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KCSE Chemistry PAPER 2 2013 WITH ANSWERS

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Kenya Certificate of Secondary Education Chemistry Past Paper 2

KCSE Chemistry Paper 2 2013 Questions and Answers
KCSE Past Papers 2013 CHEM Paper 2

CHEM paper 2

1 )The grid given below represents part of the periodic table. Study it and answer the questions that follow. The letters do not represent the actual symbols of elements. M N P T R

a)(i) Select a letter which represents an element that loses electrons most readily.Give a reason for your answer. (2 marks)

(ii) Explain why the atomic radius of P is found to be smaller than that of N. (2 marks)

(iii) Element M reacts with water at room temperature to produce 0.2 dm~‘ of gas. Determine the mass of M which was reacted with water. (Molar gas volume at room temperature is 24 dma, Relative atomic mass of M = 7). (3 marks)

b) Use the information in the table below to answer the questions that follow. (The letters are not the symbols of the elements)

Element. State of oxide at Type of oxide Bonding in oxide room temperatureSolid Acidic Covalent

Solid Basic Ionic

Liquid Neutral Covalent, p> Gas Neutral

Covalent

b)Identify a letter which represents an element in the table that could be calcium, carbon or sulphur. Give a reason in each case.

(i) Calcium:

…………………………………………………………………………………… ..(2 marks)

Reason

………………………………………………………………………………………… ..

(ii) Carbon:

…………………………………………………………………………………….. ..(2 marks)

Reason . . . . . . . . . . . . . . . . . . . . . . . . . . . ..

(iii) Sulphur:

……………………………………………………………………………………. ..(2 marks)

Reason

………………………………………………………………………………………… ..

2 (a) (i) What is meant by the term ‘Enthalpy of formation“? (1 mark) (ii) The enthalpies of combustion of carbon, methane and hydrogen are indicated below:

I0 Draw an energy cycle diagram that links the enthalpy of formation of methane to enthalpies of combustion of carbon, hydrogen and methane. (2 marks)

II) Determine the enthalpy of formation of methane. (2 marks)(b) .An experiment was carried out where different volumes of dilute hydrochloric acid and aqueous sodium hydroxide both at 25°C were mixed and stirred with a thermometer. The highest temperature reached by each mixture was recorded in the table below:

b)On the grid provided, plot a graph of highest temperature (vertical axis) against

(i) Identify X. (ii) Using your graph, detemiine the:l highest temperature reached;

II volume of acid and base reacting when highest temperature is reached;

(iii) Calculate the amount of heat liberated during the neutralisation process (Specific heat capacity is 4.2 J g‘ K‘ and the density of solutions is 1.0 g cm )

c) The molar enthalpy of neutralisation between hydrochloric acid and ammonia solution was found to be -52.2 kJ mol”, while that of hydrochloric acid and sodium hydroxide was -57.1 kJ mol”. Explain the difference in these values. (2 marks)

3 a) The diagram below shows the Frasch process used for extraction of sulphur. Use it to answer the questions that follow.

(1 mark)(ii) Why is it necessary to use super heated water in this process? (1 mark) (iii) State two physical properties of sulphur that makes it possible for it to be extracted by this method. (2 marks)

(b) The diagram below shows part of the processes in the manufacture of sulphuric (VI) acid. Study it and answer the questions that follow.

(i) Write an equation for the formation of sulphur (IV) oxide from sulphur.

(ii) What is the role of concentrated sulphuric (VI) acid in chamber A? (1 mark)

(iii) Name two catalysts that can be used in the catalytic chamber B. (2 marks) (c) Explain one way in which sulphur (IV) oxide is a pollutant. (I mark)

(d) What observation will be made when a few drops of concentrated sulphuric (VI) acid are added to crystals of sugar? Explain your answer. (1 mark)

(4) a) The set up below can be used to produce sodium hydroxide by electrolysing brine.

Identify gas Y. (1 mark)

(ii) Describe how aqueous sodium hydroxide is formed in the above set-up.

(iii) One of the uses of sodium hydroxide is in the manufacturing of soaps. (2 marks)

State one other use of sodium hydroxide. (1 mark)

(b) Study the information given rn the table below and answer the questions that follow.

i) Construct an electrochemical cell that will produce the largest emf. (3 marks)

ii)Calculate the emf of the cell constructed in (i) above. (2 marks)

iii) Why is it not advisable to store a solution containing E‘ ions in a container made of H? (2 marks)

5. a) Describe one method that can be used to distinguish between sodium sulphate and sodium hydrogen sulphate. starting with lead metal.

(c) Study the flow chart below and answer the questions that follow:

(i) Write an equation for the reaction in:

I step II;

II step IV.

(ii) State the observation made in step IH. Explain.

(iii) Name another suCHEMance that can be used in step V.

6. (a) Distinguish between a neutron and a proton.

(b) What is meant by a radioactive suCHEMance?

(c) State two dangers associated with radioactive suCHEMances in the environment. (2 marks)

(b) Describe how a pure sample of lead (II) sulphate can be prepared in the laboratory

(d) The two isotopes of hydrogen, deuterium (iD) and tritium (iT) react to form element Y and neutron particles, according to the equation below:

(i) What is the atomic:

(I) mass of Y; (l mark)

(II) number of Y. (l mark)

(ii) What name is given to the type of reaction undergone by the isotopes 0f_ hydrogen? (1 mark)

(e) (i) What is meant by half-life of a radioactive suCHEMance? (1 mark)

(ii) 288g of a radioactive suCHEMance decayed to 9g in 40 days. Determine the half-life of the radioactive suCHEMance. (2 marks)

7. (a) Give the systematic names for the following compounds:

(i) Cl-13C]-IZCOOH; (1 mark)

(ii) CH3CH2CH2CHCHZ; (1 mark)

(iii) cn c cnzcna. (1 mark)

(b) Study the flow chart below and use it to answer the questions that follow:

C1 (2)

(i) Identify the organic compound K. (l mark)

(ii) Write the formula of M.

(iii) Give one reagent that can be used in:

(I) step I;

(II) step II.

(iv) Write the equation of the reaction in step III.

c) The structure below represents a type of a cleansing agent.

R S05 Na

Describe how the cleansing agent removes grease from a piece of cloth. (3 marks)

KCSE Chemistry Paper 2 2013 Questions and Answers

KCSE Chemistry Marking schemes Paper 2 2013

CHEM paper 2

***coming soon***

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KCSE Chemistry Paper 1 2013

->> Click Here to download Chemistry KCSE Paper 1 2013 PDF

KCSE Chemistry Paper 3 2013

->> Here are the KCSE Chemistry Paper 3 2013 exams that are available

4.5.3 Chemistry Paper 3 (233/3)

1 You are provided with:

• solution A’ aqueous copper (H) sulphate;
• solid B, iron powder;
• 0.02 M acidified potassium manganate (VII), solution C.You are required to determine the molar heat of displacement of copper by iron.

  Procedure I

  Using a burette, place 50.0 cm’ of solution A in a 100 ml beaker. Measure the temperature of the solution and record it in table 1 below. Add all of solid B provided at once and start a‘ stop watch. Stir the mixture thoroughly with the thennometer and record the temperature of the mixture after every one minute in the table. Retain the mixture for use in procedure II below.

  

  (a) (i) Plot a graph of temperature (vertical axis) against time in the grid provided. (3 marks)(ii) From the graph, determine the;

  (I) highest change in temperature, AT; (1 mark)

  (II) time taken for reaction to be completed. (1mark)

  (iii) Calculate the heat change for the reaction. (Specific heat capacity of solution is 4.2 Jg” K”; Density of the solution is l gem”). (2 marks)

  Procedure II Carefully decant the mixture obtained in procedure I into a 250 ml volumetric flask. Add about 10 cm’ of distilled water to the residue in the 100 ml beaker. Shake well, allow the mixture to settle and carefully decant into the volumetric flask. Immediately, add about 50 cm‘ of 2 M sulphuric (VI) acid to the mixture in the volumetric flask. Add more distilled water to make 250.0 cm‘ of solution. Label this as solution D. Fill a burette with solution C. Using a pipette and a pipette filler, place 25.0 cm’ of solution D into a 250 ml conical flask. Titrate solution D against solution C until the first permanent pink colour is obtained. Record your results in table 2 below. Repeat the titration two more times and complete the table. Retain the remaining solution C for use in question 3.

  TABLE II

  

  (a) Determine the average volume of solution C used. (1% mark)(b) Calculate the number of moles of:

  (i) aqueous potassium manganate (VII) used; (1 mark)

  (ii) iron (II) ions in 25 .0 cm3 of solution D. (1 mole of MnOZ reacts with 5 moles of Fe“). (1 mark

  (iii) iron(II) ions in 250 cm‘ of solution D. (1 mark)

  (c) Calculate the molar heat of displacement of copper by iron. (2 marks) 2.You are provided with solid E. Carry out the following tests and write your observations and inferences in the spaces provided.

  (a) Place all of solid E in a boiling tube. Add about 10 cm’ of distilled water and shake thoroughly. Filter the mixture into another boiling tube. Retain the filtrate for use in test 2

  (b) below. Dry the residue using pieces of filter papers.

  (i) Transfer about half of the dry residue into a dry test-tube. Heat the residue strongly and test any gas produced using a burning splint.

  

  ii) Place the rest of the residue in a dry test—tube. Add 4 cm’ of 2M hydrochloric acid. Retain the mixture for test (m) below.

  

  iii) To 2 cm-‘ of the solution obtained in (ii) above, add 6 cm-‘ of aqueous ammonia dropwise.

  

  (b) (i) To 2 cm-‘ of the filtrate obtained in (a) above, add about 3 cm3 of aqueous ammonia (Excess).

  

  ii) To 2 cm’ of the filtrate, add about 2 cm’ of 2M hydrochloric acid.

  

  iii) T0 2 cm-‘ of the filtrate, add one or two drops of barium nitrate solution.

  

  3. You are provided with solid G. Carry out the tests in (a) and (b) and write your observations and inferences in the spaces provided. Describe the method used in part (c). (a) Place about one third of solid G on a metallic spatula and bum it in a Bunsen burner flame.

  

  (b) Dissolve all of the remaining solid G in about 10 cm’ of distilled water in a boiling tube. Use the solution for tests. (i) Place 2 cm-‘ of the solution in a test-tube and add 2 drops of acidified potassium manganate (VII); solution C.

  

  ) (ii) To 2 cm‘ of the solution, add all of solid sodium hydrogen carbonate provided.

  

  (c) Determine the pH of the solution obtained in (b) above.

  

  Check the answers to this paper 3 on the paper 1 page.

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