Chemistry Paper 3 Questions and Answers With Confidential - Cekana Mock Exams 2023

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INSTRUCTIONS

  • All working must be clearly shown where necessary.
  • You are not allowed to start working with the apparatus for the first 15 minutes. This time is to enable you read the question paper and make sure you have all the requirements.


QUESTIONS

  1. You are provided with:
    • Magnesium ribbon solid E
    • 2M hydrochloric acid, solution F
    • 0.375M sodium hydroxide, solution H
      You are required to determine
      1. The rate of reaction between magnesium and hydrochloric acid
      2. The mass of 1cm length of magnesium ribbon

PROCEDURE 1

Step 1: Cut out five pieces of exactly 1cm length of magnesium ribbon solid E. Carefully fill the burette with solution F.
Step 2: Drain from the burette 10cm3 solution F into a test tube. Put one piece of magnesium ribbon into the tube and                                immediately start a stopwatch. Record the time taken for the magnesium ribbon to completely react.
Step 3: Transfer all the contents of the test tube into a 250ml volumetric flask. Rinse the test tube with distilled water and put in into the volumetric flask.
Step 4: Repeat step 2 and 3 by placing 9cm3 of solution F and 1cm3 of distilled water shake the contents before use. After each experiment transfer the mixture into the volumetric flask.

Repeat the procedure using contents in test tube 3, 4 and 5 as shown in the table below.
RETAIN THE SOLUTION IN THE VOLUMETRIC FLASK FOR USE IN PROCEDURE II
Table I

Test tube number

1

2

3

4

5

Volume of solution F(cm3)

10

9

8

7

6

Volume of water added (cm3)

0

1

2

3

4

Time taken (seconds)

         

(sec-1)

         

(5mks)

  1.  
    1. Plot a graph of rate(1⁄7) , against volume of solution F. (3mks)
      chemcekena.png
    2. Use the graph to determine the time taken for 1cm length of magnesium to dissolve if volume of water added is 1.5cm3 . (2mks)
    3.  
      1. In terms of rate of reaction, explain the shape of the graph (2mks)

PROCEDURE II
Add distilled water into the solution in the 250ml volumetric flask up to the mark. Label it as solution G.
Clean the burette and fill it with Sodium hydroxide, solution H.
Pipette 25cm3 of solution G into 250ml conical flask. Add 2 drop of phenolphthalein indicator and titrate it with solution H from the burette.
Record your results in table below
Table II

 

I

II

III

Final burette reading (cm3)

     

Initial burette reading (cm3)

     

Volume of solution H used (cm3)

     


(4mks)

    1.  Determine the
      1. Average volume of solution H used. (1mk)
      2. Number of moles of hydrochloric acid in 250cm3 of solution G. (2mks)
      3. Number of moles of hydrochloric acid solution F that reacted with solid E. (2mks)
      4. The mass of magnesium ribbon that reacted. (Mg=24). (2mks)
      5. Mass of 1cm length magnesium ribbon. (1mk)

2 . You are provide with solid K. Carry out the following tests and record your observations and inferences in the spaces provided.

  1. Place all solid K into a boiling tube. Add about 5cm3 of distilled water and shake the mixture.
    Observation Inferences

    Observation

    Inferences

    (1mk)

    (1mk)

  2. To about 2cm3 of the solution K , add half a spatula of sodium hydrogen carbonate.

    Observation

    Inferences

    (½mk)

    (½mk)

  3. To the remaining solution K, add about 10cm3 of dilute hydrochloric acid. Shake thoroughly. Filter the mixture then wash the residue with distilled water. Dry the residue with filter paper.
    1. Place one third of the residue into a test tube. Add about 10cm3 of distilled water and shake the mixture. Add half a spatula sodium hydrogen carbonate.

      Observation

      Inferences

      (½mk)

      (½mk)

    2. To the remaining residue add 5cm3 of distilled water then 5cm3 of sulphuric (VI) acid, followed by 5cm3 of ethanol and warm the mixture.

      Observation

      Inferences

      (1mk)

      (1mk)

3. You are provided with solid L carry out the following test and record your observations and inferences in the space provided.

  1. Place one third of the solid L in a dry test tube. Heat it and test any gas produced with blue and red litmus paper.
    Observation Inferences

    Observation

    Inferences

    (2mks)

    (1mk)

  2. Place the remaining solid L in a boiling tube. Add about 10cm3 of distilled water and shake. Divide the solution in to four portions.
    1. To about 2cm3 of solution L add 2 drops of barium chloride solution

      Observation

      Inferences

      (1mk)

      (1mk)

    2. To about 2cm3of solution L add 5 drops of dilute hydrochloric acid

      Observation

      Inferences

      (1mk)

      (1mk)

    3. To 2cm3 of solution L add ammonia solution drop wise until in excess

      Observation

      Inferences

      (1mk)

      (1⁄2mk)

    4. To 2cm3 of solution L add sodium hydroxide drop wise until in excess

      Observation

      Inferences

      (1mk)

      (½mk)



CONFIDENTIAL

  1.  Solid E
  2. 50cm3of solution F
  3. 80cm3of solution H
  4. 0.5g of solid K
  5. 0.5g of solid L
  6. Distilled water
  7. Burette
  8. Pipette
  9. Pipette filter
  10. Label
  11. 250ml volumetric flask
  12. Two 250ml conical flasks
  13. Test tube holder
  14. 2 boiling tube
  15. 6 test tubes
  16. Stopwatch
  17.  10ml measuring cylinder
  18.  Spatula
  19.  0.5g sodium hydrogen carbonate
  20.  5cm3of ethanol
  21.  Filter paper – 3 pieces
  22.  Filter funnel
  23.  Blue and red litmus paper
    Access to
    1. 0.1M BaCl2
    2. 2M HCl
    3.  2M Ammonia solution
    4. 2M NaOH
    5. 2M H2SO4 acid
    6. Source of heat
    7. Phenolphthalein indicator
      Preparations
      1. Solid E – 5cm magnesium ribbon
      2. Solution F – 2M HCl
      3. Solution H – 0.375M NaOH
      4. Solid K – sodium benzoate
      5.  Solid L-Ammonium aluminium sulphate


MARKING SCHEME

Procedure I

Table 1…………………………….5 mks

Test-tube number

1

2

3

4

5

Volume of solution F cm3

10

9

8

7

6

Volume of water

0

1

2

3

4

Time (sec)

35.6

41.0

50.2

52.3

66.2

 1/time sec-1

0.0280

0.0243

0.0199

0.0191

0.0151

  1. Complete table (time)……..1mk
    complete table 1
    incomplete table (3-4) ½
  2. Decimal (Time) ……..½mk
    Either whole number, 1d.p or 2d.p
    Consistently written ½
    Otherwise ward 0mk
  3. Accuracy ….(experiment 1 ) ------½mk
    - compare candidates value with S.V of experiment 1. It should be within ±2 units otherwise award 0mk
  4. Trend (time)……½mk
    Continuous increase
  5. 1/ time (sec-1) ……..2½mk
    . Each correct conversion is ½mk
    Condition
    To be at least 3d.p

  1.  
    1. Graph
      • Labelling Axes…………..½mk
      • Scale………………………½mk
        Uniform scale, otherwise 0mk
        Plots to occupy at least half of grid in both axis
      • Plots…………………………………..1mk
        5 correctly plotted points
        3-4 correctly plotted points 
        Less than 3 points plotted 0mk
      • Line ………………………1mk
        Straight line passing through (0,0)
        Otherwise 0mk
    2. Show 
      recording 
      reciprocal 
      correct ans
    3. Rate is directly proportional to concentration of acid increase in the concentration of the acid increases the number of effective collisions per unit time
      Procedure II
      Table 2…………………5mks
      • Complete table …………………….1mk
        3 titration 
        2 titration 
        Penalties
        - Inverted table
        - Burette reading beyond 50cm3 unless explained
        - Volume of 1cm3 and below
      • Decimal………..1mk
        1d.p written consistently otherwise 0mk
      • Accuracy …………….1mk
        Any within ± 0.1 of s.v
        - Outside ±0.1 but within ±0.2 of s.v
        - Outside ±0.2………….0mk
      • Principle of averaging……………..1 mk
        Values within ±0.2 of each other 
        i.e working 
        Answer 
      • Final answer ………..1mk
        Average value within
        ±0.1of s.v
        ±0.2 of s.v
  2.  
    1.  
      AV × 0.375/ 1000 =ans(x)
      1:1 or equation
      ans(x) × 250/25
    2. 2 × 40/ 1000 =0.08
      0.08-ans(y)
    3. mg:HCL=1:2
      mole of mg = ansb(iii)/ 2
    4. ans(B)/ 5=ans(C)

2. 

  1.  

    Observation

    Inferences

    Dissolves ü1 to form a colourless solution

    polar

  2.  

    Observation

    Inferences

    No effervescence

    absent 

  3.  
    1.   

      Observation

      Inferences

      Effervescence

      R-COOH/H+ 


    2. Observation

      Inferences

      Pleasant smelling compound 

      Reject sweet

      R-COOH


  1.   

    Observation

    Inferences

    Colourless liquid formed on cooler part of boiling tube

    Colourless gas with pungent/ chocking smell

    Red litmus changes to blue

    Blue litmus paper persists

    White residue

    Hydrated salt/ solid

    NH+4

  2.  
    1.    

      Observation

      Inferences

      White ppt

      SO2-4CO2-3,SO2-3

    2.   

      Observation

      Inferences

      No effervescenceü

      SO2-4

    3.   

      Observation

      Inferences

      White ppt

      Insoluble in excess

      Mg2+ü½ Al3+

       

    4.  

      Observation

      Inferences

      White ppt 

      Soluble in excess 

      Al3+ü½

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