INSTRUCTIONS
- Answer all the questions in the spaces provided after each.
- Mathematical tables and silent electronic calculators may be used.
- All working must be clearly shown where necessary.
- All answers should be written in English.
QUESTIONS
- Metal Q displaces metals T and U from their oxides but does not displaces metal R. Metal T displaces U form its oxide. Arrange the metals according to their reactivity starting with the strongest reducing agent. (1 mark)
- Chlorine gas can be prepared in the laboratory using the following two methods;
Solid substance X and concentrated Hydrochloric acid
Solid substance X, concentrated sulphuric (VI) acid and solid Sodium Chloride.- Name the solid substance X (1 mark)
- What is role of concentrated sulphuric acid in the reaction? (1 mark)
- State how dry chlorine gas is collected. (1 mark)
- A white crystalline solid Q when heated to forms a brown gas, colourless gas that relights a glowing wooden splint and a yellow residue which turns white on cooling. Aqueous solution of Q forms reacts with excess aqueous ammonia solution to form a colourless solution P.
- Write the name and chemical formulae of complex ion in solution P. (2 marks)
Name;
Chemical formula; - State the observation made when the aqueous solution of P is reacted with few drops of sodium hydroxide. (1 mark)
- Write the name and chemical formulae of complex ion in solution P. (2 marks)
-
- Define an acid in terms of hydrogen ions. (1 mark)
- Study the reaction below and answer the questions that follow.
H3O+ (aq) +HSO4- (aq) H2O (l) + H2SO4 (aq)
Identify the acid and base in the forward reaction. Explain. (2 marks)
- Ammonia gas is one of the substances recycled in the Solvay process.
- Other than water name another substance that is recycled in the process. (1 marks)
- Write a balanced chemical equation for the reaction that regenerates Ammonia gas in the process. (1 mark)
- State an industrial use of the only waste product in the Solvay process. (1 mark)
- Lead (II) iodide is a toxic bright yellow solid which was used as a paint pigment known as ‘iodine
yellow’. Describe briefly how you would prepare lead (II) iodide in the laboratory starting with lead (II) oxide. (3 marks) - 5.0g of zinc carbonate were allowed to react with 25cm3 of 1M hydrochloric acid until there was no further reaction. Calculate the volume of gas that was formed at s.t.p. (Zn = 65.4, O = 16, C = 12, molar gas volume at s.t.p = 22400 cm3) (3 marks)
- Atoms of element P can be represented as 11P. Element P reacts with sulphur to form a yellow solid. 23
Using dots (•) and crosses (X) to represent electrons, draw the structure of the yellow solid. (S=16).
(2 marks) - The set up below was used by a student to carry out the electrolysis of aqueous copper (II) sulphate using copper electrodes.
- On the diagram, label the anode and cathode. (1 mark)
- Write the half ionic equation for the reaction that undergoes oxidation. (1 mark)
- Explain the observation made on the electrolyte when the copper electrodes are replaced with graphite electrodes. (1 mark)
- A fuel gas contains 50% of hydrogen gas and 44% of carbon (II) oxide by volume. The rest of is
incombustible. Calculate the volume of gas that remains at room temperature when the 100 cm3 fuel gas was ignited. (3 marks) - Study the diagram below and answer the questions that follow.
- Name substances; ( 1 mark)
Q
R - Write the equation for the reaction that leads to the formation of the yellow solid. (1 mark)
- Using a chemical test, describe how you would distinguish between hydrogen sulphide and sulphur (IV) oxide. (1 mark)
- Name substances; ( 1 mark)
- State two differences between luminous and non luminous flame of the Bunsen burner. (2 marks)
- A gas occupies a volume of 400cm3 at 227oC and 760mmHg.What will be the temperature of the gas when the volume and pressure of the gas is 100cm3 and 380mmHg respectively. (2 marks)
- For each of the following experiments, give the observations, and the type of change that
occurs (Physical or chemical) (3 marks)
Experiment
Observation
Type of change
A few drops of concentrated sulphuric acid added to small amounts of sugar
A few crystals of Iodine are heated gently in a test tube
A few crystals of copper (II) Nitrate are heated strongly in a test tube.
-
- Define solubility of a solute. (1 mark)
- The solubility of potassium nitrate is 120g/100g of water at 80 oC and 70g/100g of water at
20oC.What mass of the salt would crystallize if 80g of potassium nitrate solution saturated at 80oC was cooled to 20 oC? (2 marks)
- Zinc metal reacted with dilute hydrochloric acid. The gas produced was then passed over heated copper (II) oxide in a combustion tube.
- State two precautions that must be considered when the gas reacts with copper (II) Oxide in the combustion tube. (2 marks)
- Write a balanced chemical equation between zinc and dilute hydrochloric acid. (1 mark)
- The table below shows ammeter readings recorded when two equimolar solutions were tested separately.
Electrolyte
Current (A)
Dilute Sulphuric (VI) Acid
7.210
Ethanoic Acid
4.011
- Explain the difference in the ammeter readings. (2marks)
- Compare the reactivity of equal length of magnesium ribbon with each of the electrolytes. (1 mark)
- The set up below was used to show the solubility of ammonia gas in water.
- State and explain the observations made in the flask. (2 marks)
- Write a balanced equation to show how ammonia gas reacts with water. (1 mark)
- Magnesium ribbon was added to a solution of hydrogen chloride in methylbenzene. Another piece of Magnesium ribbon was added to distilled water. State and explain observations made. (2 marks)
- One of the disadvantages of hard water is wastage of soap.
- Write the chemical formula of a salt that causes permanent water hardness. (1 mark)
- Given the chemical formula of soap as RCOONa. Write a balanced equation show how soap reacts with the salt stated in (a) above. (1 mark)
- State two advantages of water hardness. (1 mark)
- A piece of sodium was burnt in excess oxygen gas. The product obtained was shaken with water to make a solution.
- Write a balanced equation for reaction between the product formed and water. (1 mark)
- State and explain the observation made when red and blue litmus papers are dipped into the solution.(2 marks)
- Aluminium chloride and sodium chloride are both chlorides of period 3 elements in the periodic table. Use this information to explain the following observations.
- A solution of Al2Cl6 in water turns blue litmus paper red while that of sodium Chloride does not. (1½ marks)
- Sodium chloride has a melting point 801oC is while Al2Cl6 sublimes 183oC. (1½ marks)
- The ionization energies of elements A and B are 495.9kJ/mol and 739.9kJ/ mol respectively. Both elements are in the same group of the periodic table.
- What is ionization energy? (1 mark)
- Compare the reactivity of elements A and B . Explain your answer. (2 marks)
- Study the information given in the table below and answer the questions below.
Bond
Bond energy(kJ/mol)
C-H
H-Cl
C-Cl
Cl-Cl
C - C
413
431
346
244
347
- Calculate the enthalpy change for the reaction below.
C2H6 (g) + Cl2 (g) → CH3CH2Cl (g) + HCl (g) (2 marks) - State a condition required for the reaction in (a) above to take place. (1 mark)
- Calculate the enthalpy change for the reaction below.
- Study the organic compound below:
- In which homologous series does the compund belong to?
- Name and draw the structures of two compounds that can be used to prepare the above compound. (3 marks)
- The diagram below represents a set-up that can be used to obtain nitrogen gas in the laboratory. Use the information on the diagram to answer the questions that follow
- Describe the chemical test for liquid A. (1 mark)
- What observation is made in the combustion tube during the reaction? (1 mark)
- State two uses of gas B. (1 mark)
- Analysis of an organic acid isolated from red ants shows that it contains 0.06 g of carbon, 0.01g of hydrogen and 0.16 g of oxygen.(H=1,O=16, C=12)
- Calculate the empirical formula for this acid. (1½ marks)
- What is the basicity of the acid if the empirical formula of the acid is the same as its molecular formula.
- Nitrogen (IV) oxide dissolves and reacts with Sodium hydroxide solution to form two salts and water.
- What is the nature of Nitrogen (IV) oxide? {1 mark}
- Write the Ionic equation for the reaction that takes place. {1 mark}
- When powdered brass was reacted with excess dilute sulphuric (VI) acid, a solid residue was left. (i)
- Name the residue. (1 mark)
- Explain why the residue was left. (1 mark)
- State another observation made (1 mark)
Download Chemistry Paper 1 Questions - Kapsabet Boys Post Mock 2023 Exams.
Tap Here to Download for 50/-
Get on WhatsApp for 50/-
Why download?
- ✔ To read offline at any time.
- ✔ To Print at your convenience
- ✔ Share Easily with Friends / Students