(a) Outline seven ways in which King Jeroboam promoted the spread of idolatry in Israel. (7 mks)

(b) Give seven reasons why Elijah was uncompromising in his attitude to the worship of Baal.    (7 mks)

(c) State six reasons why Christians should fight against the spread of devil worship in the society. (6 mks)

(a) Describe the call of Moses in Exodus 3:1-22. (8 marks)

(b) Give reasons why Moses was reluctant to go back to Egypt. (6 marks)

(c) What do Christians learn about God from the call of Moses? (6 marks)

(a) Outline seven importance of CRE to a secondary school student in Kenya. (7mks)

(b) Describe the second account of creation in Genesis 2:4b-25. (7mks)

(c) Give six traditional African views of creation. (6mks)

You are provided with solid T. Carry out the tests below and write your observations and inferences in the spaces provided.

a) Using a metallic spatula, heat about one half of solid T in a Bunsen burner flame.

b) Dissolve the remaining portion of solid T into about 10cm³ of distilled water. Label this solution as solution T. Use this solution for the following tests.

i)To about 2cm³ of solution T, add 3drops of acidified potassium manganate (VII) and warm.

ii) To about 2cm³ of solution T, add 2drops of bromine water.

iii) Place 2cm³ of solution T in a test-tube and add solid carbonate.

iv) To the remaining portion of solution T, test using litmus papers.

a) You are provided with solution Q. Carry out the tests below. Record your observations and inferences in the spaces provided. Place 3cm³ of solution Q in a boiling tube. Add 12cm³ of distilled water and shake.

RETAIN THE REMAINDER OF SOLUTION Q FOR USE IN (b)

i) Use about 2cm³ portions of diluted solution Q for tests I and II.

I)  To the first portion, add drop wise about 1cm³ of sodium hydroxide.

II)  To the second portion, add 2 to 3 drops of barium chloride solution.

ii) To 3cm³ of the diluted solution Q, add dropwise the chlorine water.

iii) To 2cm³ of diluted solution Q, add drop wise the bromine water provided.

iv) To 2cm³ of the diluted solution Q, add 2or 3 drops of lead (II)nitrate solution.

b) You are provided with;

    Solution P containing barium ions,

    Solution R containing potassium ions.

    Solution S containing sodium ions.

Carry out the tests on solutions P,R,S and Q in order to identify the cation present in solution Q.

PROCEDURE

Clean one end of the glass rod thoroughly. Dip the clean end of the glass rod in solution P. Remove the end and heat it in the non-luminous part of a Bunsen burner flame. Note the colour of the flame and record it in table 2. Allow the glass rod to cool for about TWO minutes. Repeat the procedure with solutions R,S and Q and complete the table.

                                                                                               (4mks)

ii) Identify the cation present in solution Q.                    (1mk)

You are provided with the following:

• Hydrogen Peroxide labelled solution J.
• Dilute sulphuric acid labelled solution K.
• Sodium thiosulphate labelled solution L.
• Potassium Iodide labelled solution M.
• Starch solution labelled solution N.
• Distilled water in a wash bottle.

You are required to determine how the rate of reaction of hydrogen peroxide with potassium iodide varies with the concentration of hydrogen peroxide.

PROCEDURE.

- Label two 200ml or 250ml beakers as beaker 1 and beaker 2. Using a burette, place 25.0cm³ of solution J into beaker 1.Into the same beaker, add 20cm³ of solution K using a 50ml or 100ml measuring cylinder. Shake the contents of beaker 1.

- Using a 10ml measuring cylinder, place 5cm³ of solution L into beaker 2 followed by 5cm3 of solution M then 2cm³ of solution N. Shake the contents of beaker 2. Pour  the contents of beaker 2 into beaker 1 and start a stop clock /watch IMMEDIATELY.

- Swirl the mixture and let it stand. Note the time taken for the blue colour to appear. Record the time in the space provided for experiment 1 in the table below. Clean beaker 1. Repeat the procedure with volumes of water, solutions J,K,L,M and N as shown in the table for experiments 2 to 5. Complete the table by computing ¹/_time (sec^-1)

a)  TABLE I

                                                                                                                              ( 7 ½ mks)

b) Plot a graph of  ¹/_time (sec^-1)  (y-axis) against volume of hydrogen peroxide.            (4mks)

c) From your graph ,determine the time that would be taken if the contents  of beaker 1 were  17.5cm³ water, 7.5cm³ solution J and 20cm³ solution K.                                 (2mks)

d) How does the rate of reaction of hydrogen peroxide with potassium iodide vary with the concentration of hydrogen peroxide?                          (2mks)

You are provided with solid F. Carry out the test below. Write your observations and inferences in the spaces provided.

a) Place about ½ (half) of solid F on a metallic  spatula and heat over a Bunsen burner flame,

b) Place the remaining solid into a boiling tube. Add about 10cm³ of distilled water and shake well to dissolve.

c) Divide  the solution in (b) above into four portions. To the first portion, in a test-tube, add 3 drops of universal  indicator.

d) To the second  portion in a test-tube, add a spatula-full of sodium hydrogen carbonate

e)To the third portion, add 3 drops of acidified potassium manganate (vii)

You are provided with solid E. carry out tests below. Record your observations and inferences in the spaces provided.

a) Put  about one half of solid E in a dry test-tube and heat it strongly. Test for any gas produced.

b) Dissolve  the rest of the solid E in 10 cm³ of distilled water in boiling tube. Divide solution into 3 portions.

i) To a first portion in test-tube, add aqueous sodium hydroxide dropwise until in excess.

ii) To the second portion in test tube, add aqueous  ammonia solution dropwise until in excess

iii) To the  third portion in a test-tube, add lead(ii) Nitrate solution and then warm the mixture.

You are provided with :

i)         Solution A which is 2.0M hydrochloric Acid (HCL)

ii)        Solution B, which is 0.1 M sodium thiosulphate (Na₂S₂O₃)

iii)       Solution C which is  monobasic alkali of 0.1 M concentration

You are required to:

i) Find the effect of change of temperature on the rate of reaction between sodium thiosulphate, solution B and hydrochloric Acid, solution A.

ii)  Prepare a dilute solution of hydrochloric acid, solution A

iii) Write an ionic equation for the reaction  between hydrochloric acid solution A and the alkali solution C.

Procedure I

- Using a  measuring cylinder measure 10 cm³ of solution B  into a clean  100 cm³ glass beaker. Place it together with its content on a white piece of paper with  a cross(X) written on it with bold blue print. Measure the temperature of the solution and record it as shown in the table below.

- Using a clean measuring cylinder, measure 5 cm³ of solution A. add it to the contents of the beaker containing solution B and immediately set  on the stop watch. Record the time  it will take for the cross (X) to become invisible when viewed above the reaction mixture in the beaker.

- Wash the glass beaker used and repeat the experiment at the temperature  indicated in the  table below by warming  sodium thiosulphate solution B to  the  stated temperature before adding hydrochloric Acid, solution A.

Table I

                                                                                                                                                (5mks)

Note:

Sodium  thiosulphate solution reacts with dilute  hydrochloric acid to form a yellow precipitate  of colloidal sulphur as shown  in the equation below.

Na₂S₂O_3(aq) + 2HCl_(aq) ------------> S_(s)+SO_2(g) + 2NaCl_(aq)+H₂O_(l)

              a) On the grid provided, plot a graph of  reciprocal of time ¹/_t against temperature   (3marks)

b) Comment on the effect of change in temperature on the reaction between sodium thiosulphate, solution B and hydrochloric acid, solution A.          (2mks)

………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………

c)         Use your graph to determine:

            i) The time taken by the  reaction when the temperature is 58⁰C.          (1mk)

            ii) The temperature at which the rate  of the reaction is 0.045 sec^-1          (1mk)

Procedure II

Using a clean measuring  cylinder, place 12.5 cm³ of solution A in 250ml volumetric flask. Add 200 cm³ of distilled water  and shake. Add distilled water upto the mark. Label this solution D. Fill a burette with solution D. Using a pipette and a pipette filler, place 25.0 cm³ of solution C  into a 250 ml conical  flask. Add two drops of phenolphthalein indicator and titrate  with solution D  until the pink colour disappears.

Record your results in table II. Repeat the titration  two more times and complete the table.

                        Table II

                                                                                                             (3mks)

            d)         Calculate:

                        i)         The average volume of solution D used.                                            (1 mark)

                        ii)        Moles of hydrochloric Acid, solution D used.                                   (2 mark)

                        iii)       Moles of Alkali solution C used.                                                        (1 mark)

e)  Write ionic equation for the reaction between hydrochloric acid, solution A and Alkali, solution C.                                  (1mk)

You are provided with solid F. Carry out the tests below. Record your observations

And inferences in the spaces provided.

(a) Place about half of solid F on a metallic spatula and burnt it using a non-luminous

(b) Place the remaining solid F in a clean boiling tube and add about 10cm³ of water and shake thoroughly.

i) To about 2cm³ of the solution F, put the universal indicator paper

(ii) To about 2cm³ of solution F, add 2cm³ of acidified potassium dichromate (VI) and warm to boiling

(iii)      To about 2cm³ of solution F, add three drops of bromine water

(iv) To about 2cm³ of solution F, add three drops of acidified potassium manganate (VII) solution; then warm