MOKASA Joint Evaluation Examination Chemistry Paper 1 2016- Pre MOCK with answers

Share via Whatsapp
  1. Explain the following:
    1. It is always advisable to scoop chemical substances using a clean spatula. ( ½ mark)

       To prevent contamination of the chemicals.

    2. Flammable substances should always be kept away from flames in the laboratory. ( ½ mark)

      To prevent fire accidents.

  2. Name one reagent that can be used to distinguish between Al3+ and Zn2+ ions in solution and state what would be observed if each of the ions is treated with the reagent you have named. (3 marks)

     Ammonia solution

    Al3+ - A white precipitate would be formed which is insoluble in excess ammonia solution.

    Zn2+ - A white precipitate would be formed which is insoluble in excess ammonia solution.

  3. Manganese sulphide reacts with acids according to the following equation.

    manganese sulphide mokasa 2016
    State, giving a reason what would happen to the equilibrium if;
    1. Water is added to the equilibrium mixture. (1 ½ marks)

       Increasing the concentration of water would shift the equilibrium to the left.

    2. Hydrogen chloride is bubbled into the equilibrium mixture. (1 ½ marks)

       HCl would react with the H2S thereby reducing its concentration.  The equilibrium would shift to the right.

  4. Use the thermochemical equations below to answer the questions that follow.

    thermochemical equation mokasa 2016

    1. Draw an energy cycle diagram to show the enthalpy of formation of ethane. (1 ½ marks)
    2. Calculate the enthalpy of formation of ethane. (1 ½ marks)

       ΔHf  = ΔH1 + ΔH2 - ΔH3
             
        = (2 x - 394) + (3 x -286) - 1560
              = -788 + -856 - -1560
              = -1646 + 1560
              = -86 kJ/mole

  5. State the conditions under which copper reacts with sulphuric acid and give an equation for the reaction. (2 marks)

    The acid must be concentrated and hot 
    Cu(s) + H2SO4(l) --------> CuSO4(aq) + SO2(g) + H2O(l)

  6. When 8.8g of hydrocarbon Z was burnt in excess air, 14.4g of water and 11.95 dmof carbon (IV) oxide were obtained at s.t.p. Determine the empirical formula of Z. (3 marks)

     mokasa16pp1a6

  7. Perspex is a synthetic polymer of formula

    perspex mokasa 2016

    1. Write the structural formula of the monomer of Perspex. (1 mark)

       mokasa16pp1a7a

    2. State the type of polymerization involved in the formation of perspex. (1 mark)

       Addition polymerization

  8. When zinc granules are dropped into two separate solutions of dilute sulphuric (VI) and concentrated sulphuric (VI) acid, effervescence of a colourless gas occurs in each case. Give equations to represent the reactions that take place. (2 marks)

    Zn(s) + H2SO4(aq) ---------> ZnSO4(aq) + H2(g)
    Zn(s) + 2H2SO4(l) ---------> ZnSO4(aq) + SO2(g) + 2H2O(l)

  9. Study the chart below and answer the questions that follow.

    copper sulphate reaction mokasa 2016

    1. Identity solid X. (1 mark)

       Hydrated iron (III) oxide

    2. Write an ionic equation for the reaction between P and copper (II) sulphide solution. (1 mark)

       H2S(g)  +  Cu2+(aq)  --------------->  CuS(s)   +  2H+(aq)

    3. State the observation made when gas P is bubbled through iron (III) chloride solution. (1 mark)

       The yellow iron (III) chloride solution turns green.

  10. Use the nuclear equations below to answer the questions that follow.

    nuclear equations mokasa 2016

    1. Give the actual names of particles X and Y. (1 mark)

       X -  Alpha particles

       Y   Beta particles

    2. Give the name of a radiation whose emission does not change the mass number or the atomic number of a radioisotope. (1 mark)

       Gamma radiatons

  11. The structures below represent two cleaning agents M and P.

    cleansing agents mokasa 2016
    Which cleaning agent would be most suitable for use with water containing calcium sulphate. Give a reason. (2 marks)

     P – when used with hard water it does not form scum.

  12. You are given the following half equations:

    cell reactions mokasa 2016

    1. Obtain an equation of the cell reaction. (1 mark)

       Mg(s)  +  Zn2+(aq)  ------------>    Mg2+(aq)  +  Zn(s)

    2. Calculate the value Eϑ for the cell. (1 mark)

       E.m.f = Eϑ reduced - Eϑ oxidised
               = -0.76 + 2.37
               = +1.61V

    3. Give the oxidizing species. (1 mark)

       Zn2+ ion

  13. Using dots (.) and crosses (×) to represent outermost electrons; draw diagrams to show bonding in:
    1. Aluminium chloride. (1 ½ marks)
    2. Sulphuric (IV) oxide. (1 ½ marks)

  14. Use the information in the table below to answer the questions that follow.

    Melting point  Element  Atomic number 
     97.8  R  11
     660  S  13
     1440  T  14
     -40.1  U  17
     63.1  V  19


    1. Write the electron arrangement of: (1 mark)
      1. ion of S

         2.8

      2. atom of T

         2.8.4

    2. Explain why the melting point of T is higher than that of U. (2 marks)

      Atoms are covalently bonded together to form a giant atomic structure.  Atoms of U are bonded covalently to form molecules.  The molecules are then hold together by weak Van der waals to form a simple molecule structure.

  15. Complete the table below. (3 marks)

    Metal Aluminium Lead Sodium
    Chief Ore Bauxite

    Galena

    Rock salt
    Chemical name

    Al2O3.2H2O

    PbS

    NaCl

    Method of extraction 

    Electrolysis

    reduction

    Electrolysis



  16. The diagram below represents a set up used for the large scale manufacture of hydrochloric acid.

    manufacture of hydrochloric acid mokasa 2016
    1. Name substance X. (1 mark)

       Hydrogen

    2. What is the purpose of the glass beads? (1 mark)

       They increase the surface area over which the gas dissolves in water.

    3. Give one use of hydrochloric acid. (1 mark)

      -Treatment of water at the water works
      -Sewage treatment
      -Manufacture of dyes, drugs etc
      -To clean metal surfaces to remove rust

  17. Calculate the volume of nitrogen (I) oxide produced when 38.2g of ammonium nitrate is completely decomposed by heating (at s.t.p). (N = 14, H = 1, O = 16) (3 marks)

     mokasa16pp1a17

  18. Give equations to show the reactions that take place when;
    1. iron reacts with steam. (1 mark)

       3Fe(s)  +  4H2O(g)  --------->     Fe3O4(s)   +  4H2(g)

    2. Give one industrial use of the gas produced in the reactions in (i) and (ii) above. (1 mark)

      -Industrial manufacture of hydrochloric acid
      -Industrial manufacture of Ammonia
      -Used in weather balloons

    1. When magnesium metal is burnt in air, it reacts with both oxygen and nitrogen gases giving a white ash. Write two equations for the reactions that take place. (2 marks)

      2Mg(s) + O2(g) -------> 2MgO(s)
      3Mg(s) + N2(g) --------> Mg3N2(s)

    2. Give the total number of atoms present in the gas produced when water is added to magnesium nitrate. (1 mark)

       Four

  19. The graph below shows the behavior of a fixed mass of a gas at constant temperature.

    gas laws mokasa 2016
    1. What is the relationship between the volume and the pressure of the gas? (1 mark)

       At constant temperature, the volume of a fixed mass of gas is inversely proportional to pressure or  V  α  1/p   ,  V  = K/P

    2. 60 cm3 of oxygen gas diffused through a porous partition in 50 seconds. How long would it take 60 cmof sulphur (IV) oxide gas to diffuse through the same partition under the same conditions? (S = 32.), O = 16.0) (3 marks)

       mokasa16pp1a20b

  20. State and explain the observation made when a moist red litmus paper is put in a gas jar of dry chlorine gas. (2 marks)

     The red litmus paper is bleached.  This is because chlorine gas has bleaching property.

    1. When extinguishing a fire caused by burning kerosene, carbon (IV) oxide is preferred to water. Explain. (2 marks)

       Kerosene floats on water therefore it continues to burn.  Carbon (IV) oxide cuts off the supply of oxygen.

    2. Write the formula of the oxide of carbon which is ‘silent killer’. (1 mark)

       CO

  21. Explain why chlorine is a gas while iodine is a solid at room temperature. (2 marks)

     The molecules of chlorine are smaller compared to those of iodine; thus the strength of the intermolecules forces of attraction in iodine are much stronger than in chlorine.

  22. Apart from their location, state any two differences between a proton and an electron. (2 marks)

    A proton is positively charged whereas an electron is negatively charged.
    The mass of a proton is/atomic mass units whereas that of an electron is 1/1840 a.m.u

  23. What term is given to: The amount of energy given out when a neutral atom in gaseous state gains an electron? (1 mark)

     Electron affinity

  24. A certain fertilizer is suspected to be containing nitrate ions. Describe how the presence of nitrate ions can be determined in such fertilizer. (3 marks)

     Add water to a small sample of the fertilizer in a test tube and shake well.  Filter to obtain a solution.  To the solution add some freshly prepared ion (II) sulphate solution and shake well.  With a test tube in a slanting position, add concentrated sulphuric (VI) acid to the mixture carefully along one side of the tube.  A brown ring between two layers indicates the presence of nitrate ions.

  25. Write balanced chemical equations to show the action of heat on the following nitrates.
    1. Lead (II) nitrate (1 mark)

       2Pb(NO3)2 (s) 2PbO(s)   +  4NO2(s)    +  O2(g)

    2. Silver nitrate (1 mark)

       2Ag NO3(s)   --------->     2Ag(s)  +2NO2(g)   +   O2(g)

  26. What is an amphoteric oxide? (1 mark)

     An oxide that behaves as an acid or a base in chemical reactions.

  27. Starting with zinc carbonate solid describe how zinc hydroxide can be prepared in the laboratory. (3 marks)

     Heat the zinc carbonate  solid in a test tube to obtain zinc oxide.  To a certain volume of dilute nitric (V) acid the zinc oxide a little at a time while stirring till in excess.  Filter the unreacted zinc oxise.  To the filtrate add aqueous

  28. Below is a scheme of some reactions starting with but-z-yne. Study it and answer the questions that follow.

    alkanols reactions mokasa 2016

    1. Name Y, X and T (1 ½ marks)

       Y Chlorine gas

       X Hydrogen gas

       T Butyl hydrogen sulphate

    2. Give the name of the following organic compounds. ( ½ mark)

      alkanols mokasa 2016

       Ethanoic acid

      alkanols mokasa 2016

       Ethylpropanoate

      alkanols mokasa 2016

       Sodium ethanoate

  29. The following results were obtained during an experiment to determine the solubility of potassium nitrate in water at 30oC. Mass of dish = 15.86g, mass of dish + saturated
    solution at 30oC = 26.86g, mass of dish + solid KNO3 after evaporation to dryness = 16.7g. Calculate the mass of saturated solution containing 60.0g of water at 30o C. (3 marks)

     mokasa16pp1a31

Join our whatsapp group for latest updates

Download MOKASA Joint Evaluation Examination Chemistry Paper 1 2016- Pre MOCK with answers.


Tap Here to Download for 50/-




Why download?

  • ✔ To read offline at any time.
  • ✔ To Print at your convenience
  • ✔ Share Easily with Friends / Students


Get on WhatsApp Download as PDF
.
Subscribe now

access all the content at an affordable rate
or
Buy any individual paper or notes as a pdf via MPESA
and get it sent to you via WhatsApp

 

What does our community say about us?

Join our community on:

  • easyelimu app
  • Telegram
  • facebook page
  • twitter page
  • Pinterest