Form 4 Chemistry Paper 2 Endterm 1 Exam 2023

Get the Answers here Form 4 End Term 1 Exams 2023 Questions and Answers

.  The grid below represents part of the periodic table.  Study it and answer the questions that

      follow.

     (a)  Identity the family name to which element F and G belong.                                      (1 mk)

                        Alkaline earth metals

     (b)  Name the type of bond formed when a and F belong.                                                (1 mk)

                        Ionic bond

     (c)  Write the formula of the oxide formed when D reacts with oxygen.             (1 mk)

                        D₂O₃

    (d)  What type of oxide is formed in (c)  above.                                                                (1 mk)

     (e)  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  

            to F.

     (f)  Element F burns in air to form two products.  Write two equations of the two products

            formed.                                                                                                                       (3 mks)

                        2F_(s)

₎                                   F₃N_2(s)

     (g)  Stat e 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.  (a)  Name the following organic compounds.

          (i)  CH₃CH₂CH(Br)CH₃

                   2, 3 – dibromo – 2 – chloropentane

(ii)  CH₃-CH₂CH₂-CH₂-C-OH

          Butanoic acid

(iii)  CH₂CHCH₂CH(Br)CH₃

            4 – bromopent-i-ene

     (b)  Study the flow chart below and answer the questions that follow.

(a)  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.

(i)  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.

            (ii)  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.

          (b)  The Standard enthalpy change of formation of methanol is -239Kjmol-1

            (i)  Write the thermal chemical equation for the standard enthalpy change of formation of

                  methanol.                                                                                                              (1 mk)

C_(s) + 2H_2(g)  +  ½ O_2(g)                      H₃OH_(g)

            (ii)  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 O_2(g)                     CO₂;    H^ɵ  = -283Kj/mol

                        H_2(g)  +  ½ O_2(g)                       H₂O_(l); =  H^ɵ = -286Kj/mol

                        CH₃OH  +                         CO_2(g)  +  2H₂O; H^ɵ = -715Kj/mol

                        C   +  2H₂            +         ½ O₂                      CH₃OH

                        H= -283Kj/mol       

                                    O₂                       O₂                     O₂

                                      CO₂ + H₂O

                        _σCH₃OH   = H_cC  +  H_cH₂  –  H_cCH₃OH

                                    = -283 + 2(-286) – (-715)

                                    = -283 – 576 + 715

                                    = -859 + 715

                                    _f CH₃OH = – 144Kj/mol

 (c)  Study the information given in the table below and answer the questions that follow.

            Calculate the enthalpy change for the reaction.                                                          (3 mks)

                        CH_4(g)  + Cl_2(g)                        CH₃Cl_(g) + HCl_(g)

                                     H                                              H

                                     │                                              │

                              H ─C─H  +  Cl─H                 H─C─Cl + H─Cl

                                     │                                              │

                                     H                                              H

                        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.

     (a)  (i)  Name solid X.                                                                                                        (1 mk)

                        Calcium carbonate

            (ii)  Write an ionic equation for the reaction of X and acid.                                      (1 mk)

                        CO₃^2-_(s)  +  2H⁺_(aq)                    CO_2(g) + H₂O_(l)

     (b)  A gas jar full of Carbon (IV) oxide was inverted over burning candle.

            (i)  State the observations made.                                                                                (1 mk)

                        Candle is immediately extinguished

            (ii)  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.

            (iii) Name a practical everyday use of this property of carbon (IV) oxide.               (1 mk)

                        As a fire extinguisher

     (c)  The flow diagram below shows some reactions of calcium compounds.

(i)  Give one condition other than the    of a catalyst that would favour the reaction in step I.                                                                                                                                             (1 mk)

                        High pressure

            (ii)  Name the catalysts used in step I and II.                                                             (2 mks)

                        Step I  –  finely divided iron

                        Step II – Vanadium V oxide/platinum

            (iii)  Name substances  P, Q, X and Y .                                                                      (2 mks)

                        P – ammonium sulplhate

                        Q – Copper metal

                        X – Oxygen

                        Y – nitrogen gas

            (iv)  Write equations for the reactions that takes kplace in step II.                            (3 mks)

                        4NH₃(g) + 5O_2(g)                                  4NO(g) + 6H2O_(l)

                        2NO(s) + O_2(g)                                    2NO₂

                        4NO_2(g) + 2H₂O_(g) + O_2(g)                     HNO_3(aq)

            (v)  Name the oxidizing agent for the reaction that takes place in step IV.               (1 mk)

                        Nitric acid

            (vi)  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.

                                                                         E^ɵ (volts)

          A²⁺_(aq)  +  2e-                         A_(s)             -2.90

          B²⁺_(aq)  + 2e-                           B_(s)             -2.38

          C⁺_(aq) + 2e-                             ½ C_(g)           -0.00

          D²⁺_(aq)  + 2e-                           D_(s)             +0.34

          ½ F_2(g)  +  e-                           F^–_(aq)           +2.87

            (i)  Which element is likely to be hydrogen? Give a reason for your answer.           (2 mks)

                        C⁺/C₂ = hydrogen is used as the reference electrode

                        E^ɵ value is 0.00/standard electrode potential

            (ii)  What is the E^ɵ value of the strongest reducing.                                                   (1 mk)

                        E^ɵ = -2.90V

            (iii) 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)

            (iv)  Calculate the E^ɵ 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

     (b)  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.

            (i)  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)

            (ii)  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)