Chemistry Paper 2 Questions and Answers - Moi Tea Mock Examinations 2022

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INSTRUCTIONS TO CANDIDATES:

  • Answer all the questions in the spaces provided.
  • Mathematical tables and electronic calculators may be used.
  • All working must be clearly shown where necessary.

 

  1. The grid below represents part of the periodic table. Study it and answer the questions that follow.
    Chemp02q01
    1. Identity the family name to which element F and G belong. (1 mk)
    2. Name the type of bond formed when a and F belong. (1 mk)
    3. Write the formula of the oxide formed when D reacts with oxygen. (1 mk)
    4. What type of oxide is formed in (c) above. (1 mk)
    5. Compare the atomic radii of F and D. Explain. (2 mks)
    6. Element F burns in air to form two products. Write two equations of the two products formed. (3 mks)
    7. State two uses of element K and its compounds. (2 mks)
  2.  
    1. Name the following organic compounds.
      1. CH3CH2CH(Br)CH3
      2. CH3-CH2CH2-CH2-C-O2H
      3. CH2CHCH2CH(Br)CH3
    2. Study the flow chart below and answer the questions that follow.
      Chemp02q02b
      Name:-
      1. The process that occur in steps marked I, II and IV. (1 mk)
      2. The reagent and conditions in step II. (1½ mks)
      3. Draw the structural formula of substance X, give the name of the substance. (2 mks)

    3. The diagram below shows a structure of a cleansing agent.
      Chemp02q02c
      1. Name the cleansing agent above. (1 mk)
      2. State the type of cleansing agent above. (1 mk)
      3. Name the material added to the cleansing agent in order to improve its cleansing property.
  3.  
    1. 50cm3 of 1M copper (II) Sulphate solution was placed in a 100cm3 plastic beaker. The temperature of the solution was measured. Excess metal A powder was added to the solution, the mixture stirred and the maximum temperature was repeated using powder of metal B and C. The results obtained are given in the table below.
         A
       Maximum temperature °C  2.63 31.7  22.0 
       Initial temperature (°C)  22.0 22.0  22.0 

      1. Arrange the metal A, B, C and Copper in order of reactivity starting with the least reactive. Give reasons for the order. (3 marks)
      2. Other than temperature change, state one other observation that was made when the
    2. The Standard enthalpy change of formation of methanol is -239Kjmol-1
      1. Write the thermal chemical equation for the standard enthalpy change of formation of
      2. Use the following data to calculate the enthalpy change for the manufacture of methanol from carbon (II) oxide and hydrogen. (3 mks)
        • CO(g) + ½ O2(g) CO2; ∆Hɵ = -283Kj/mol
          H2(g) + ½ O2(g) H2O(l); = ∆Hɵ = -286Kj/mol
          CH3OH + 32 CO2(g) + 2H2O; ∆Hɵ = -715Kj/mol
    3. Study the information given in the table below and answer the questions that follow.
       Bond  Bond energy (Kjmol-1)
       C – H
      Cl – Cl
      C – Cl
      H - Cl
       414
      244
      326
      431
      Calculate the enthalpy change for the reaction. (3 mks)
  4. Carbon IV oxide is produced when solid X is heated strongly. It can also be prepared by adding dilute hydrochloric acid to solid X. The reaction between X and dilute Sulphuric acid, however gradually slows down and stops.
    1.      
      1. Name solid X. (1 mk)
      2. Write an ionic equation for the reaction of X and acid. (1 mk)
    2. A gas jar full of Carbon (IV) oxide was inverted over burning candle.
      1. State the observations made. (1 mk)
      2. What two properties of carbon (IV) oxide does this observation illustrate. (2 mks)
      3. Name a practical everyday use of this property of carbon (IV) oxide. (1 mk)
    3. The flow diagram below shows some reactions of calcium compounds.
      Chemp02q04c
      1. Name compound F and G. (2 mks)
      2. Write equations for reactions in step A, B and C. (3 mks)
  5.     
    1. A piece of sodium metal which had been exposed to air, was found to be covered with a white powder. The piece was dropped into 50g of ethanol and 2400cm3 of hydrogen gas measured at room temperature and pressure was obtained. The unused ethanol was distilled off and a white solid remained (Na = 23, molar gas volume at room temperature and pressure = 24dm3)
      1. Name the other substance formed other than hydrogen. (1 mk)
      2. Calculate the mass of sodium that dissolved in ethanol. (2 mks)
      3. What mass of ethanol was distilled of assuming there was no loss during the process? (2 mks)
      4. The ethanol was distilled off at 80oC, while the white solid remained unaffected at this temperature. What is the difference in structure of ethanol and the white solid. (2 mks)
    2. Name another liquid which produces;
      1. Hydrogen with sodium metal. (1 mk)
      2. What difference would you observe if identical pieces of sodium were dropped
    3.  
      1. Name the white powder coating the original piece of sodium, explain how it was formed. (3 mks)
      2. Describe one test by which you could identify white powder which originally covered
  6. The scheme below shows various reactions starting with hydrogen and nitrogen. Study it carefully and answer the questions that follow.
    Chemp02q06i
    1. Give one condition other than the of a catalyst that would favour the reaction in step I. (1 mk)
    2. Name the catalysts used in step I and II. (2 mks)
    3. Name substances P, Q, X and Y . (2 mks)
    4. Write equations for the reactions that takes kplace in step II. (3 mks)
    5. Name the oxidizing agent for the reaction that takes place in step IV. (1 mk)
    6. Why is a concentrated nitric acid transported on aluminium container and not copper? (1 mk)
  7. Use standard electric potentials for elements A, B, C, D and F given below to answer the questions that follow.
       Eɵ (volts)
     A2+(aq) + 2e-  ⇌ A(s)
    B2+(aq) + 2e- ⇌B(s) 
    C+(aq) + 2e- ⇌ ½ C(g)
    D2+(aq) + 2e- ⇌ D(s) 
    ½ F2(g) + e- ⇌ F-(aq)
     -2.90
    -2.38
    -0.00
    +0.34
    +2.87

    1. Which element is likely to be hydrogen? Give a reason for your answer. (2 mks)
    2. What is the Eɵ value of the strongest reducing. (1 mk)
    3. In the space provided, draw a labeled diagram of the electrochemical cell that would be obtained when half-cells of elements B and D are combined. (3 mks)
    4. Calculate the Eɵ value of the strongest reducing agent. (2 mks)
  8. During the electrolysis of aqueous copper II Sulphate using copper electrodes, al current of
    1. Write an ionic equation for the reaction that took place at the anode. (1 mk)
    2. Determine the change in mass of the anode which occurred as a result of the electrolysis process. (C.u = 63.5, 1 Faraday = 96,500 coulombs) (2 mks)

Marking Scheme

  1. The grid below represents part of the periodic table. Study it and answer the questions that follow.
    1. Identity the family name to which element F and G belong. (1 mk)
      • Alkaline earth metals
    2. Name the type of bond formed when a and F belong. (1 mk)
      • Ionic bond
    3. Write the formula of the oxide formed when D reacts with oxygen. (1 mk)
      • D2O3
    4. What type of oxide is formed in (c) above. (1 mk)
      • Amphoteric oxide
    5. Compare the atomic radii of F and D. Explain. (2 mks)
      • Has a smaller atomic radius than F because D has more protons hence stronger nuclear attraction compared to F.
    6. Element F burns in air to form two products. Write two equations of the two products formed. (3 mks)
      • 2F(s) + O2(g) → 2FO(s)
      • 3F(s) + N2(g) → F3N2(s)
    7. State two uses of element K and its compounds. (2 mks)
      • K cyanide is used in the extraction of gold
      • Mixture of K and potassium is used as nuclear coolant.
  2.        
    1. Name the following organic compounds.
      1. CH3CH2CH(Br)CH3
          • 2, 3 – dibromo – 2 - chloropentane
      2. CH3-CH2CH2-CH2-C-O2H
        • Butanoic acid
      3. CH2CHCH2CH(Br)CH3
        • 4 – bromopent-i-ene
    2. Study the flow chart below and answer the questions that follow.
      Name:-
      1. The process that occur in steps marked I, II and IV. (1 mk)
        • I – cracking
        • II- Hydrogenation
        • IV – Oxidation
      2. The reagent and conditions in step II. (1½ mks)
        • Reagent – hydrogen
        • Conditions – temp 150 – 250oC, nickel catalyst
      3. Draw the structural formula of substance X, give the name of the substance. (2 mks)
        Chemp02q02biii
    3. The diagram below shows a structure of a cleansing agent
      1. Name the cleansing agent above. (1 mk)
        • Sodium alkylbenzene sulphonate
      2. State the type of cleansing agent above. (1 mk)
        • Soapless detergent
      3. Name the material added to the cleansing agent in order to improve its cleansing property.
        • Tetraoxophosphate materials
  3.        
    1. 50cm3 of 1M copper (II) Sulphate solution was placed in a 100cm3 plastic beaker. The temperature of the solution was measured. Excess metal A powder was added to the solution, the mixture stirred and the maximum temperature was repeated using powder of metal B and C. The results obtained are given in the table below.
      1. Arrange the metal A, B, C and Copper in order of reactivity starting with the least reactive. Give reasons for the order. (3 marks)
        • C, Copper, A, B.
        • B is the most reactive because it has highest ∆T.
        • C is the least reactive because it cannot displace ions of copper from solution.
        • A is more reactive than Copper because it displaces Cu2+ from solutions.
      2. Other than temperature change, state one other observation that was made when the most reactive metal was added to the copper (II) Sulphate solution. (1 mk)
        • Blue colour of the solution fades /disappeared
        • Black deposit is formed.
    2. The Standard enthalpy change of formation of methanol is -239Kjmol-1
      1. Write the thermal chemical equation for the standard enthalpy change of formation of methanol. (1 mk)
        • C(s) + 2H2(g) + ½ O2(g) → H3OH(g) ∆H= -239Kjg/mol
      2. Use the following data to calculate the enthalpy change for the manufacture of methanol from carbon (II) oxide and hydrogen. (3 mks)
        • CO(g) + ½ O2(g) → CO2; ∆Hɵ = -283Kj/mol
          H2(g) + ½ O2(g) → H2O(l); = ∆Hɵ = -286Kj/mol
          CH3OH + 3/2 → CO2(g) + 2H2O; ∆Hɵ = -715Kj/mo
        •        
          Chemp03qa03bii
          ∆HσCH3OH = ∆HcC + ∆HcH2 - ∆HcCH3OH
          = -283 + 2(-286) – (-715)
          = -283 – 576 + 715
          = -859 + 715
          ∆Hf CH3OH = - 144Kj/mol
    3. Study the information given in the table below and answer the questions that follow.
      Calculate the enthalpy change for the reaction. (3 mks)
      •            
        Chemp02q03d
        Bond breaking energy – Bond formation energy
        BBE - BFE
        4(414) + 244 = 3 (414 + 326 + 431
        (1900 – 1999) = -99Kj
        = -99Kj
  4. Carbon IV oxide is produced when solid X is heated strongly. It can also be prepared by adding dilute hydrochloric acid to solid X. The reaction between X and dilute Sulphuric acid, however gradually slows down and stops.
    1.        
      1. Name solid X. (1 mk)
        • Calcium carbonate
      2. Write an ionic equation for the reaction of X and acid. (1 mk)
        • CO32-(s) + 2H+(aq) → CO2(g) + H2O(l)
    2. A gas jar full of Carbon (IV) oxide was inverted over burning candle.
      1. State the observations made. (1 mk)
        • Candle is immediately extinguished
      2. What two properties of carbon (IV) oxide does this observation illustrate. (2 mks)
        • It does not support combustion and it is denser than air since it is poured downwards from gas jar.
      3. Name a practical everyday use of this property of carbon (IV) oxide. (1 mk)
        • As a fire extinguisher
    3. The flow diagram below shows some reactions of calcium compounds.
      1. Name compound F and G. (2 mks)
        • F = Calcium carbonate
          G = Calcium hydroxide
      2. Write equations for reactions in step A, B and C. (3 mks)
        • Step A: CaCO3(s) + H2O(l) + CO2(g) → Ca(HCO3)2(aq)
          Step B: Ca(HCO3)2(aq) → CaCO3(s) + CO2(g) + H2O(l)
          Step C: Ca(OH)2(g) → CaCO3(s) + H2O
  5.        
    1. A piece of sodium metal which had been exposed to air, was found to be covered with a white powder. The piece was dropped into 50g of ethanol and 2400cm3 of hydrogen gas measured at room temperature and pressure was obtained. The unused ethanol was distilled off and a white solid remained (Na = 23, molar gas volume at room temperature and pressure = 24dm3)
      1. Name the other substance formed other than hydrogen. (1 mk)
        • Sodium ethoxide
      2. Calculate the mass of sodium that dissolved in ethanol. (2 mks)
        • 2C2H5OH(l) + 2Na(s) → 2C2H5ONa(l) + H2(g)
          2 moles Na gives 1 mole H2 at r.t.p.
          46g Na gives 24.000cm3
          2400cm3
          2400cm3 x 46g
          24000cm3 = 4.6g of sodium
      3. What mass of ethanol was distilled of assuming there was no loss during the process? (2 mks)
        • 2 moles of C2H5OH 1 mole of H2 gas
          (2 x 46)g C2H5OH gives 24000cm3
          X 2400cm3
          2 x 46 x 2400
          2400 = 9.2g
          Mass of distilled = (50g – 9.2g) = 40.8g
      4. The ethanol was distilled off at 80°C, while the white solid remained unaffected at this temperature. What is the difference in structure of ethanol and the white solid. (2 mks)
        • Ethanol is molecular structure with hydrogen bonds between molecules while white solid must be giant ionic structure with strong ionic bonds.
    2. Name another liquid which produces;
      1. Hydrogen with sodium metal. (1 mk)
        • Water
      2. What difference would you observe if identical pieces of sodium were dropped separately into small beakers containing ethanol and this other liquid? (2 mks)
        •  In ethanol  In water
           Sinks, gas bubbles are formed  Floats on surfaces, reacts vigorously and darts on surface producing a hissing sound.
    3.    
      1. Name the white powder coating the original piece of sodium, explain how it was formed. (3 mks)
        • Sodium in air forms sodium oxide, which in presence of moisture forms sodium hydroxide, which reacts with carbon (iv) oxide in air to form sodium carbonate.
      2. Describe one test by which you could identify white powder which originally covered sodium. (2 mks)
        • Add dilute HCl acid. Effervescence occurs and colourless gas is given off which forms a white precipitate in lime water.
  6. The scheme below shows various reactions starting with hydrogen and nitrogen. Study it carefully and answer the questions that follow.
    1. Give one condition other than the of a catalyst that would favour the reaction in step I. (1 mk)
      • High pressure
    2. Name the catalysts used in step I and II. (2 mks)
      • Step I - finely divided iron
        Step II – Vanadium V oxide/platinum
    3. Name substances P, Q, X and Y . (2 mks)
      • P – ammonium sulplhate
        Q – Copper metal
        X – Oxygen
        Y – nitrogen gas
    4. Write equations for the reactions that takes kplace in step II. (3 mks)
      • 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)
        2NO(s) + O2(g) → 2NO2
        4NO2(g) + 2H2O(g) + O2(g) → HNO3(aq)
    5. Name the oxidizing agent for the reaction that takes place in step IV. (1 mk)
      • Nitric acid
    6. Why is a concentrated nitric acid transported on aluminium container and not copper? (1 mk)
      • Concentrated nitric acid with copper oxidizes it to Copper(II) nitrate, while aluminium forms layer of aluminium oxide which is a passive and stops any further action by the acid.
  7. Use standard electric potentials for elements A, B, C, D and F given below to answer the questions that follow.
    1. Which element is likely to be hydrogen? Give a reason for your answer. (2 mks)
      • C+/C2 = hydrogen is used as the reference electrode
        Eɵ value is 0.00/standard electrode potential
    2. What is the Eɵ value of the strongest reducing. (1 mk)
      • Eɵ = -2.90V
    3. In the space provided, draw a labeled diagram of the electrochemical cell that would be obtained when half-cells of elements B and D are combined. (3 mks)
      Chemp02q07aiii
    4. Calculate the Eɵ value of the strongest reducing agent. (2 mks)
      • 2.38 + 0.34 = 2.72
        0.34 –(-2.38) = +2.72
        (0.34 + 2.38) = +2.72V
    1. During the electrolysis of aqueous copper II Sulphate using copper electrodes, al current of 0.2 amperes was passed through the cell for 5 hours.
      1. Write an ionic equation for the reaction that took place at the anode. (1 mk)
        • Cu(s) → Cu2+(aq) + 2e-
          or
          Cu(s) → Cu2+(aq)
      2. Determine the change in mass of the anode which occurred as a result of the electrolysis process. (C.u = 63.5, 1 Faraday = 96,500 coulombs) (2 mks)
        • C = AI
          (0.2 x 5 x 60 x 60)
          0.2 x 5 x 60 x 60 x 63.5
                    2 x 96500
          63 .5g Cu requires 2 x 96500
          3600 C produces 63. 5 x 3600
                                         2 x 96500
          = 1.18gm

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