INSTRUCTIONS TO THE CANDIDATES:-
- Answer all the questions in the spaces provided.
- Mathematical tables and electronic used calculators may be
- All working MUST be clearly shown where necessary.
- Matter exists in three states which can be related as shown in the diagram below.
Name processes: P: ………………………………………… (1mk)
R: ………………………………………………….. (1mk) -
- Give one reason some of the laboratory apparatus are made of ceramics. (1 mark)
- Name two apparatus that can be used to measure approximately 75 cm of dilute sulphuric (VI) acid. (2 marks)
- Draw the procedural set-ups that can be used to separate a mixture of sand and calcium chloride to obtain crystals of calcium chloride. (3 marks)
- State two applications of chromatography. (2 marks)
-
The above set-up was used to determine the chemical properties of carbon (II) oxide.- Write the chemical equation for the reaction taking place in the combustion tube. (1 mark)
- State and explain the observation made in the boiling tube. (2 marks)
- A student placed some hydrogen peroxide in a test tube then added a small amount of Solutions can be classified as acids, bases or neutral. The table below shows solutions and their pH values
Solution pH - values K 1.5 L 7.0 M 14.0 - Select any pair that would react to form a solution of pH 7 (1 Mark)
- Identify two solutions that would react with aluminium hydroxide. Explain (2 Marks)
- 9.12g of a gaseous compound contains 8g of silicon while the rest is hydrogen. Determine the empirical formula of the compound. (H = 1, Si = 28) (3 Marks)
- Study the set-up below and answer the questions that follow.
- Why is aqueous ammonia warmed gently? (1 Mark)
- What is the colour of the flame? (1 Mark)
- Write the chemical equation for the reaction that takes place (1Mark)
-
- Chlorine can be prepared in the laboratory by using the following reagents and chemicals. Concentrated sulphuric (VI) acid, water, manganese (IV) oxide, concentrated hydrochloric acid.
- State the role of concentrated sulphuric (VI) acid. (1 mark)
- Write the equation for formation of chlorine. (1 mark)
- What is the role of manganese (IV) oxide? (1 mark)
- Chlorine can be prepared in the laboratory by using the following reagents and chemicals. Concentrated sulphuric (VI) acid, water, manganese (IV) oxide, concentrated hydrochloric acid.
-
- State Boyle’s law. (1 mark)
- A gas occupies 270cm3 at a pressure of 660mmHg at 37°C. What is the new volume if pressure is changed to 810 mmHg at 63°C? (2 marks)
- An organic compound contain s 24.24% carbon, 4.04% hydrogen and the rest chlorine. If its relative molecular mass is 99, what is its molecular formula? (3 marks)
(C = 12, H = 1, Cl = 35.5) - A given mass of sodium nitrate was heated completely and 320cm3 of the gas was produced at s.t.p. Determine the mass of the sodium nitrate heated.
(Na = 23. N = 14, O = 16, molar gas volume = 22.4L) (3 marks) -
- Give one advantage of using methyl orange over phenolphthalein as an indicator. (1 mark)
- Three drops of litmus solution was added to 20cm3 of 2M hydrochloric acid in a beaker followed by 20cm3 of 2M ammonium hydroxide. State and explain the observation made. (2 marks)
- Study the flow chart below and answer the questions that follow.
- Identify solid G………………………………………………………………… (1mk)
- Write a balanced chemical equation between the yellow solid and dilute nitric acid. (1mk)
- Study the diagram below and answer the questions that follow.
- Define the term electrolysis. (1 mark)
- On the diagram, label the Anode and Cathode. (2 marks)
- Write the equation at the anode. (1 mark)
- In order to find the proportion by volume of gases in air, a sample of air was passed through two wash bottles, the first containing sodium hydroxide solution and the second containing concentrated sulphuric (VI) acid. The remaining gas was then collected in a syringe.
- Why was the air passed through;
- sodium hydroxide solution? (1 mark)
- concentrated sulphuric (VI) acid? (1 mark)
- Name is the major gas collected in the syringe. (1 mark)
- Why was the air passed through;
- During the manufacture of sodium carbonate in the industry.
- Give the name of the process to manufacture sodium carbonate. (1 mark)
- Write the final equation to form sodium carbonate during the process. (1 mark)
- Give one use of sodium carbonate. (1 mark)
- Describe how to prepare crystal of magnesium sulphate starting with magnesium powder.(3mks)
-
- Complete the diagram below to show how dry sample of hydrogen gas is prepared in the laboratory. (2 marks)
- Name the catalyst which could be used to increase the reaction rate of production of hydrogen gas in the set up drawn above. (1 mark)
- Complete the diagram below to show how dry sample of hydrogen gas is prepared in the laboratory. (2 marks)
- An element consists of two isotopes with atomic masses 59 and 61 in the ratio of 3 : 2 respectively.
- What are isotopes? (1 mark)
- Calculate the relative atomic mass of the element. (2 marks)
- An element:
- To which chemical family does it belong? (1 mark)
- Write the electron arrangement of the atom. (1 mark)
- Draw the structure of its ion. (1 mark)
- If 25cm3 of 0.1M H2SO4 solution neutralized a solution contain 1.06g of sodium carbonate in 250cm3 of solution, calculate the morality and volume of sodium carbonate solution. (Na = 23, O = 16, C = 12) (3 Marks)
- 50cm3 of oxygen gas diffused through a porous plug in 80 seconds. How long will it take 100cm3 of sulphur (IV) oxide to diffuse through the same plug? (S = 32, o = 16) (3 Marks)
-
- State the role of the following parts during fractional distillation of a mixture of water and ethanol
- Glass beads in the fractionating column (1 Mark)
- Fractionating column (1 Mark)
- State any one application of fractional distillation (1 Mark)
- State the role of the following parts during fractional distillation of a mixture of water and ethanol
-
- State what is observed when sodium hydroxide pellets are left in air overnight.(1 mark)
- What name is given the process shown by the salt in (a) above? (1 mark)
- Given;
- Identify;
Solid F - …………………………………………………………………………. (1 mark)
Solid J - …………………………………………………………………………… (1 mark) - Write equation for step 1. (1 mark)
- Identify;
- Use dot (•) and cross (X) to show the bonding in Lithium oxide. (2 mark)
- Excess magnesium ribbon was burnt in air to form a white solid mixture. Write two equations to show the formation of the white solid mixture. (2 marks)
- The set-up below shows how gas A was prepared and reacted with heated magnesium
- Give a reason why it is not advisable to heat magnesium before heating ammonium nitrite. (1mk)
-
- Identify gas A ....................................................................... (1mk)
- Write a chemical equation for the reaction between gas A and magnesium (1mk)
- Study the set-up below and answer questions that follow.
- Name the gas that is produced when concentrated sulphuric (VI) acid reacts with the sodium chloride (1 mark)
- Why is it necessary to use a funnel in the beaker? (1 mark)
- How does the gas affect the PH of the water in the beaker? (1 mark)
MARKING SCHEME
- Matter exists in three states which can be related as shown in the diagram below.
Name processes: P: ……Evaporation…………………………………… (1mk)
R: …………Condensation/ freezing……………………………………….. (1mk) -
- Give one reason some of the laboratory apparatus are made of ceramics. (1 mark)
- Because they do not react with laboratory chemicals.
- Name two apparatus that can be used to measure approximately 75 cm of dilute sulphuric (VI) acid. (2 marks)
- Measuring cylinder
- Burette
- Beaker
- Give one reason some of the laboratory apparatus are made of ceramics. (1 mark)
- Draw the procedural set-ups that can be used to separate a mixture of sand and calcium chloride to obtain crystals of calcium chloride. (3 marks)
- State two applications of chromatography. (2 marks)
- To identify banned substances in sports.
- To test for drug purity
- To identify contaminants in foods and drinks.
- To identify harmful substnaces in cosmetics.
-
The above set-up was used to determine the chemical properties of carbon (II) oxide.- Write the chemical equation for the reaction taking place in the combustion tube. (1 mark)
CO(g) + CuO(s) → Cu(s) + CO2(g) - State and explain the observation made in the boiling tube. (2 marks)
- Colour of CuO changes from black to browm copper
- Write the chemical equation for the reaction taking place in the combustion tube. (1 mark)
- A student placed some hydrogen peroxide in a test tube then added a small amount of Solutions can be classified as acids, bases or neutral. The table below shows solutions and their pH values
Solution pH - values K 1.5 L 7.0 M 14.0 - Select any pair that would react to form a solution of pH 7 (1 Mark)
- K and M
- Identify two solutions that would react with aluminium hydroxide. Explain (2 Marks)
- K and M because aluminium hydroxide is amphoteric hydroxide.
- Select any pair that would react to form a solution of pH 7 (1 Mark)
- 9.12g of a gaseous compound contains 8g of silicon while the rest is hydrogen. Determine the empirical formula of the compound. (H = 1, Si = 28) (3 Marks)
Si H
8 1.12
8/28 1.12/1
0.286 1.12
0.286 0.286
1 4
= SiH4 - Study the set-up below and answer the questions that follow.
- Why is aqueous ammonia warmed gently? (1 Mark)
- To produce ammonia vapours /gas
- What is the colour of the flame? (1 Mark)
- green-yellow flame
- Write the chemical equation for the reaction that takes place (1Mark)
- 4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g)
- Why is aqueous ammonia warmed gently? (1 Mark)
-
- Chlorine can be prepared in the laboratory by using the following reagents and chemicals. Concentrated sulphuric (VI) acid, water, manganese (IV) oxide, concentrated hydrochloric acid.
- State the role of concentrated sulphuric (VI) acid. (1 mark)
- Drying agent
- Write the equation for formation of chlorine. (1 mark)
- MnO2(s) + 4HCl(l) → MnCl2(aq) + H2O(l) + Cl2(g)
- What is the role of manganese (IV) oxide? (1 mark)
- Oxidising agent
- State the role of concentrated sulphuric (VI) acid. (1 mark)
- Chlorine can be prepared in the laboratory by using the following reagents and chemicals. Concentrated sulphuric (VI) acid, water, manganese (IV) oxide, concentrated hydrochloric acid.
-
- State Boyle’s law. (1 mark)
- The volume of a given mass of gas is inversely propotional to its pressure at constant temperature.
- A gas occupies 270cm3 at a pressure of 660mmHg at 37°C. What is the new volume if pressure is changed to 810 mmHg at 63°C? (2 marks)
V1 = 270cm3 V2 =?
P1 = 660mmHg P2 = 810mmHg
P1V1 = P2V2
270 × 660 = 810V2
V2 = 270 × 660
810
V2 = 220cm3
- State Boyle’s law. (1 mark)
- An organic compound contain s 24.24% carbon, 4.04% hydrogen and the rest chlorine. If its relative molecular mass is 99, what is its molecular formula? (3 marks)
(C = 12, H = 1, Cl = 35.5)
C H Cl
24.24 4.04 71.72
12 1 35.52
2.02 4.04 2.02
2.02 2.02 2.02
1 2 1
E.F CH2Cl
(CH2Cl) × n = 99
49.5n = 99
n = 99
49.5
n = 2
M.F C2H4Cl2 - A given mass of sodium nitrate was heated completely and 320cm3 of the gas was produced at s.t.p. Determine the mass of the sodium nitrate heated.
(Na = 23. N = 14, O = 16, molar gas volume = 22.4L) (3 marks)
2NaNO3 2NaNO2 + O2
2 2 1
Moles of gas
1mole = 22400cm3
= 320cm3
320 = 0.0143
22400
0.0143 × 2 = 0.0286 moles of NaNO3
Mass of NaNO3 = 0.0286 × 85
= 2.431g -
- Give one advantage of using methyl orange over phenolphthalein as an indicator. (1 mark)
- Methyl orange is used in neutralization and reaction between carbonates and dil. acids while phenolphthalein is used in neutralization only.
- Three drops of litmus solution was added to 20cm3 of 2M hydrochloric acid in a beaker followed by 20cm3 of 2M ammonium hydroxide. State and explain the observation made. (2 marks)
- The colour changes from colourless to pink to the neutralization reaction (formation of NH4Cl)
- Give one advantage of using methyl orange over phenolphthalein as an indicator. (1 mark)
- Study the flow chart below and answer the questions that follow.
- Identify solid G………………………………………………………………… (1mk)
- Lead (II) Nitrate
- Write a balanced chemical equation between the yellow solid and dilute nitric acid. (1mk)
- PbO(s) + 2HNO3(aq) →Pb(NO3)2(aq) + H2O(l)
- Identify solid G………………………………………………………………… (1mk)
- Study the diagram below and answer the questions that follow.
- Define the term electrolysis. (1 mark)
- Is the process of decomposing an electrolyte by passing an electric current.
- On the diagram, label the Anode and Cathode. (2 marks)
- Write the equation at the anode. (1 mark)
- 2Cl−(l) → Cl2(g) + 2e−
- Define the term electrolysis. (1 mark)
- In order to find the proportion by volume of gases in air, a sample of air was passed through two wash bottles, the first containing sodium hydroxide solution and the second containing concentrated sulphuric (VI) acid. The remaining gas was then collected in a syringe.
- Why was the air passed through;
- sodium hydroxide solution? (1 mark)
- To remove carbon (IV) oxide
- concentrated sulphuric (VI) acid? (1 mark)
- To absorb water vapour/ remove water vapour
- sodium hydroxide solution? (1 mark)
- Name is the major gas collected in the syringe. (1 mark)
- Nitrogen
- Why was the air passed through;
- During the manufacture of sodium carbonate in the industry.
- Give the name of the process to manufacture sodium carbonate. (1 mark)
- Solvay process
- Write the final equation to form sodium carbonate during the process. (1 mark)
- 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(l)
- Give one use of sodium carbonate. (1 mark)
- Manufacture of glass
- Softening of water
- Give the name of the process to manufacture sodium carbonate. (1 mark)
- Describe how to prepare crystal of magnesium sulphate starting with magnesium powder.(3mks)
- React excess magnesium powder with dil. sulphuric acid to obtain magnesium sulphate
- Filter to obtain the filtrate
- Heat the filtrate to saturation and allow it to cool to obtain the crystals.
- Dry the crystals between two filter papers.
-
- Complete the diagram below to show how dry sample of hydrogen gas is prepared in the laboratory. (2 marks)
- Name the catalyst which could be used to increase the reaction rate of production of hydrogen gas in the set up drawn above. (1 mark)
- Crystals of Copper (II) Sulphate.
- Complete the diagram below to show how dry sample of hydrogen gas is prepared in the laboratory. (2 marks)
- An element consists of two isotopes with atomic masses 59 and 61 in the ratio of 3 : 2 respectively.
- What are isotopes? (1 mark)
- Are atoms with the same atomic number but different mass number
- Calculate the relative atomic mass of the element. (2 marks)
59 × 3 + 61 × 2
2+3
177 + 122
5
299
5
= 59.8
- What are isotopes? (1 mark)
- An element:
- To which chemical family does it belong? (1 mark)
- Alkaline Earth Metal
- Write the electron arrangement of the atom. (1 mark)
- 2.8.2
- Draw the structure of its ion. (1 mark)
- To which chemical family does it belong? (1 mark)
- If 25cm3 of 0.1M H2SO4 solution neutralized a solution contain 1.06g of sodium carbonate in 250cm3 of solution, calculate the morality and volume of sodium carbonate solution. (Na = 23, O = 16, C = 12) (3 Marks)
Molarity of Na2CO3
1.06 × 4 = 4.24
106 106
=0.04M
Na2CO3 + H2SO4 → Na2CO3 + CO2 + H2O
1 1
Moles of H2SO4
25 × 0.1
1000
= 0.0025 moles
Vol = 0.0025 × 1000
0.04
= 62.5cm3 - 50cm3 of oxygen gas diffused through a porous plug in 80 seconds. How long will it take 100cm3 of sulphur (IV) oxide to diffuse through the same plug? (S = 32, o = 16) (3 Marks)
-
- State the role of the following parts during fractional distillation of a mixture of water and ethanol
- Glass beads in the fractionating column (1 Mark)
- To increase the surface area for condensation
- Fractionating column (1 Mark)
- Is to allow water vapour to condense into liquid and flow back into the flask
- Glass beads in the fractionating column (1 Mark)
- State any one application of fractional distillation (1 Mark)
- Distillation of crude oil
- Recycling of used oil
- Fractional distillation of liquid air to manufacture nitrogen and oxygen.
- State the role of the following parts during fractional distillation of a mixture of water and ethanol
-
- State what is observed when sodium hydroxide pellets are left in air overnight.(1 mark)
- It wets up/ absorbs water to form a solution.
- What name is given the process shown by the salt in (a) above? (1 mark)
- Deliquescence
- State what is observed when sodium hydroxide pellets are left in air overnight.(1 mark)
- Given;
- Identify;
Solid F - …………………………Copper (II) Carbonate………………………………………………. (1 mark)
Solid J - ……………………Copper (II) Sulphate……………………………………………………… (1 mark) - Write equation for step 1. (1 mark)
- CuCO3(s) CuO(s) + CO2(g)
- Identify;
- Use dot (•) and cross (X) to show the bonding in Lithium oxide. (2 mark)
Li2O - Excess magnesium ribbon was burnt in air to form a white solid mixture. Write two equations to show the formation of the white solid mixture. (2 marks)
2Mg(s) + O2(g) → 2MgO(s)
3Mg(s) + N2(g) → Mg3N2(s) - The set-up below shows how gas A was prepared and reacted with heated magnesium
- Give a reason why it is not advisable to heat magnesium before heating ammonium nitrite. (1mk)
- Because it will be oxidised by oxygen in the combustion tube
-
- Identify gas A ............Nitrogen gas............................ (1mk)
- Write a chemical equation for the reaction between gas A and magnesium (1mk)
- 3Mg(s) + N2(g) → Mg3N2(s)
- Give a reason why it is not advisable to heat magnesium before heating ammonium nitrite. (1mk)
- Study the set-up below and answer questions that follow.
- Name the gas that is produced when concentrated sulphuric (VI) acid reacts with the sodium chloride (1 mark)
- Hydrogen Chloride gas
- Why is it necessary to use a funnel in the beaker? (1 mark)
- To increase the surface of absorption
- How does the gas affect the PH of the water in the beaker? (1 mark)
- The pH reduces
- Name the gas that is produced when concentrated sulphuric (VI) acid reacts with the sodium chloride (1 mark)
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