II) oxide is formed when copper(II) nitrate, Cu(NO$_3$)$_2$, is heated. $$2Cu(NO_3)_2(s) \rightarrow 2CuO(s) + 4NO_2(g) + O_2(g)$$
(i) State the class of oxide to which copper(II) oxide belongs. [1]
(ii) State the meaning of the Roman numeral (II) in the name copper(II) oxide. [1]
(iii) 0.0200 moles of Cu(NO$_3$)$_2$ is heated. Calculate the mass of 0.0200 moles of Cu(NO$_3$)$_2$. [2]
(iv) Calculate the total volume of gas, in dm3 at r.t.p., produced when 0.0200 moles of Cu(NO$_3$)$_2$ is heated. [2]
(v) Powdered aluminium reduces copper(II) oxide. Write the symbol equation for this reaction. [2]
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539
5. Propane, propene, propan-1-ol, and propanoic acid are members of different homologous series. Molecules of these substances contain three carbon atoms.
(a) Explain why members of a homologous series have similar chemical properties. [1]
(b) Name the homologous series to which propanoic acid belongs. [1]
(c) State the general formula of the homologous series to which propanoic acid belongs. [1]
(d) Propan-1-ol has an unbranched isomer.
● Name this isomer.
● Draw the displayed formula of this isomer. [2]
(e) Propane and propene can be manufactured by heating decane, C$_{10}$H$_{22}$, in the presence of a catalyst. One other product is formed.
(i) Complete the equation for this reaction. $$C_{10}H_{22} \rightarrow ... + ... + ...$$ [2]
(ii) Name this manufacturing process. [1]
(f) Propene forms a polymer named poly(propene).
(i) Draw the displayed formula of a section of poly(propene) showing three repeat units. [2]
(ii) State the type of polymerisation that occurs when propene forms poly(propene). [1]
(g) Propanoic acid reacts with aqueous sodium carbonate to form a salt.
(i) Suggest the name of the salt formed. [1]
(ii) Suggest the formula of the anion in this salt. [1]
(h) Propanoic acid forms an ester when it reacts with ethanol in the presence of a catalyst.
(i) Suggest a suitable catalyst. [1]
(ii) Name the ester formed. [1]
(iii) Draw the displayed formula of this ester. [2]
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566
