The diagram below shows the set up used in an experiment to prepare chlorine gas and react it with aluminium foil. Study it and answer the question that follow

​(a) In the experiment, concentrated hydrochloric acid and potassium manganate (VII) were used to prepare chlorine gas. State two precautions that should be taken in carrying out this experiment. 
(b) Write the formula of another compound that could be used instead of potassium manganate (VII) 
(c) Explain why it is necessary to allow the acid to drip slowly onto potassium manganate (VII) before the aluminium foil is heated. 
(d) State the property of the product formed in the combustion tube that makes it possible for it to be collected in the receiver 
(e) When 1.08g of aluminum foil were heated in a stream of chlorine gas, the mass of the product formed was 3.47 g
Calculate the:
(i) Maximum mass of the product formed if chlorine was in excess; (Al= 27; Cl = 35.5)
(ii) Percentage yield of the product formed 
(f) Phosphorous trichloride is a liquid at room temperature. What modification should be made to set up if it is to be used to prepare phosphorous trichloride?

(i) On the grid provided, draw the solubility curve of ammonium phosphate (Temperature on x – axis) 
(ii) Using the graph, determine the solubility of ammonium phosphate at 25°C 
(iii) 100g of a saturated solution of ammonium phosphate was prepared at 25°C
I what is meant by a saturated solution? 
II Calculate the mass of ammonium phosphate which was used to prepare the saturated solution 
(c) The graph below shows how the PH value of soil in a farm changed over a period of time

​(i) Describe how the pH of the soil can be determined 
(ii) State one factor that may have been responsible for the change in the soil pH in the time interval AB

(a) The diagram below represents part of the structure of a sodium chloride crystal.
The position of one of the sodium ions in the crystal is shown as 
(i) On the diagram, mark the position of the other three sodium ions 
(ii) The melting and boiling points of sodium chloride are 801°C and 1413°C respectively.
Explain why sodium chloride does not conduct electricity at 25°C, but does so at temperatures between 801° C and 1413°C 
(b) Give a reason why ammonia gas is highly soluble in water 
(c) The structure of an ammonia ion is shown below:

​Name the type of bond represented in the diagram by N → H 
(d) Carbon exists in different crystalline forms. Some of these forms were recently discovered in soot and are called fullerenes
(i) What name is given to different crystalline forms of the same element?
(ii) Fullerenes dissolve in methylbenzene while the other forms of carbon do not.
Given that soot is a mixture of fullerenes and other solid forms of carbon, describe how crystals of fullerenes can be obtained from soot. 
(iii) The relative molecular mass of one of the fullerenes is 720. What is the molecular formula of this fullerene? (C=12.0)

​(a) Methanol is manufactured from carbon (IV) oxide and hydrogen gas according to the equation:

The flow chart below shows a sequence of chemical reactions starting with copper study it and answer the questions that follow.

​(a) In step 1, excess 3M nitric acid was added to 0.5g of copper powder
(i) State two observations which were made when the reactions was in progress 
(ii) Explain why dilute hydrochloric acid cannot be used in step 1 
(iii) I Write the equation for the reaction that took place in step 1 
II Calculate the volume of 3M nitric that was needed to react completely with 0.5g of copper powder. (Cu = 63.5) 
(b) Give the names of the types of reactions that took place in steps 4 and 5 
Step 4
Step 5
(c) Apart from the good conductivity of electricity, state two other properties that make it possible for copper to be extensively used in the electrical industry.

(a) Give the systematic names of the following compounds

(b) State the observations made when Propan – 1- ol reacts with:
(i) Acidified potassium dichromate (VI) Solution 
(ii) Sodium metal 
(c) Ethanol obtained from glucose can be converted to ethane as shown below

(a) State two factors that should be considered when choosing fuel for cooking 
(b) The diagram below represents a set – up that was used to determine the molar heat of combustion of ethanol

During the experiment, the data given below was recorded

Below is a sketch of a graph showing the change in viscosity? (Ease of flow) with temperature when solid sulphur is heated.

​Describe what happens to the sulphur molecules when sulphur is heated from 150°C to about 200°C.

The diagram below is a section of a model of the structure of element T.

a) State the type of bonding that exists in T. 
b) In which group of the period table does element T belong? Give a reason.

During the electrolysis of aqueous silver nitrate, a current of 5.0a was passed through the electrolysis for 3 hours.
a) Write the equation for reaction which took place at the anode. 
b) Calculate the mass of silver deposited (Ag = 108; IF=96500C)

The diagram below formula for the most stable ion of Q.

​On the same axis, sketch the graph for the decomposition of hydrogen peroxide when manganese (IV) oxide is added.

The table below shows the number of valence electrons of the element P, Q and R.

​a) Explain why p and R would not be expected to form a compound.
b) Write an equation to show the effect of heat on the carbonate of R 
c) Write the formula for the most stable ion or Q.

The diagram below shows a student's set-up for the preparation and collection of hydrogen gas.

​(a) How would the final volume of hydrogen gas produced be affected if 80cm3 of 0,75M hydrochloric acid was used? 
(b) Give a reason why helium is increasingly being preferred to hydrogen in weather balloons.

State and explain the observations made when excess ammonia gas reacts with chlorine gas

The table below shows the relative molecular masses and the boiling points of pentane and propan-1-ol

Explain why the boiling point of propane-1-ol is higher than that of pentane.