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  • kcse form 2 mathematics questions

The following set – up was made in an experiment by a group of form four students. The readings of the balance before and after experiment were indicated in the diagram below.

14/10/2021

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The following set – up was made in an experiment by a group of form four students. The readings of the balance before and after experiment were indicated in the diagram below. Given that the initial temperature of water was 26.70C respectively. The specific heat capacity of water is 4200Jkg-1k-1
The following set – up was made in an experiment by a group of form four students. The readings of the balance before and after experiment were indicated in the diagram below. Given that the initial temperature of water was 26.7 degrees centigrade respectively. The specific heat capacity of water is 4200Jkg-1k-1

​Determine:

​a) Temperature change that occurred (1mk)

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​b) Amount of ethanol used (1mk)

​10.5 – 1.0 = 9.5g

​c) Moles of ethanol used (2mks)

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​d) Amount of heat gained by water (2mks)

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​e) Molar enthalpy of combustion of ethanol (2mks)

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​f) Use the following thermochemical processes to answer the questions that follow;

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​i) Draw an energy level diagram representing the formation and combustion processes of propane, carbon and hydrogen (2mks)



​ii) Hence or otherwise, determine the heat of formation of propane (2mks)

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The table below gives the volume of hydrogen gas produced when different acids of 50cm3 were each reacted with 10cm piece of magnesium ribbon in a conical flask.

14/10/2021

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The table below gives the volume of hydrogen gas produced when different acids of 50cm3 were each reacted with 10cm piece of magnesium ribbon in a conical flask.
The table below gives the volume of hydrogen gas produced when different acids of 50cm3 were each reacted with 10cm piece of magnesium ribbon in a conical flask.

a) On the grid provided, plot on the same axis, the graph of volume of gas produced against time (4mks)



In the graph plotted ; Award marks as follows:
  1. Plotting; award 2 marks for 
  2. Smooth curve
  3. Scale (x and y)

​b) From the graph, determine the rate of reaction of both acids at 55 seconds

​i) 1M sulphuric (VI) acid (1mk)

​Rate of 1M H2SO4 = 0.5 ± 0.05

​ii) 1M ethanoic acid (1mk)

​Rate of 1M ethanoic acid = 0.25 ± 0.01

c) The rate of reaction of H2SO4 is twice that of ethanoic acids. This is because H2SO4 is stronger while ethanoic acid is a weak acid.

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​c) Explain the difference in the rate of evolution of the gas as determined in (b) above       (2mks)



d) Calculate the number of moles of hydrogen gas produced when 10cm magnesium ribbon is completely reacted with 1M sulphuric (VI) acid. (Molar gas volume = 24dm3 at r.t.p) (2mks)

​e) What mass of magnesium had therefore reacted? (Mg = 24) (2mks)

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Below is a simplified diagram of a Down’s cell used for the manufacture of Sodium metal. Study it and answer the questions that follow.

14/10/2021

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Below is a simplified diagram of a Down’s cell used for the manufacture of Sodium metal. Study it and answer the questions that follow.
Above is a simplified diagram of a Down’s cell used for the manufacture of Sodium metal. Study it and answer the questions that follow.

​a) Name the substance the anode is made of (1mk)

​Graphite

​b) Explain your answer in (a) above (1mk)

​Reject carbon
​Graphite does not react with chlorine liberated at the anode 


​c) What is the role of the diaphragm in Down’s cell (1mk)

​To prevent metal and chlorine gas from recombining

d) In Down’s cell for the manufacture of Sodium metal, Calcium chloride salt is added to lower the melting point from 8000C to 6000C. Explain why it is necessary to lower the melting point (1mk)

​To reduce the cost of energy used to melt the sodium metal 

​e) Calculate the mass of sodium metal produced if a current of 50 amperes is passed through the molten Sodium chloride for two (2) hours (Na = 23, F = 96500C) (2mks)

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​f) Below is a list of potential differences obtained when metal P, Q, R, S and T are used in the following electrochemical cell
Metal (s) / Metal ions // Copper (II) ions / copper (s) 

Below is a list of potential differences obtained when metal P, Q, R, S and T are used in the following electrochemical cell
Below is a list of potential differences obtained when metal P, Q, R, S and T are used in the following electrochemical cell

​i) Which metal is likely to be Copper. Explain (2mks)

​R

​ii) Identify the strongest reducing agent (1mk)

​P


​iii) Which two half – cells would be combined to produce the highest voltage? (1mk)

​P and T

​iv) Give a cell representation of the cell in F (iii) above. (2mks)

​P/p ions // T ions /T (s) 

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The empirical formula of a hydrocarbon is (CH2). It has a density of 0.001167g/cm3 at room temperature and pressure. (Molar gas volume at r.t.p is 24dm3)

13/10/2021

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The empirical formula of a hydrocarbon is (CH2). It has a density of 0.001167g/cm3 at room temperature and pressure. (Molar gas volume at r.t.p is 24dm3)

​a) Determine the molecular formula of the hydrocarbon (3mks)

Determine the molecular formula of the hydrocarbon


b) Draw the structural formula of the hydrocarbon (1mk)

Draw the structural formula of the hydrocarbon

​c)  Ethene gas burns in Oxygen to form Carbon (IV) oxide and water.

​i) Write an equation for the reaction between ethane gas oxygen gas (1mk)

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ii) 15cm3 of ethene gas were mixed with 50cm3 of oxygen gas and the mixture was ignited into complete combustion. Calculate the volume of excess unreacted gas  (3mks)

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​d) What happens when ethene gas is bubbled through bromine water? (2mks)

  • Bromine water is decolourised
  • Ethene gas is unsaturated hydrocarbon


​e) Give any two uses of ethene gas (2mks)

​Uses of Ethene gas
  • Manufacture of ethanol
  • Manufacture of polythene 
  • Ripening of fruits
  • Laboratory preparation of ethane -1,2-diol used as coolant
  • Manufacture of detergents
(award 1mk for any one correct)

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The apparatus shown below were used for the preparation of hydrogen sulphide gas in the laboratory

13/10/2021

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The apparatus shown below were used for the preparation of hydrogen sulphide gas in the laboratory
The apparatus shown above were used for the preparation of hydrogen sulphide gas in the laboratory


​​a) Name;

​i) Substance V (1mk)

​V is Dilute hydrochloric Acid 

​ii) Solid X (1mk)

​W is Iron (ii) Sulphide 

​b) Write an equation for the preparation of hydrogen sulphide (1mk)

Write an equation for the preparation of hydrogen sulphid

​c) What property of the gas enables it to be collected by the method shown in the diagram? (1mk)

​It is denser than air 

​d) What is the purpose of the water in the second flask? (1mk)

​To absorb acid vapour (HCl) 

​e) What precaution should be taken when preparing the gas? (1mk)

​The gas should be prepared in a fume chamber or in the open 

​f) Explain the observations made when dry hydrogen sulphide is exposed to wet Lead (II) acetate paper (2mks)

Black colour observed; black lead (ii) sulphide is formed.

​g) State the observation that would be made when hydrogen sulphide gas is bubbled through acidified Potassium dichromate (VI) solution (1mk)

  • Yellow deposit of sulphur 
  • Colour change from orange to green 


​h) Explain why it is not advisable to dispose off hydrogen sulphide gas by burning (1mk)


SO2 is formed causing acid rain

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

13/10/2021

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Use the information in the table below to answer the questions that follow
Use the information in the table above to answer the questions that follow

​a) i) Are the members in this group likely to be conductor or non – conductors? (1mk)

  • Conductors
    Reasons:
    They are metals
    They larger atomic radius and  therefore have free (delocalised) electrons


ii) Which element would have the lowest atomic number? Explain. (1mk)

  • F
    ​Reasons:
    ​It has the smallest atomic radius 

​b) The grid below represents part of the periodic table. Study it and answer the questions that follow. (The letters are not the actual symbols of the elements)

b) The grid below represents part of the periodic table. Study it and answer the questions that follow. (The letters are not the actual symbols of the elements)
b) The grid above represents part of the periodic table. Study it and answer the questions that follow. (The letters are not the actual symbols of the elements)

​i) Select the element in period three which has the shortest atomic radius. Give a reason for your answer. (2mks)

  • Z – Atomic radius decrease across the period due to increase in nuclear force of attraction (effective nuclear charge)

​ii) Using dots (•) and crosses (x) to represent outermost electrons, draw a diagram to show the bonding in the compound formed when chlorine reacts with element X (1mk)

Using dots (•) and crosses (x) to represent outermost electrons, draw a diagram to show the bonding in the compound formed when chlorine reacts with element X
½mk @ x 2 = 1mk Penalize fully if dots or crosses alone are used


​iii) When three liters of chlorine gas were completely reacted with element Y, 11.85g of the product were formed. Calculate the relative atomic mass of element Y. (3mks)

​(R.A.M of chlorine = 35.5, molar gas volume = 24 liters) 
When three liters of chlorine gas were completely reacted with element Y, 11.85g of the product were formed. Calculate the relative atomic mass of element Y.

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Use the flow chart below to answer the questions that follow

13/10/2021

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Use the flow chart below to answer the questions that follow
Use the flow chart above to answer the questions that follow


​​a) Name the following;

​i) Gas L (1mk)

​Gas L – Carbon (IV) Oxide

​ii) Gas H (1mk)

​Gas H – Hydrogen 

​iii) K (1mk)

​K – Propane 

​​b) Name the processes involved in the following steps

​i) Step I (1mk)

Step I : Hydrogen 

​ii) Step II (1mk)

​Step II – Neutralization

​​iii) Step III (1mk)

​Step III – Substitution 

​c) Draw the structure of compound E (1mk)

Draw the structure of compound E

​d) Write a chemical equation for the complete combustion of substance F (1mk)

rite a chemical equation for the complete combustion of substance F

​e) Name the condition and reagents in step III 

​i) Condition (1mk)

​U.V light  

​ii) Reagent (1mk)

​Chlorine

​f) Calculate the mass of salt Q that would be formed by using 21.9kg of G when it reacts with excess sodium hydroxide (2mks)
(C = 120, H = 1.0, Na = 23.0, O = 16.0)

Calculate the mass of salt Q that would be formed by using 21.9kg of G when it reacts with excess sodium hydroxide


​g) i) Draw the structure of polymer D (1mk)

Draw the structure of polymer D

​ii) State one use of the above polymer (1mk)

  1. Mouldings 
  2. Plastic ropes / Synthetic fibres 
  3. Use in films

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K.C.S.E Chemistry Q & A-MODEL 2018.PP2.Q N.6

25/11/2020

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KCSE Chemistry 2018 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


(a) In Kenya, sodium carbonate is extracted from trona at Lake Magacli.
(i) Give the formula of trona. 
(ii) Name the process of extracting sodium carbonate from trona. 
(b) The flow chart in Figure 5 summarises the steps involved in the production of sodium carbonate.
Use it to answer the questions that follow.
Picture
​(i) Name the process illustrated in Figure 5. 
(ii) Identify the starting raw materials required in the production of sodium carbonate. 
(iii) Write equations for the two reactions that occur in the carbonator. 
(iv) Name two substances that are recycled. 
(v) Identify:
Solid X; 
Process W. 
(vi) Write an equation for the reaction that produces solution Z. 
(vii) Apart from softening hard water, state two other uses of sodium carbonate.
 
ANSWERS
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K.C.S.E Chemistry Q & A-MODEL 2018.PP2.Q N.5

25/11/2020

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KCSE Chemistry 2018 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


 (a) The diagram in Figure 4 was used to prepare hydrogen chloride gas which was passed over heated iron powder.
Picture
(i) Give a pair of reagents that will produce hydrogen chloride gas in flask A. 
(ii) Name the substance in flask B. 
(iii) State the observation made in the combustion tube. 
(iv) Write an equation for the reaction in the combustion tube. 
(v) Describe a chemical test for hydrogen chloride gas. 
(b) (1) Identify the gas that burns at the jet. 
(ii) Explain why the gas in (b) (I) is burned.
(c) Give reasons why excess hydrogen chloride gas is dissolved using the funnel arrangement. 
(d) State what will be observed when the reaction in the combustion tube is complete.
(e) Another experiment was carried out where hydrogen chloride gas was bubbled through methylbenzene and water in separate beakers. The resulting solutions were tested with blue litmus papers and marble chips.
(i) Write the observations made in the following table.
Picture
​(ii) Explain the observations in (e) (i). 
ANSWERS
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K.C.S.E Chemistry Q & A-MODEL 2018.PP2.Q N.4

25/11/2020

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KCSE Chemistry 2018 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


​An experiment was carried out to prepare crystals of magnesium sulphate. Excess magnesium powder was added to 100 cm3 of dilute sulphuric (VI) acid in a beaker and warmed until no further reaction took place. The mixture was filtered and the filtrate evaporated to saturation, then left to cool for crystals to form.
(a) (i) Write an equation for the reaction. 
(ii) Explain why excess magnesium powder was used. 
(iii) State how completion of the reaction was determined. 
(iv) What is meant by a saturated solution? 
(v) Explain why the filtrate was not evaporated to dryness. 
(b) When bleaching powder, CaOCl2, is treated with dilute nitric(V) acid, chlorine gas is released. This reaction can be used to determine the chlorine content of various samples of bleaching powders and liquids.
(i) Write an equation for the reaction of nitric(V) acid with bleaching powder.
(ii) Calculate the volume of chlorine produced when 10g of CaOCl2 is treated with excess nitric (v) acid. (Ca = 40.0; 0 = 16.0; Cl = 35.5; 1 mole of gas occupies 22.4dm3 at s.t.p) 
(c) Apart from use of chlorine gas in bleaches and water treatment, state two other uses of chlorine gas.
ANSWERS
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K.C.S.E Chemistry Q & A-MODEL 2018.PP2.Q N.3

25/11/2020

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KCSE Chemistry 2018 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


​(a) Complete Table I by indicating the observations, type of permanent or temporary change and name of new compound formed.
Picture
(b) Use the set-up in Figure 3 to answer the questions that follow. The flask was covered with a cloth that had been soaked in ice-cold water.
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(i)State the observation made on the coloured water. Explain.
(ii) Name the gas law illustrated in Figure 3. 
(c)Use the standard electrode potentials in Table 2 to answer the questions that follow.
Picture
​(i)Write the half-cell representation for the element whose electrode potential is for hydrogen. 
(ii) Arrange the elements in order of reducing power, starting with the weakest reducing agent. 
(iii) I Select two half cells which combine to give a cell with the least e.m.f. 
II Calculate the e.m.f of the half cells identified in (iii) I. 
ANSWERS
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K.C.S.E Chemistry Q & A-MODEL 2018.PP2.Q N.2

25/11/2020

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KCSE Chemistry 2018 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


Figure 2 is a section of the periodic table. Study it and answer the questions that follow. The letters do not represent the actual symbols of elements.
Picture
(a) (i) Select elements which belong to the same chemical family.
(ii) Write the formulae of ions for elements in the same period.
(b) The hrst ionisation energies of two elements K and M at random are 577 kJ/mol and 494 kJ/mol 
(i) Write equations for the 1ˢᵗ ionisation energies for elements K and M and indicate their energies.
(iii) Write the formula of the compound formed when L and I react.
(iv) Give one use of elemcnt V.
(c) (i) State anothcr group that G can be placcd in Figure 1. Explain. 
(ii) How do the reactivity of elements J and K compare? Explain. 
(d) (i) Elements L and M form chlorides.
​Complete the following table by writing the formulae of each chloride and state the nature of the solutions.
Picture
​(ii) The chloride of element M vapourises easily while its oxide has a high melting point. Explain.
ANSWERS
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K.C.S.E Chemistry Q & A-MODEL 2018.PP2.Q N.1

25/11/2020

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KCSE Chemistry 2018 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


The diagram in figure I shows some natural and industrial processes. Study it and answer the questions that follows
Picture
​(a) Identify the processes labelled: 
A...................
B...................
C...................
D...................
(b) State the reagents and conditions required for processes B and D.
(i) Process B:
Reagent................
Conditions ............ 
(ii) Process D:
Reagent................
Conditions ............ 
(iii) Describe how process D is carried out.
(iv) State two additives used to improve the quality of soap.
(c) State the reagents required in steps F and G.
(iii) Draw the structure of terylene.
(d) (i) Name the polymer formed in step C.
(ii) State one disadvantage of the polymer formed in (d) (i).
ANSWERS
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K.C.S.E Chemistry Q & A-MODEL 2017.PP2.Q N.7

23/11/2020

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KCSE Chemistry 2017 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


The decay rates of a sample of a radioisotope of bismuth at different time intervals is indicated in the following table.
Picture
(a)(i) Draw a graph of disintegration rate against time. 
(ii) Determine the half-life of bismuth. 
(iii) What would be the effect on the curve if half the amount of sample of bismuth were used. 
(b) Radioactivity has several applications. State one application of radioactivity in: 
(i) Medicine 
(ii) Agriculture 
(iii) Tracers 
(iv) Nuclear power station 
(c) State two dangers associated with radioactivity. 
ANSWERS
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(ii) It would have no effect on the curve as the quantity of bismuth does not affect half-life. 
(b)(i)Applications in medicine
 Sterilizing surgical instruments.
 Destroying cancerous tissues during radiotherapy.
 Provide power to the heart pace setters.
(ii) Applications in agriculture
 Monitor photosynthesis and other related processes.
 Preservation of foodstuffs, by exposing 
Micro-organisms to gamma rays.
 Rate of absorption of a fertilizer by the plant.
(iii)Applications in Tracers
 Detecting leakages in underground water or oil pipes. 
(iv)Applications in Nuclear power stations.
To generate electricity. 
(d) Dangers of radioactivity
 Long term exposure causes genetic mutation;
 Radioisotopes can be used as weapon of mass 
Destruction;
 Causes skin cancer;
 When tested causes environmental pollution.​

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K.C.S.E Chemistry Q & A-MODEL 2017.PP2.Q N.6

23/11/2020

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KCSE Chemistry 2017 Topical Questions and Answers

All Questions Featuring Chemistry Form 1, Form 2, Form 3, Form 4, Paper 1, Paper 2 and Paper 3


The following steps were used to analyse a metal ore.
(i) An ore of a metal was roasted in a stream of oxygen. A gas with a pungent smell was formed which turned acidified potassium dichromate(VI) green.
(ii) The residue left after roasting was dissolved in hot dilute nitric(V) acid. Crystals were obtained from the solution.
(iii) Some crystals were dried and heated. A brown acidic gas and a colourless gas were evolved and a yellow solid remained. (iv) The solid was yellow when cold.
(v) The yellow solid was heated with powered charcoal. Shiny beads were formed.
Name the:
(a) gas formed when the ore was roasted in air. 
(b) gases evolved when crystals in step (iii) were heated. 
(c) yellow solid formed in step (iii). 
(d) shiny beads in step (iv). 
(e) The yellow solid from procedure (iii) was separated, dried, melted and the melt electrolysed using graphite electrodes.
I. Describe the observations made at each electrode. 
II. Write the equation for the reaction that took place at the anode. 
(f) Some crystals formed in step (ii) were dissolved in water, and a portion of it reacted with potassium iodide solution. A yellow precipitate was formed. Write an ionic equation for this reaction. 
(g) To another portion of the solution from (f), sodium hydroxide solution was added drop by drop until there was no further change. Describe the observation made. 
(h) To a further portion of the solution from (f), a piece of zinc foil was added.
I. Name the type of reaction taking place. 
II. Write an ionic equation for the above reaction.
ANSWERS
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    chemistry topical questions and answers for kcse exams

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