​These are chemistry questions and answers categorized according to topics, papers i.e. Paper 1 and 2, Levels i.e. form 1 to form 4, kcse year the examination was done and section A or B
Select topic/category to open topical questions from that particular option provided.

 (a) Name two ores of iron. 
(b) Describe how the amount of iron in a sample of iron(III) oxide can be determined. 

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.

(a) Name two ores in which sodium occurs. 
(b) During extraction of sodium using the down's process, calcium chloride is added to the ore.
Give a reason for the addition of calcium chloride. 
(c) State two uses of sodium.

The diagram below represents a set up of an electrolytic cell that can be used in the production of aluminium.

​(a) On the diagram, label the anode.
(b)Write the equation for the reaction at the anode.
(c) Give a reason why the electrolytic process is not carried out below 950°C.
(d)Give a reason why the production of aluminium is not carried out using reduction process
(e)Give two reasons why only the aluminium ions are discharged
(f)State two properties of duralumin that makes it suitable for use in aircraft industry.
(g)Name two environmental effects caused by extraction of aluminium.

​(a) Zinc occurs mainly as zinc blende. Name one other ore from which Zinc can be extracted. (1 mark)
(b) The flow chart in Figure 2 shows the various stages in the extraction of zinc metal. Study it and answer the questions that follow.

• (i) Write an equation for the reaction which occurs in the roasting chamber. (1 mark)
• (ii) Describe the process that takes place in the blast furnace. (3 marks)
• (iii) Explain why molten lead is added to the condenser. (1 mark)
• (iv) State two uses of zinc. (1 mark)
• (v) Give one reason why the extraction of zinc causes pollution to the environment. (1 mark)

​(c) Explain the observations made when zinc metal is added to hot sodium hydroxide. (2 marks)

Sodium hydroxide can be prepared by the following methods; I and II

​(a) Name one precaution that needs to be taken in method I. 
(b) Give the name of process A. 
(c) Give one use of sodium hydroxide.

Aluminium is both malleable and ductile.
(a)What is meant by?
(i) Malleable:
(ii)Ductile
(b)State One use of aluminium based on:
(i)malleability
(ii)ductility

The flow chart below shows various reactions of aluminium metal. Study it and answer the questions that follow

a) i) Other than water, name another reagent that could be R 
 ii) Write the formula of reagent Q 
 b) Write an equation or the reaction in step 5. 

​(a) Name the raw material from which sodium is extracted. 
(b) Give a reason why sodium is extracted using electrolysis. 
(c) Give two uses of sodium metal.

The diagram below represents a set up of an electrolytic cell that can be used in the production of aluminium

​(a) One the diagram, label the anode 
(b) Write the equation for the reaction at the anode 
(c) Give a reason why the electrolytic process is not carried out below 950°C 
(d) Give a reason why the production of aluminium is not carried out using reduction process
(e) Give two reasons why only the aluminium ions are discharged
(f) State two properties of duralumin that makes it suitable for use in aircraft industry 
(g)Name two environmental effects caused by extraction of aluminium

​The flow chart in Figure 1 represents some stages in the extraction of copper metal. Study it and answer the questions that follow.

​Identify:

• (i) the copper ore ………………………. (1 mark)
• (ii) process B ................................. (1/2 mark)
• (iii) solid C  ....................................(1/2 mark)
  ​Write an equation for the reaction that forms the slag. (1 mark)

a) Name two ores from which copper is extracted 
b) During extraction of copper metal, the ore is subjected to froth flotation.
Give a reason why this process is necessary. 
c) Name one alloy of copper and state its use.