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0620_m21_qp_42
A paper of Chemistry, 0620
Questions:
6
Year:
2021
Paper:
4
Variant:
2
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1
The table shows the numbers of protons, neutrons and electrons in particles A to I. particle protons neutrons electrons A B C D E F G H I Answer the following questions about particles A to I. Each letter may be used once, more than once or not at all. State which of the particles A to I: is an anion are cations and are noble gas atoms and is a halogen atom is a Group I atom have the same nucleon number and causes acidity in aqueous solutions is used to define the relative atomic mass of elements. Explain why B and C are isotopes of the same element. 
2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table
2. Atoms, elements and compounds  →  2.3. Isotopes
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2
The elements shown are gases at room temperature and pressure. hydrogen nitrogen oxygen chlorine State which one of these gases is green. The gases shown exist as diatomic molecules. State the name of another element which has diatomic molecules and is a gas at room temperature and pressure. When separate samples of each of these gases are placed in a container they will diffuse. Describe why these gases diffuse. State which of these four gases has the highest rate of diffusion. Explain your answer. gas explanation  Nitrogen, oxygen and other substances are found in clean, dry air. State the percentage of nitrogen in clean, dry air. Other than nitrogen and oxygen, identify another element found in clean, dry air. Identify a compound found in clean, dry air. Nitrogen and oxygen can be separated from liquid air. State the name of this process. 
10. Chemistry of the environment  →  10.3. Air quality and climate
1. States of matter  →  1.2. Diffusion
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
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3
This question is about ammonia. Nitrogen reacts with hydrogen to form ammonia in an industrial process. N2+ 3H22NH3Name this industrial process. State the meaning of the symbol . State the conditions used in this industrial process. Include units. temperature pressure  Name the catalyst used in this industrial process. If the pressure is increased, the yield of ammonia increases. Explain why, in terms of equilibrium. If the temperature is increased, the rate of reaction increases. Explain why, in terms of particles. Ammonia reacts with sulfuricacid to make a compound which is used as a fertiliser. Write the chemical equation for the reaction between ammonia and sulfuricacid. 
6. Chemical reactions  →  6.3. Reversible reactions and equilibrium
6. Chemical reactions  →  6.2. Rate of reaction
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4
A student wanted to make some zincchloride crystals. The student followed the procedure shown. step 1 Add excess zinc powder to dilute hydrochloricacid to form aqueous zincchloride. step 2 Remove unreacted zinc powder from the aqueous zincchloride. step 3 Heat the solution until it is saturated. step 4 Allow the saturated solution to cool and remove the crystals that form. Write the equation for the reaction in step1. Include state symbols. Explain why excess zinc powder is added in step1. Suggest how unreacted zinc powder is removed in step2. A saturated solution is formed in step3. Suggest what is meant by the term saturated solution. Explain why crystals form as the solution cools in step4. Name two zinc compounds which react with dilute hydrochloricacid to form zincchloride. If excess calcium metal is used instead of excess zinc powder in step1, pure calciumchloride crystals do not form. Explain why. Some salts can be made by titration. In a titration experiment, 20.0 cm3 of aqueous sodiumhydroxide reacts exactly with 25.0 cm3 of 0.100 mol / dm3 dilute sulfuricacid to make sodium sulfate. 2NaOH+ H2SO4→ Na2SO4+ 2H2OCircle the name of the type of reaction that takes place. decomposition neutralisation precipitation reduction  Calculate the concentration of the aqueous sodiumhydroxide in g / dm3 using the following steps. ● Calculate the number of moles of dilute sulfuricacid used.  mol ● Determine the number of moles of sodium hydroxide which react with the dilute sulfuricacid.  mol ● Calculate the concentration of the aqueous sodiumhydroxide in mol / dm3.  mol / dm3 ● Calculate the concentration of the aqueous sodiumhydroxide in g / dm3.  g / dm3  
12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases
9. Metals  →  9.4. Reactivity series
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5
The table shows the names or structures of organic compounds P to U. P Q R H C H H C H H C H H H propanoic acid but-1-ene S T U propan-1-ol methyl butanoate C C H C H H H H H Give the letters of the organic compounds, P to U, that are unsaturated hydrocarbons. Describe the test for an unsaturated hydrocarbon. test observations  But-1-ene is an unbranched molecule. Name the unbranched isomer of but-1-ene. Draw the structure of a branched isomer of but-1-ene. Show all of the atoms and all of the bonds.  Dodecane is an alkane with 12 carbon atoms. Dodecane can be cracked. Write the formula of dodecane. Give the letters of all the organic compounds, P to U, that can be formed when dodecane is cracked. Name the reagent and suggest the conditions needed to convert organic compoundU into organic compoundS. reagent conditions  Organic compoundS can be converted to organic compoundQ by reaction with an acidified reagent. Name the type of chemical change that happens to organic compoundS. Name the acidified reagent added to organic compoundS. Organic compoundT is made by reacting two compounds together. Name the homologous series that organic compoundT belongs to. Name the two compounds which react together to make organic compoundT. Draw the structures of each compound you have named. Show all of the atoms and all of the bonds. name structure name structure  Deduce the molecular formula of organic compoundT. 
11. Organic chemistry  →  11.2. Naming organic compounds
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6
Polymers are large molecules built up from small molecules. State the name given to the small molecules from which polymers are made. The formula of a polymer is shown. n C CH3 C CH3 H H Draw the structure of the small molecule from which this polymer is made. Show all of the atoms and all of the bonds.  State the type of polymerisation used to make this polymer. Three amino acids are shown. They combine to form part of a natural polymer. H2N COOH H2N COOH H2N COOH Name the type of natural polymer formed when amino acids combine. Complete the diagram to show part of the structure of the natural polymer that forms when these three amino acids combine. Show all of the bonds in the linkages.  Name the type of chemical reaction that takes place when this natural polymer is converted back to amino acids. 
11. Organic chemistry  →  11.8. Polymers
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