9701_w21_qp_21 - revisedeck

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Sulfides are compounds that contain sulfur but not oxygen. Carbondisulfide, CS2, is a volatile liquid at room temperature and pressure. State the meaning of volatile. Draw a ‘dot-and-cross’ diagram of the CS2 molecule. Suggest the bond angle in a molecule of CS2. CS2 is a liquid under room conditions, while CO2 is a gas. Explain what causes the difference in the physical properties between CS2 and CO2. The enthalpy change of combustion of CS2is represented by the following equation. ∆Hc CS2+ 3O2CO2+ 2SO2Define enthalpy change of combustion. The table shows the enthalpy changes of formation of CS2, CO2and SO2. compound enthalpy change of formation, ∆Hf / kJ mol–1 CS2+89.7 CO2–394 SO2–297 Use the data in the table to calculate the enthalpy change of combustion, ∆Hc, of CS2, in kJ mol–1. Show your working. ∆Hc of CS2= kJ mol–1 Hydrogensulfide gas, H2S, is slightly soluble in water. It acts as a weak acid in aqueous solution. State the meaning of weak acid. Give the formula of the conjugate base of H2S. H2Sreacts slowly with oxygen dissolved in water. The reaction is represented by the following equation. H2S+ 1 2O2→ H2O+ SExplain, with reference to oxidation numbers, why this reaction is a redox reaction. The compound As2S3 is a common mineral. When As2S3 is heated strongly in air, it forms a mixture of products, as shown. 2As2S3+ 9O2→ As4O6+ 6SO2A sample containing 0.198 g As2S3 is placed in 0.100 dm3 of pure oxygen, an excess, in a reaction chamber connected to a gas syringe at room temperature. The reactants are heated until no further change is observed. The products are then allowed to cool to room temperature. Calculate the volume, in dm3, of gas present at the end of the experiment. The molar volume of gas is 24.0 dm3 mol–1 under these conditions. Assume that the pressure is constant throughout the experiment. Show your working. volume of gas remaining = dm3 State the environmental consequences of releasing SO2into the atmosphere. SO2can be removed from the air by reacting it with NaOH. Construct an equation for the reaction of SO2with NaOH. Include state symbols.

12. Nitrogen and sulfur → 12.1. Nitrogen and sulfur

5. Chemical energetics → 5.1. Enthalpy change, \(\Delta H\)

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The reaction scheme shows some reactions of calcium. CaCa(NO3)2CaOCa(OH)2reaction 1 heat CaCO3+ H2Oreaction 2 CO2CaC2reaction 4 Ca(HCO3)2reaction 3 excess CO2CHNO3 NaOHReaction1 produces Ca(NO3)2 and one other product. Identify the other product. Construct an equation for the thermal decomposition of Ca(NO3)2. State the trend in the thermal stability of the Group2 nitrates down the group. In reaction 3, excess CO2 is bubbled through water containing CaCO3. A solution of Ca(HCO3)2forms. Construct an equation for reaction3. Describe how Ca(OH)2 is used in agriculture. In reaction4, calciumcarbide, CaC2, is formed from CaO. CaC2 contains the C2 2– anion. Each carbon in C2 2– is sp hybridised. Describe how sp hybridised orbitals are formed. Sketch a diagram to show how two sp hybrid orbitals can form a sigma (σ) bond. The flowchart shows some reactions of CaC2. CaC2 CaCN2 NaCN CaCO3 + NH3 reaction 5 NaCl and C N2 H2O Reaction5 can be used to prepare NH3. CaCN2 + 3H2O → CaCO3 + 2NH3 Calculate the minimum mass, in tonnes, of calciumcyanamide, CaCN2, that is required to produce 1.50×106 tonnes of NH3. Show your working. 1 tonne = 1.00 × 106 g minimum mass of CaCN2 = tonnes Draw the structure of the organic products formed in the following reactions. CH3CH2Br NaCN dissolved in ethanol H2SO4heat under reflux NaCN and HCN O

11. Group 17 → 11.4. The reactions of chlorine

2. Atoms, molecules and stoichiometry → 2.4. Reacting masses and volumes (of solutions and gases)

15. Halogen compounds → 15.1. Halogenoalkanes

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Phosphorus is a reactive Period3 element. Phosphorus has several allotropes. Details of two allotropes are given. allotrope of phosphorus formula melting point / °C white P4 red P White phosphorus and red phosphorus both have covalent bonding. Suggest the types of structure shown by white phosphorus (P4) and red phosphorus (P). Explain why red phosphorus (P) has a higher melting point than white phosphorus (P4). structure of P4 structure of P explanation Red phosphorus (P) forms when white phosphorus (P4) is exposed to sunlight. 4 P4→ P∆H = –17.6 kJ mol–1 white red Use this information to draw a reaction pathway diagram to show the formation of red phosphorus (P) from white phosphorus (P4). enthalpy progress of reaction P4 Some reactions of P4are shown in the reaction scheme. P4PCl 5excess Cl 2excess O2P4O10Q reaction 2 H2OH2Oreaction 1 State the oxidation number of phosphorus in P4O10. Deduce the identity of Q and hence construct chemical equations for reactions 1 and 2. reaction 1 PCl 5 + H2O → reaction 2 P4O10 + H2O → Triphenylphosphine is used in a type of reaction known as a Wittig reaction. P triphenylphosphine where = –C6H5 Give the empirical formula of triphenylphosphine. In a Wittig reaction, an aldehyde reacts with a halogenoalkane to form an alkene. The conversion is shown in the following unbalanced equation. O + H R1 R2 R2 I R1 H triphenylphosphine strong base CompoundH can be made from propanal, C2H5CHO. Stage3 in the reaction scheme is a Wittig reaction. stage 1 C2H5CHO G triphenylphosphine NaBH4 stage 2 G C2H5CH2I stage 3 (Wittig reaction) H C2H5CH2I + C2H5CHO red phosphorus and I2 strong base State the types of reaction that occur in stages 1 and 2. stage 1 stage 2 Draw the structures of G and H in the boxes provided. G H Identify the organic products formed when compound J, shown below, is heated with hot concentrated acidified manganate(ions. hot concentrated MnO4 – H2SO4 J

9. The Periodic Table: chemical periodicity → 9.2. Periodicity of chemical properties of the elements in Period 3

14. Hydrocarbons → 14.2. Alkenes

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CompoundB is a liquid with a fruity smell. O B O Br The reaction scheme shows how B can be made from ethanol, C2H5OH. O B O Br O HO O HO Br C2H5OH and H2SO4 C2H5OH reaction 2 reaction 3 reaction 1 [O] Reaction1 is an oxidation reaction. Give the reagentand conditions required for reaction1. reagentconditions Construct an equation to represent reaction1. Use [O] to represent an oxygen atom from the oxidising agent in this reaction. Suggest the type of reaction that occurs in reaction2. H2SO4 acts as a homogeneous catalyst in reaction3. Explain why H2SO4 is described as homogeneous. Reaction2 needs to take place in the absence of water to prevent formation of compound C. O C HO OH If C is present in the reaction mixture of reaction3, a different compound, compoundD, will also form. CompoundD has two identical functional groups. The infrared spectrum of D shows strong absorptions at 1100 cm–1 and 1720 cm–1, but no absorption due to O–H bonds. Use the Data Booklet to identify the functional group present in D. Explain your answer as fully as you can. Some other reactions of C are shown. O C HO OH Na2CO3 E F (CH2OH)2 G (CH2Cl )2 SOCl 2 Draw the structure of E. Suggest why NaBH4 is not a suitable reagent to make F, (CH2OH)2, from C. Explain your answer. Construct an equation for the reaction of (CH2OH)2 with SOCl 2 to form G, (CH2Cl )2. Explain why C is very soluble in water.

18. Carboxylic acids and derivatives → 18.1. Carboxylic acids

8. Reaction kinetics → 8.3. Homogeneous and heterogeneous catalysts

17. Carbonyl compounds → 17.1. Aldehydes and ketones

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