KCSE Past Papers 2021 Chemistry paper 2(233/2)

Chemistry - Paper 2 2021 - 2 Hours

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Kenya certificate of Secondary Education

2021 Chemistry paper 2

1. Table 1 gives the properties of two compounds, A and B.

a. Table 1


A
   
B   
   
white, crystalline, efflorescent   
   
white, crystalline, deliquescent   

State and explain the observation made when each of the compounds is left exposed in air: i. Compound A (2 marks)

ii. Compound B (2 marks)

b. In an experiment to determine the formula of hydrated magnesium sulphate, a sample was heated in a crucible until a constant mass was obtained. The results are shown in Table 2.


Mass of crucible
   
25.62 g   
   
Mass of crucible + solid before   heating   
   
28.08 g   
   
Mass of crucible + solid after heating   
   
26.82 g   

Using the information in Table 2, determine the formula of the hydrated salt (Mg - 24.0; S = 32.0; O=16.0; H = 1.0). (3 marks)

c. Figure 1 shows analysis of an alloy containing two metals.


Time (se

conds)
   
0   
   
30   
   
60   
   
90   
   
120   
   
150   
   
180   
   
210   
   
240   
   
Volume
   
Of CO2
   
(cm3)   
   
O   
   
62   
   
92   
   
113   
   
124   
   
130   
   
132   
   
133   
   
133   
Using the information in Table 2, determine the formula of the hydrated salt

(Mg - 24.0; S = 32.0; O=16.0; H = 1.0). (3 marks)

c. Figure 1 shows analysis of an alloy containing two metals.

i. Give the name of another product formed in step 1. (1 mark)

ii. Write the formula of the complex ion present in the colourless solution obtained in step 2 (1 mark)

iii. Identify the metals in the alloy, (2 marks)

2. The flow chart in Figure 2 shows the processes involved in the manufacture of sulphuric(VI) acid.

a. Explain how the sulphur used in this process is obtained. (2 marks)

b. Give one advantage of using air in chamber 1 instead of using oxygen gas. (1 mark)

c. Identify substances: (1)

i. M (1 mark)

ii. N (1 mark)

d.i. In chamber 2, drying and purification take place. Give a reason why this is necessary (1 mark)

ii. The reaction in chamber 3 is highly exothermic.

I. Explain why high temperature is required for the reaction in chamber 3. (1 mark)

II. State how heat produced in chamber 3 can be utilised in this process e. Give a reason why this method of manufacture is known as 'contact process". (1 mark)

f. Emission of gases in the sulphuric(VI) acid plant may lead to environmental pollution.

i. State the evidence that could be used to show that the sulphuric(VI) acid plant causes pollution (1 mark)

ii. Explain how the pollution identified in 2(1)(i) can be controlled. (1 mark)

3.a. Chemical reactions occur as a result of collisions of particles. Give a reason why not all collisions are effective. (1 mark)

b. State and explain how the following factors affect the rate of reaction: i. Surface area of reactants. (1 mark)

ii. Pressure. (1 mark)

c. In an experiment to determine the rate of a reaction, marble chips were added to excess 2M hydrochloric acid. The equation for the reaction is:

CaCO3(s) + 2HCl(aq) → CaCI2(aq) + CO2(g) + H2O(l)

The volume of carbon(IV) oxide produced was measured at 25°C and recorded after every 30 seconds.

Table 3 shows the results obtained.


Time (se

conds)
   
0   
   
30   
   
60   
   
90   
   
120   
   
150   
   
180   
   
210   
   
240   
   
Volume
   
Of CO2
   
(cm3)   
   
O   
   
62   
   
92   
   
113   
   
124   
   
130   
   
132   
   
133   
   
133   
i. On the grid provided, plot a graph of volume of carbon(IV) oxide (vertical axis) against time (horizontal axis). (3 marks)

ii. Using the graph, determine the rate of reaction at the:

I. 45th second. (1 mark)

II. 105th second. (1 mark)

iii. Give a reason for the differences in the two rates. (1 mark)

iv. Using the graph, determine the mass of marble chips that reacted (2 marks)

(Ca=40.0; C = 12.0; 0 - 16.0;)

Molar gas volume at room temperature and pressure = 24000 cm").

4.a. Sea water contains approximately 3% sodium chloride. Describe how sodium chloride is obtained from sea water. (3 marks)

b. The solubility of sodium chloride is 36.2 g in 100 g of water at room temperature.

Determine the concentration in moles per litre of a saturated aqueous sodium chloride at room temperature (Na= 23.0; Cl= 35.5; density of water = 1.0 gem"). (2 marks)

c. Ammonia is highly soluble in water.

i. Explain how aqueous ammonia is prepared starting with ammonia gas. (2 marks)

ii. On the axes provided, sketch a curve showing how solubility of ammonia gas varies with temperature. (1 mark)

iii. Give a reason for the shape of the curve. (1 mark)

d. Water hardness is due to the presence of magnesium and calcium ions. Explain how these ions get into sources of water. (2 marks)

5.a. Figure 3 shows part of a Periodic Table.

i. Select from the table the most reactive: I. metal. (1 mark)

II. non-metal. (1⁄2 mark)

ii. Select an element with the highest first ionisation energy. (1 mark)

iii.I. Name the method used to obtain argon from its source. (1 mark)

II. Give one industrial use of argon. (1 mark)

iv. Explain each of the following observations:

I. The melting point of lithium is higher than that of potassium. (1 mark)

II. The melting point of chlorine is lower than that of iodine. (1 mark)

v. The following ions have the same number of electrons: N2-, Mg2+, 02, Na+ Arrange them in order of increasing ionic size. Give a reason for the order. (2 marks)

b. Use Table 4 to answer the questions that follow.

Properly Substance  
H I J K

Melting point (°C)
   
993   
   
113   
   
-38.9   
   
-85   

Boiling point (°C)
   
1695   
   
183   
   
357   
   
-60   

Electrical conductivity at

room temperature
   
Does not conduct   
   
Does not conduct   
   
Conducts   
   
Does not conduct   
   
Electrical conductivity in
   
molten state   
   
Conducts   
   
Does not conduct   
   
Conducts   
   
Does not conduct   
i. Identify the substance which is a gas at room temperature. Give a reason. (1 mark)

ii. Name the particles responsible for electrical conductivity in substance: IH (1 mark)

I. H II. J (1 mark)

iii. Identify the type of forces that hold the particles together in: I. H (1 mark)

II. Κ (1 mark)

6. Figure 4 shows a flow chart involving reactions of some organic compounds.

a. Write the formula and give the names of compounds: i. X

Name:

Formula:

ii. Y

Name:

Formula:

b. Give the reagents and conditions necessary for carrying out:

i. Step 3. (1 mark)

ii. Step 5. (1 mark)

i. Write an equation for the reaction in step 6. (1 mark)

ii. State the observations made in step 6. (1 mark)

7.a. Using the oxidation numbers of chlorine, explain why the following is a redox reaction. HCIO3(aq) + 5HCl(aq) → 3CI2(g) + 3H2O(I) (2 marks)

b. Use the following standard reduction potentials to answer the questions that follow:


I
   
Half cell reactions   
   
Eo/V   

II

PSO4 (s) + 2e → Pb(s) +

SO4'-(aq)
   
-0.36   

III

PBO2(s) + S042- (aq) +
4H+(aq) + 2e → PbSO4 (s) +
2HyO(1)
   
+1.69   

IV

Fe3+(aq) + e → Fe2+(aq)
   
+0.77   
   
V   

Zn2+(aq) + 2e → Zn(s)
   
-0.76   
   
V   

MnO4-' (aq) + 8H+(aq) + 5e -+

Mn2 (aq) + 4HtO(I)
   
+1.51   
   
Vl   

O2g+ 2 H -I- (aq) -- 2e —+
H2O2(aq)
   
+0.68   
   
VII   

Fe2+(aq) -i- 2e → Fe(s)
   
-0.44   
   
VIII   

Ca2+(aq) → 2e  Cu(s)
   
+0.34   

i. The half cells I and II are combined to form an electrochemical cell.

I. Write an equation for the cell reaction. (1 mark)

II. Calculate the e.m.f of the cell. (1 mark)

ii. Draw a labelled diagram for the electrochemical cell formed using half cells III and IV. (3 marks)

iii. State and explain the observations made when a few drops of acidified potassium manganate(VII) are added to hydrogen peroxide. (3 marks)

iv. Coating iron with zinc is a more effective way of corrosion prevention than coating it with copper. Explain. (2 marks)

Questions and Answers

Kenya certificate of Secondary Education

2021 Chemistry paper 2

1. Table 1 gives the properties of two compounds, A and B.

a. Table 1

1.


A
   
B   
   
white, crystalline, efflorescent   
   
white, crystalline, deliquescent   

State and explain the observation made when each of the compounds is left exposed in air:

i. Compound A (2 marks)

  • Powder
  • loss water of crystalization

    ii. Compound B (2 marks)

  • Dissolve/color loss liquid
  • Absorbs water vapour

    b. In an experiment to determine the formula of hydrated magnesium sulphate, a sample was heated in a crucible until a constant mass was obtained. The results are shown in Table 2. Table 2


    Mass of crucible
       
    25.62 g   
       
    Mass of crucible + solid before   heating   
       
    28.08 g   
       
    Mass of crucible + solid after heating   
       
    26.82 g   

    Using the information in Table 2, determine the formula of the hydrated salt (Mg - 24.0; S = 32.0; O=16.0; H = 1.0). (3 marks)

    MgSO4 H2O

    Mass(g) 1.20 1.26

    Moles 1.20 1.26

    120 18 0.07/0.01

    0.01/0.01

    1 7

    MgSO4.7H2O

    c. Figure 1 shows analysis of an alloy containing two metals.


    Time (se

    conds)
       
    0   
       
    30   
       
    60   
       
    90   
       
    120   
       
    150   
       
    180   
       
    210   
       
    240   
       
    Volume
       
    Of CO2
       
    (cm3)   
       
    O   
       
    62   
       
    92   
       
    113   
       
    124   
       
    130   
       
    132   
       
    133   
       
    133   
    i. Give the name of another product formed in step 1. (1 mark)

  • Hydrgen gas

    ii. Write the formula of the complex ion present in the colourless solution obtained in step 2 (1 mark)

  • [Zn(OH)42-

    iii. Identify the metals in the alloy, (2 marks)

  • Zinc/Zn

  • Copper/Cu

    2. The flow chart in Figure 2 shows the processes involved in the manufacture of sulphuric(VI) acid.

    a. Explain how the sulphur used in this process is obtained. (2 marks)

  • Three concentric pipes
  • Super heated water through outer pipe
  • Hot compressed air through inner pipe
  • Molten sulphur through middle pipe

    b. Give one advantage of using air in chamber 1 instead of using oxygen gas. (1 mark)

  • Air is cheap/Economical/Readily available

    c. Identify substances: (1)

    i. M (1 mark)

  • Concentrated sulphur(VI) acid/ H2SO4

    ii. N (1 mark)

  • Water/H2O

    d.i. In chamber 2, drying and purification take place. Give a reason why this is necessary (1 mark)

  • Impurities poisons catalyst/make it inefficient

    ii. The reaction in chamber 3 is highly exothermic.

    I. Explain why high temperature is required for the reaction in chamber 3. (1 mark)

  • Increase rate of reaction
  • Effective collisions/Fruitful

    II. State how heat produced in chamber 3 can be utilised in this process

  • Preheat SO2 & O2/ reactants
  • Recycling of heat

    e. Give a reason why this method of manufacture is known as 'contact process". (1 mark)

    Reactants come in contact with catalyst

    f. Emission of gases in the sulphuric(VI) acid plant may lead to environmental pollution.

    i. State the evidence that could be used to show that the sulphuric(VI) acid plant causes pollution (1 mark)

  • Rusting of mettalic structures
  • Stone structure wearing/ chlorosil
  • Death of aquatic life
  • Wilting of plants
  • Respiratory diseases
  • Acid rain loweing pH of soil

    ii. Explain how the pollution identified in 2(1)(i) can be controlled. (1 mark)

    Passing through Ca(OH)2/CaO

    Scrubbing

    3.a. Chemical reactions occur as a result of collisions of particles. Give a reason why not all collisions are effective. (1 mark)

  • Particles not possess necessary kinetic energy /activation of energy
  • Particles collide in wrong orientation

    b. State and explain how the following factors affect the rate of reaction:

    i. Surface area of reactants. (1 mark)

  • Increases rate of reaction
  • Move particles are in contact
  • More collision per unit time
  • More particles exposed

    ii. Pressure. (1 mark)

  • Increases rate of reaction
  • Increases manner of collision
  • Molecules of gaseous reactants close
  • Decrease volume/frequency of collision

    c. In an experiment to determine the rate of a reaction, marble chips were added to excess 2M hydrochloric acid. The equation for the reaction is:

    CaCO3(s) + 2HCl(aq) → CaCI2(aq) + CO2(g) + H2O(l)

    The volume of carbon(IV) oxide produced was measured at 25°C and recorded after every 30 seconds.

    Table 3 shows the results obtained.


    Time (se

    conds)
       
    0   
       
    30   
       
    60   
       
    90   
       
    120   
       
    150   
       
    180   
       
    210   
       
    240   
       
    Volume
       
    Of CO2
       
    (cm3)   
       
    O   
       
    62   
       
    92   
       
    113   
       
    124   
       
    130   
       
    132   
       
    133   
       
    133   
    i. On the grid provided, plot a graph of volume of carbon(IV) oxide (vertical axis) against time (horizontal axis). (3 marks)

    ii. Using the graph, determine the rate of reaction at the: I. 45th second. (1 mark)

    Tangent 45

    Calculations from graph

    dy2/dx2 - dy1/dx1

    Ans = cm3/sec

    II. 105th second. (1 mark)

    Tangent 45

    Calculations from graph

    dy2/dx2 - dy1/dx1

    Ans = cm3/sec

    iii. Give a reason for the differences in the two rates. (1 mark)

  • Rate at 45th is greater than 105th Hence faster rate of reaction/
  • Rate at 105 sec is low to reduce reactants

    iv. Using the graph, determine the mass of marble chips that reacted (2 marks) (Ca=40.0; C = 12.0; 0 - 16.0;) Molar gas volume at room temperature and pressure = 24000 cm").

    Moles = 133/24000

    Moles ratio 1:1

    CaCO3

    5.54 x 10-3 x 100 RFM

    100 x 133 (over) 24000

    Ans = 0.554g

    4.a. Sea water contains approximately 3% sodium chloride. Describe how sodium chloride is obtained from sea water. (3 marks)

  • Heat/Boil/Evaporate to saturation
  • Allow to cool; crystals formed or
  • Sea water trapped in pan/shallow pond solid crystallises out

    b. The solubility of sodium chloride is 36.2 g in 100 g of water at room temperature.

    Determine the concentration in moles per litre of a saturated aqueous sodium chloride at room temperature (Na= 23.0; Cl= 35.5; density of water = 1.0 gem"). (2 marks)

    RFM NaCl = 58.5

    36.2 x 1000 (over) 100 = 362

    362/58.5

    6.188M or 6.19M

    c. Ammonia is highly soluble in water.

    i. Explain how aqueous ammonia is prepared starting with ammonia gas. (2 marks)

  • Pass inserted funnel to prevent suck back

    ii. On the axes provided, sketch a curve showing how solubility of ammonia gas varies with temperature. (1 mark)

    iii. Give a reason for the shape of the curve. (1 mark)

  • Solubility decreases with increase in temperature becasue the gaseous particles gain energy and escape from solution

    d. Water hardness is due to the presence of magnesium and calcium ions. Explain how these ions get into sources of water. (2 marks)

  • Formation of carbon acid reacts with rocks with Ca & Mg salts leading to Ca2+ and Mg2+

    ions

    5.a. Figure 3 shows part of a Periodic Table.

    i. Select from the table the most reactive: I. metal. (1 mark)

    Cs

    II. non-metal. (1⁄2 mark)

    F

    ii. Select an element with the highest first ionisation energy. (1 mark)

    HI

    I. Name the method used to obtain argon from its source. (1 mark)

    Fractional distillation

    II. Give one industrial use of argon. (1 mark)

    Used in flourescent bulbs/lamps

    iv. Explain each of the following observations:

    I. The melting point of lithium is higher than that of potassium. (1 mark)

  • Lithium has stronger metallic bonds than potassium

    II. The melting point of chlorine is lower than that of iodine. (1 mark)

  • Iodine has more forces than chlorine
  • Iodine is stronger/more intermolecular forces

    v. The following ions have the same number of electrons: N2-, Mg2+, 02-, Na+ Arrange them in order of increasing ionic size. Give a reason for the order. (2 marks)

    Mg2+; Na+; O2-; N3-;

    Protons decreases from Mg to nitrogen hence nuclear attraction decreases from Mg to N

    b. Use Table 4 to answer the questions that follow.

    Properly Substance  
    H I J K

    Melting point (°C)
       
    993   
       
    113   
       
    -38.9   
       
    -85   

    Boiling point (°C)
       
    1695   
       
    183   
       
    357   
       
    -60   

    Electrical conductivity at

    room temperature
       
    Does not conduct   
       
    Does not conduct   
       
    Conducts   
       
    Does not conduct   
       
    Electrical conductivity in
       
    molten state   
       
    Conducts   
       
    Does not conduct   
       
    Conducts   
       
    Does not conduct   

    i. Identify the substance which is a gas at room temperature.

    Give a reason. (1 mark)

    K; boiling point below room temperature

    ii. Name the particles responsible for electrical conductivity in substance: IH (1 mark)

    I. H ions/ mobile ions

    II. J (1 mark)

    electrons/ delocalized electrons

    iii. Identify the type of forces that hold the particles together in:

    I. H (1 mark)

    electrostatic forces/ ionic bonds

    II. Κ (1 mark)

    weak van der waals forces/ intermolecular

    6. Figure 4 shows a flow chart involving reactions of some organic compounds.

    a. Write the formula and give the names of compounds: i. X

    Name:

    i. Magnesium propoxide

    Formula:

    (CH3CH2CH2O)2Mg

    ii. Y

    Name:

    Sodium propanoate

    Formula:

    CH3CH2COONa

    b. Give the reagents and conditions necessary for carrying out:

    i. Step 3. (1 mark)

    H+/ KMnO4/H+K2Cr2O7

    Warm/ Heat/ High temperature

    ii. Step 5. (1 mark)

    i. Write an equation for the reaction in step 6. (1 mark)

    CH3CHCH2 + Br2 → CH3CHBr2

    ii. State the observations made in step 6. (1 mark)

  • Brown/Yellow/Orange/decolorized

    7.a. Using the oxidation numbers of chlorine, explain why the following is a redox reaction.

    HCIO3(aq) + 5HCl(aq) → 3CI2(g) + 3H2O(I) (2 marks)

    Oxidatopn of Cl in HClO from +5 to 0 Reduction -1 to 0 - Oxidation

    b. Use the following standard reduction potentials to answer the questions that follow:


    I
       
    Half cell reactions   
       
    Eo/V   

    II

    PSO4 (s) + 2e → Pb(s) +

    SO4'-(aq)
       
    -0.36   

    III

    PBO2(s) + S042- (aq) +
    4H+(aq) + 2e → PbSO4 (s) +
    2HyO(1)
       
    +1.69   

    IV

    Fe3+(aq) + e → Fe2+(aq)
       
    +0.77   
       
    V   

    Zn2+(aq) + 2e → Zn(s)
       
    -0.76   
       
    V   

    MnO4-' (aq) + 8H+(aq) + 5e -+

    Mn2 (aq) + 4HtO(I)
       
    +1.51   
       
    Vl   

    O2g+ 2 H -I- (aq) -- 2e —+
    H2O2(aq)
       
    +0.68   
       
    VII   

    Fe2+(aq) -i- 2e → Fe(s)
       
    -0.44   
       
    VIII   

    Ca2+(aq) → 2e  Cu(s)
       
    +0.34   

    i. The half cells I and II are combined to form an electrochemical cell.

    I. Write an equation for the cell reaction. (1 mark)

    PbO2(s) + 2SO22-(aq) + 4H+ + Pb → 2PbSO4(s) +2H2O(I)

    II. Calculate the e.m.f of the cell. (1 mark)

    +1.69 = 0.36

    + 2.05V

    ii. Draw a labelled diagram for the electrochemical cell formed using half cells III and IV. (3 marks)

    iii. State and explain the observations made when a few drops of acidified potassium manganate(VII) are added to hydrogen peroxide.(3 marks)

    H+/KMnO4 Decolorized/ Purple to colourless Effervescence/ Bubbles of colourless gas H2O2 oxidised to O2 gas/ Production of O2S4 MnO4-

    Mn2+

    iv. Coating iron with zinc is a more effective way of corrosion prevention than coating it with copper. Explain. (2 marks)

  • Zinc is more reactive than iron
  • Iron is more reactive than copper/copper is less reactive than iron

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