0620_s24_qp_42
A paper of Chemistry, 0620
Questions:
6
Year:
2024
Paper:
4
Variant:
2
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1
A list of gases is shown. ammonia helium hydrogen carbon dioxide carbon monoxide chlorine methane nitrogen dioxide propene sulfur dioxide Answer the following questions about these gases. Each gas may be used once, more than once or not at all. State one gas which: is the main constituent of natural gas is responsible for both photochemical smog and acid rain is unsaturated has monatomic particles reduces iron(oxide in a blast furnace. Nitrogen dioxide, NO2, and carbon monoxide are removed from a car exhaust by a catalytic converter. Write the symbol equation for this reaction.
10. Chemistry of the environment  →  10.3. Air quality and climate
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2
A list of five metals is shown. copper iron magnesium potassium silver All metals form positive ions. Describe how atoms form positive ions. State which of the five metals in the list has the greatest tendency to form positive ions. Suggest one of the five metals in the list which is not likely to show catalytic properties. State which of the five metals in the list is a major component of stainless steel. A student adds a sample of a metal to an aqueous metal salt in a beaker to see if a displacement reaction takes place. Complete Table 2.1 to show the colour of the solution in the beaker at the start and at the end of the experiment. Table 2.1 metal aqueous solution colour at the start colour at the end magnesium iron(sulfate green silver copper(sulfate Most Group II metals form a gas when placed into cold water. An alkaline solution is also formed. Name the gas formed when strontium is added to cold water. Name the alkaline solution formed when strontium is added to cold water. One Group II metal reacts very slowly when placed in cold water. When heated, the metal reacts with steam to form a white solid. Identify this metal and name the white solid formed. metal white solid Under certain conditions, iron will react with steam to form an oxide of iron with the formula Fe3O4. Fe3O4 reacts with dilute hydrochloric acid to form a mixture of iron(and iron(salts and water. Deduce the symbol equation for the reaction between Fe3O4 and dilute hydrochloric acid. ,  ,
9. Metals  →  9.4. Reactivity series
9. Metals  →  9.1. Properties of metals
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3
The symbol equation for the industrial production of ammonia is shown. N2+ 3H22NH3∆H = –90 kJ / mol Name this industrial process. State the meaning of ∆H. State the typical conditions and name the catalyst used in the industrial production of ammonia. temperature and units pressure and units catalyst used State two methods of increasing the rate of this reaction. The symbol equation for the reaction can be represented as shown in . N N + +  H H = –90 kJ / mol H H N H H H N H H H H H H Table 3.1 shows some bond energies. Table 3.1 bond N≡N H–H bond energy in kJ / mol Use the bond energies in Table 3.1 and ∆H to calculate the bond energy of an N–H bond, in kJ / mol. Use the following steps. ● Calculate the energy needed to break bonds in the reactants. kJ ● Calculate the energy released when bonds form in the products. kJ ● Calculate the energy of an N–H bond. kJ / mol ,  , An incomplete symbol equation for the preparation of ammonia in the laboratory is shown. CaO + 2NH4Cl → CaCl 2 + + 2NH3 Complete the symbol equation. Name NH4Cl. Calculate the volume of ammonia, NH3, measured at room temperature and pressure, which forms when 1.12 g of CaO is heated with excess NH4Cl. [Mr: CaO, 56] cm3 ,  ,
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
5. Chemical energetics  →  5.1. Exothermic and endothermic reactions
6. Chemical reactions  →  6.2. Rate of reaction
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4
A carboxylic acid reacts with an alcohol to produce an ester and water. Under certain conditions, this reaction can be reversed so an ester reacts with water to produce a carboxylic acid X and an alcohol Y. The reaction reaches an equilibrium. CH3CH2COOCH3 + H2O X + Y The forward reaction is endothermic. Deduce the empirical formula of the ester. Name the ester. Name carboxylic acid X and draw its displayed formula. name displayed formula Name alcohol Y and give its structural formula. name structural formula Complete Table 4.1 to show the effect, if any, for each change of condition. Table 4.1 change of condition effect on the concentration of carboxylic acid X at equilibrium temperature is decreased concentration of CH3CH2COOCH3 is decreased more alcohol Y is added a catalyst is added At the beginning of the reaction between the ester and water, no carboxylic acid is present in the reaction mixture. Suggest how the pH of the reaction mixture changes from the start of the reaction until equilibrium is reached. Assume alcohols and esters are neutral. pH at start of reaction pH at equilibrium Identify the ion that causes the change in pH. Name an indicator which can be used to follow the change in pH. ,   ,
11. Organic chemistry  →  11.7. Carboxylic acids
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
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5
Sulfur is a Group VI element. A sample of sulfur contains two isotopes, 32S and 34S. Complete Table 5.1 to show the number of protons and neutrons in one atom of each isotope of sulfur. Table 5.1 32S 34S protons neutrons State why these isotopes have identical chemical properties. State the mass of 6.02 × 1023 atoms of 34S. Include units in your answer. State the name of the amount of substance which contains 6.02 × 1023 atoms. Table 5.2 shows the relative abundance of these isotopes of sulfur in the sample. Table 5.2 atom 32S 34S relative abundance 95% 5% Calculate the relative atomic mass of sulfur in this sample to one decimal place. relative atomic mass = Sulfur reacts with magnesium to form magnesium sulfide, MgS, an ionic compound. Complete the dot-and-cross diagram in of the ions in magnesium sulfide. Give the charges on the ions. Mg S State why MgS has a high melting point. State why molten MgS conducts electricity. An acid containing sulfur reacts with sodium hydroxide, NaOH, to form a salt and water. The salt has the formula Na2SO3. Deduce the formula of this acid. Deduce the formula of the anion in Na2SO3. Na2SO3 is oxidised by acidified aqueous potassium manganate(. State what VII refers to in the name potassium manganate(. State the colour change when this reaction happens. from to . ,  ,
2. Atoms, elements and compounds  →  2.3. Isotopes
3. Stoichiometry  →  3.2. Relative masses of atoms and molecules
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
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6
Glucose is involved in two processes. Glucose, C6H12O6, is made in plants from carbon dioxide and water. Name this process. Write the symbol equation for this process. State two essential conditions needed for this process to happen. Glucose is converted to ethanol. Name this process. Name the other product formed when glucose is converted to ethanol. Ethanol is made by reacting ethene with steam in an industrial process. State the conditions and type of catalyst used in this industrial production of ethanol. temperature and units pressure and units type of catalyst used Explain why this reaction is an addition reaction. Complete the dot-and-cross diagram in of a molecule of ethanol. H H H H C O H H C ,  ,
11. Organic chemistry  →  11.6. Alcohols
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