General Chemistry Revision Questions

General Revision for Ordinary Level Chemistry

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Senior one to Senior Four Revision Questions

Write the answers in the spaces provided

a) State how the mixtures of the following substances can be separated

MIXTURE	METHOD
Sulphur and Iron
Oxygen and Nitrogen
Iodine and Potassium Sulphate
Sodium Chloride and Sodium Carbonate
Ink

b) State one difference between a chemical and a physical change

………………………………………………………………………

c) State whether the following is a physical or a chemical change

i) Heating iodine

………………………………………………………………………

ii) Heating a piece of Magnesium ribbon in air

………………………………………………………………………

iii) Heating Sodium carbonate.

………………………………………………………………………

d)State what is observed when Iron (III) Chloride was heated.

……………………………………………………………………

2.a)State how a Non Luminous flame is obtained on a Bunsen burner.

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

b)Give examples in everyday life of:

i)Luminous flame

………………………………………………………………

ii)Non luminous flame

…………………………………………………………………

c)Why is luminous Bunsen flame not used in the laboratory?

…………………………………………………………………

d)State the differences between a luminous and Non –luminous flame.

LUMINOUS FLAME	NON-LUMINOUS FLAME

3.(a)What are the three states of matter?

……………………………………………………………………………………………………………………………………………………………………………………………....

(b)In what state are particles?

i)Further apart.

…………………………………………………………………

ii)Closest together.

…………………………………………………………………

(c)What is:

i)an Element

…………………………………………………………………

iii)a Compound

…………………………………………………………………

d)Give one example of the following:

(i)a pure element

…………………………………………………………………

(ii)a pure compound

…………………………………………………………………

(iii)a mixture

…………………………………………………………………

4.a)Draw a well labeled diagram of a Bunsen burner.

b)Describe a method of lighting a Bunsen burner

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

5.a) What is meant by the following terms?

(i)Freezing
………………………………………………………………………………………………………………………………………………… (ii)Condensation

…………………………………………………………………........................................................................................................................ (iii)Melting

………………………………………………………………………………………………………………………………………………… (iv)Evaporation

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

(iv)Sublimation

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

b) Give three examples of substances which sublime.

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

c)Differentiate between a Mixture and a Compound.

MIXTURE	COMPOUND

d)A Senior One Student was sent to buy a sachet of salt from a nearby shop. On her way home she fell down and all the salt poured on the ground. She removed the salt including the soil from the ground. Described the methods of how she will obtain clean salt from this dirty one.

................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................

6.a)What is air?

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

(b)State the components of air and their percentages.

(c)How can the components of air be separated?

(d)What is the effect of increasing the percentage of carbon dioxide in the air?

(e)What natural process removes carbon dioxide from the atmosphere?

……………………………………………………………………

(f)What process adds carbon dioxide in the atmosphere?

……………………………………………………………………

7.(a)Describe the procedure of Industrial Preparation of Oxygen.

………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………................................................................................................................................................................................................................................................................................................

(b)State the uses of Oxygen

(c)Draw and label the experimental set up of the apparatus for the preparation of Oxygen.

(d)(i)What is a Catalyst?

……………………………………………………………………………………….……………………………………………………………………………………….

(ii)What Catalyst is used in the preparation of Oxygen?

……………………………………………………………………

(iii)Write equations to show the different compounds from which oxygen can be prepared.

8.(a)What is rusting?

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

(b)What is the chemical name for rust?

……………………………………………………………………

(c)State the conditions necessary for Iron to rust.

(d)Describe an experiment to show that a special condition is required for Iron to rust.

9.(a)What is an Oxide?

(b)(i)State the different types of Oxides.

(ii)Give examples of each types of Oxide.

(c)(i) Describe what is observed when Carbon, Copper, Phosphorus, Sodium and Magnesium burn in air.

…………………………………………………………………

(ii) Classify the products of burning the elements in oxygen as either acidic or basic.

(e)State whether the following oxides are Acidic, Basic or Amphoteric

i) ZnO

………………………………………………………………...

ii) SO₂…………………………………………………………………

iii) CO …………………………………………………………………

iv) Al ₂O₃………………………………………………………………

v)PbO ………………………………………………………………...

10.(a)Steam was passed over heated Magnesium ribbon in a tube.

(i)State what was observed

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

(ii)Write an equation for the reaction that took place.

(b)The gaseous product formed in (a) was dried and passed over heated Lead (II) Oxide in an ignition tube.

(i)State what was observed

(ii)Write an equation for the reaction that took place.

(c)Arrange the following elements in order of their reactivity starting with the least reactive. Na, K, C, Zn and Fe

(c)Write the equation for the reaction between heat and stream.

11.(a)What is meant by the terms:

(i)Oxidation

(ii)Reduction

(b)Outline the uses of hydrogen

(c)How is hydrogen obtained on a large scale?

(d)Describe the method of preparation of hydrogen and state how it can be tested

12.The full symbol of an atom of an element is 27 X

(a)(i)State the number of protons in X

................................................................................................................................................

(ii)Write the electronic configuration of X

………………………………………………………………………………………………
(iii)State the group in the periodic table to which X belongs

……………………………………………………………………………………....

(b)(i)Write the formula of the Oxide X

………………………………………………………………………………………………

(iii)State the type of the bond that exists in the Oxide of X

………………………………………………………………………………………………

13.(a) Explain giving examples what is meant by:

(i)Basicity of an acid

………………………………………………………………………………………………

(ii)An Acid Salt

(iii)Outline how a pure dry sample of Sodium hydrogen sulphate can be prepared in the laboratory (No equation or diagrams required)

(iv)An acidified solution of barium chloride was added to aqueous Sodium hydrogen Sulphate. State what was observed and write equation for the reaction that took place.

14.(a) Describe how a dry pure sample of chloride can be prepared in the laboratory starting from potassium Manganate VII

(b). State what would be observed and write equation(S) for the reaction(s) that would occur if:
(i) Chloride was bubbled into an aqueous sodium hydroxide
………………………………………………………………………………………..……………………………………………………………………………………………..
(ii) Burning magnesium was lowered into a jar of chlorine

(iii) Chlorine was passed through a solution of potassium iodide

(v) State three uses of Chlorine.

……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………… 15.(a)Describe how a dry sample of hydrogen Chloride gas can be prepared in the laboratory.

(b)Draw a well labeled diagram to show that hydrogen chloride gas is highly soluble in water.

(c) Using equations, explain why when hydrogen chloride gas was bubbled into silver nitrate solution a white precipitate R was formed. R dissolved in Ammonia to form a colourless solution.

(d)The table below shows the variation in solubility of hydrogen chloride with temperature.

Temp. ⁰C	0	30	40	50	60
Solubility of HCl in g/1 of water	824	672	632	596	560

(i)Plot a solubility curve hydrogen chloride in g/litre against temperature.

(Graph paper)

(ii) From your graph determine the solubility of hydrogen chloride at 20 ⁰C.

17.A sample of dry hydrogen can be prepared in the laboratory using Zinc and Dilute Sulphuric acid in presence of a catalyst:

a) Draw a diagram to show a set up of the apparatus that can be used to prepare dry hydrogen in laboratory.

ii) Name the catalyst that can be used in this reaction.

………………………………………………………………………………………………

iii) Write the equation for the reaction leading to the formation of hydrogen.

iv) State how hydrogen can be identified.

b)Dry hydrogen was passed over heated lead (II) Oxide.
i) State what was observed.

ii) Write the equation for the reaction that took place.

………………………………………………………………………………………………………………………………………………………………………………………………
c)Hydrogen burns in Oxygen according to the following equation

2H_2(g) + O_2(g) 2H₂O_(g) +Heat

i)Name one substance that be used to identify the products of combustion of hydrogen in Oxygen.

………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………........................

ii)State what would be observed if the reagent you have named in c(i) above was used to identify the product.

iii) Calculate the volume of hydrogen at s.t.p that would burn in oxygen to produce 5720 J of heat.

(The motor heat of combustion of hydrogen = - 286KJ mo11^-1 of gas occupies 22.4dm³ at s.t.p.)

18.(a)(i)Write the equation to show how ammonia can be prepared from calcium hydroxide.

ii)Name one substance that can be used to dry ammonia.

………………………………………………………………………………………………

b) Ammonia was passed over heated copper (II) oxide,
(i) State what was observed.

(ii)Write the equation for the reaction that took place.

(d) State two use of ammonia gas.

(e) Ammonia when mixed with oxygen and passed over heated platinum catalyst, steam and gas X were formed.
(i) Name gas X.

(ii) Write the equation for the reaction leading to the formation of gas X.

(e) State what is observed when excess ammonia is lowered into a gas jar of Chlorine.

………………………………………………………………………………………………

(ii) Write the equation for the reaction.

(g) When ammonia gas was bubbled through a solution containing Zinc ions, a white precipitate wad formed later dissolved
(i) Write the equation for the reaction leading to the formation of the precipitate.

(ii) Identify the cation in the solution formed when the precipitate dissolved.

(h)State two ways in which the white precipitate can be obtained from colourless Solution.

19.(a)(i)Name one substance which when reacted with dilute Sulphuric Acid can produce Sulphur dioxide.

………………………………………………………………………………………………

(ii) Name the reagent that can be used to confirm the presence of Sulphur dioxide.

(iv) State what is observed when the named reagent is used.

(v)State the property of Sulphur dioxide demonstrated in 10(b) above.

(vi)Describe a method of extracting Sulphur.

(vii)Describe the contract process in the manufacture of Sulphuric acid.

(viii) State three uses of Sulphuric acid.

(ix) State three properties of sulphuric acid

20.(a)What is allotropy?

(b) Name two crystalline allotropes of carbon.

(d) Dilute Hydrochloric Acid was added to calcium carbonate in a conical flask and the gas evolved was passed through aqueous calcium hydroxide solution in the boiling tube.

(a) What was the observed in the conical flask?

(b) Write the equation(s) for the reaction (s).

(i) Between hydrochloric acid and calcium carbonate.

(ii) That took place in the boiling tube.

(iii) State what is observed when excess gas is passed through the boiling tube.

(i) State what was observed.

(ii) Write the equation for the reaction that took place.

(d) To the residue in (c) was added dilute hydrochloric acid solution.

(i) State what was observed.

(ii) Write ionic equation for the reaction that took place

(e) Explain why it is dangerous to use a charcoal stove in a poorly ventilated room.

(f) State the use of carbon dioxide.

(g) Describe the industrial manufacture of sodium carbonate.

21.(a) Write the structural formula of:

(i) Ethene

(ii) Ethane

(iii) Ethanol

(b) Name on reagent which can be used to distinguish between ethane and ethene.

(d)Write the equation for the polymerization of ethane.

22.(a)(i) State what is meant by the term soap

(ii) Briefly describe how a dry sample of soap flakes can be prepared in the Laboratory.

(b)A water sample X was boiled and on cooling was tested by shaking it with a known volume of soap solution. A greasy scum and a cloudy solution were observed.

(i) State what is meant by scum.

………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………(ii) Write an ionic equation for the reaction leading to the formation of scum.

(b)(i) Name one compound that can be used to stop scum formation in the water Sample X.

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

(ii) Write the equation for the reaction that would take place when the compound named in c (i) above is used.

(d)Describe how soap can remove grease from fabrics when washed.

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

23.(a) Describe how dry crystals of lead (II) nitrate can be prepared in the Laboratory from lead (II) oxide.

(b) State what would be observed when to an aqueous solution of lead (II) nitrate was added to:
(i)Sodium Chloride Solution

(ii)Zinc powder

(c)(i) Write equations for the reactions that took place in (i).

(ii) Explain your answer in b (ii).

(Your answer should include equation for the reaction)

(d) Lead (II) nitrate decomposes when heated according to the following equation:
2Pb(NO₃)₂ (s) 2PbO(s) + 4NO₂ (g)+O₂ (g)

Calculate the total volume of the gaseous product formed at the s.t.p when 3.31g of lead (II) nitrate is decomposed (Pb=207, O=16, N=14, I mole of gas occupied 22400cm³.

23. The figure below shows the set up of the apparatus in which electric current was produced by dipping two different metal rods A and B into dilute Sulphuric Acid.

(a) Name one metal that can be used as:

(i) A …………………………………………………………………………………….......

(ii) B ………………………………………………………………………………………..

(b) State which of the metals A and B is the:

(i) Anode:

……………………………………………………………………………………

(ii) Cathode:

………………………………………………………………………………..

(i)Anode:

…………………………………………………………………………

(ii)Cathode:

………………………………………………………………………

24.(a)(i) State what is meant by the rate of reaction.

(ii) With the aid of a well labeled diagram, describe an experiment that can be carried out to determine the rate of production of carbon dioxide gas from calcium carbonate and hydrochloric acid.

(b)The table below shows the variation in mass of calcium carbonate with time

when reacted with dilute hydrochloric acid.

Mass of Ca CO₃(g)	84	64	49	27	11	92	08
Time Min.	0	1	2	4	7	8	9

(i) Sketch a graph to show how the mass of calicium carbonate varies with time.

Graph paper

(i) The rate of reaction at 3 minutes.

(ii) The time taken for the calcium carbonate to react.

(d) State at least two ways in which the rate of production of carbon dioxide can be increased.

25.(a) Name the raw materials which are used in the extraction of iron using a blast furnace.

(b) Briefly describe the reactions that lead to the formation of iron during the extraction using a blast furnace (Youth answer should include equations for the reactions).

(c) State what would be observed write the equation for the reaction that would take place when the following gases are passed over heated iron:

(i)Dry Chlorine:

(ii)Steam:

(d)Dilute hydrochloric Acid was added to iron fillings and the mixture warned. Write the equation for the reaction that took place.

26.Outline how copper is refined by electrolysis

27.a)Define an alloy

b) State some common alloys and give their composition

28.Describe how sugar is manufactured in an industry

29(a) What is a standard solution?

(b) 20.10cm³ of a solution BA1 containing 6.8g1^-1 of an impure sample of oxalic acid was completely neutralized by 19.90cm³ of 0.01M potassium hydroxide solution.

Calculate the percentage of oxalic acid in the impure sample (H₂C₂O₄ =90).

30. A compound Q of formula mass 60, contains carbon, 40%, hydrogen 6.7% and the rest being oxygen.

(a)(i) Calculate the empirical formula of Q.

(iii)Determine the molecular formula of Q.

(b)Q dissolves in aqueous sodium hydrogen carbonate with effervescence.

(i)Suggest the chemical nature of Q.

………………………………………………………………………………………………

(ii)Write an ionic equation for the reaction between Q and aqueous sodium hydrogen carbonate.

…………………………………………………………………………………………….

31.a)State three industrial and domestic uses of water

b)State three causes of water pollution

c)Define

(i)Hard water

(ii)Soft Water

d)Outline the methods of removing water hardness

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