- Explain the following:
- It is always advisable to scoop chemical substances using a clean spatula. ( ½ mark)
To prevent contamination of the chemicals.
- Flammable substances should always be kept away from flames in the laboratory. ( ½ mark)
To prevent fire accidents.
- It is always advisable to scoop chemical substances using a clean spatula. ( ½ mark)
- Name one reagent that can be used to distinguish between Al3+ and Zn2+ ions in solution and state what would be observed if each of the ions is treated with the reagent you have named. (3 marks)
Ammonia solution
Al3+ - A white precipitate would be formed which is insoluble in excess ammonia solution.
Zn2+ - A white precipitate would be formed which is insoluble in excess ammonia solution.
- Manganese sulphide reacts with acids according to the following equation.
State, giving a reason what would happen to the equilibrium if;- Water is added to the equilibrium mixture. (1 ½ marks)
Increasing the concentration of water would shift the equilibrium to the left.
- Hydrogen chloride is bubbled into the equilibrium mixture. (1 ½ marks)
HCl would react with the H2S thereby reducing its concentration. The equilibrium would shift to the right.
- Water is added to the equilibrium mixture. (1 ½ marks)
- Use the thermochemical equations below to answer the questions that follow.
- Draw an energy cycle diagram to show the enthalpy of formation of ethane. (1 ½ marks)
- Calculate the enthalpy of formation of ethane. (1 ½ marks)
ΔHf = ΔH1 + ΔH2 - ΔH3
= (2 x - 394) + (3 x -286) - 1560
= -788 + -856 - -1560
= -1646 + 1560
= -86 kJ/mole
- State the conditions under which copper reacts with sulphuric acid and give an equation for the reaction. (2 marks)
The acid must be concentrated and hot
Cu(s) + H2SO4(l) --------> CuSO4(aq) + SO2(g) + H2O(l) - When 8.8g of hydrocarbon Z was burnt in excess air, 14.4g of water and 11.95 dm3 of carbon (IV) oxide were obtained at s.t.p. Determine the empirical formula of Z. (3 marks)
- Perspex is a synthetic polymer of formula
- Write the structural formula of the monomer of Perspex. (1 mark)
- State the type of polymerization involved in the formation of perspex. (1 mark)
Addition polymerization
- Write the structural formula of the monomer of Perspex. (1 mark)
- When zinc granules are dropped into two separate solutions of dilute sulphuric (VI) and concentrated sulphuric (VI) acid, effervescence of a colourless gas occurs in each case. Give equations to represent the reactions that take place. (2 marks)
Zn(s) + H2SO4(aq) ---------> ZnSO4(aq) + H2(g)
Zn(s) + 2H2SO4(l) ---------> ZnSO4(aq) + SO2(g) + 2H2O(l) - Study the chart below and answer the questions that follow.
- Identity solid X. (1 mark)
Hydrated iron (III) oxide
- Write an ionic equation for the reaction between P and copper (II) sulphide solution. (1 mark)
H2S(g) + Cu2+(aq) ---------------> CuS(s) + 2H+(aq)
- State the observation made when gas P is bubbled through iron (III) chloride solution. (1 mark)
The yellow iron (III) chloride solution turns green.
- Identity solid X. (1 mark)
- Use the nuclear equations below to answer the questions that follow.
- Give the actual names of particles X and Y. (1 mark)
X - Alpha particles
Y Beta particles
- Give the name of a radiation whose emission does not change the mass number or the atomic number of a radioisotope. (1 mark)
Gamma radiatons
- Give the actual names of particles X and Y. (1 mark)
- The structures below represent two cleaning agents M and P.
Which cleaning agent would be most suitable for use with water containing calcium sulphate. Give a reason. (2 marks)P – when used with hard water it does not form scum.
- You are given the following half equations:
- Obtain an equation of the cell reaction. (1 mark)
Mg(s) + Zn2+(aq) ------------> Mg2+(aq) + Zn(s)
- Calculate the value Eϑ for the cell. (1 mark)
E.m.f = Eϑ reduced - Eϑ oxidised
= -0.76 + 2.37
= +1.61V - Give the oxidizing species. (1 mark)
Zn2+ ion
- Obtain an equation of the cell reaction. (1 mark)
- Using dots (.) and crosses (×) to represent outermost electrons; draw diagrams to show bonding in:
- Aluminium chloride. (1 ½ marks)
- Sulphuric (IV) oxide. (1 ½ marks)
- Use the information in the table below to answer the questions that follow.
Melting point Element Atomic number 97.8 R 11 660 S 13 1440 T 14 -40.1 U 17 63.1 V 19 - Write the electron arrangement of: (1 mark)
- ion of S
2.8
- atom of T
2.8.4
- ion of S
- Explain why the melting point of T is higher than that of U. (2 marks)
Atoms are covalently bonded together to form a giant atomic structure. Atoms of U are bonded covalently to form molecules. The molecules are then hold together by weak Van der waals to form a simple molecule structure.
- Write the electron arrangement of: (1 mark)
- Complete the table below. (3 marks)
Metal Aluminium Lead Sodium Chief Ore Bauxite Galena
Rock salt Chemical name Al2O3.2H2O
PbS
NaCl
Method of extraction Electrolysis
reduction Electrolysis
- The diagram below represents a set up used for the large scale manufacture of hydrochloric acid.
- Name substance X. (1 mark)
Hydrogen
- What is the purpose of the glass beads? (1 mark)
They increase the surface area over which the gas dissolves in water.
- Give one use of hydrochloric acid. (1 mark)
-Treatment of water at the water works
-Sewage treatment
-Manufacture of dyes, drugs etc
-To clean metal surfaces to remove rust
- Name substance X. (1 mark)
- Calculate the volume of nitrogen (I) oxide produced when 38.2g of ammonium nitrate is completely decomposed by heating (at s.t.p). (N = 14, H = 1, O = 16) (3 marks)
- Give equations to show the reactions that take place when;
- iron reacts with steam. (1 mark)
3Fe(s) + 4H2O(g) ---------> Fe3O4(s) + 4H2(g)
- Give one industrial use of the gas produced in the reactions in (i) and (ii) above. (1 mark)
-Industrial manufacture of hydrochloric acid
-Industrial manufacture of Ammonia
-Used in weather balloons
- iron reacts with steam. (1 mark)
- When magnesium metal is burnt in air, it reacts with both oxygen and nitrogen gases giving a white ash. Write two equations for the reactions that take place. (2 marks)
2Mg(s) + O2(g) -------> 2MgO(s)
3Mg(s) + N2(g) --------> Mg3N2(s) - Give the total number of atoms present in the gas produced when water is added to magnesium nitrate. (1 mark)
Four
- When magnesium metal is burnt in air, it reacts with both oxygen and nitrogen gases giving a white ash. Write two equations for the reactions that take place. (2 marks)
- The graph below shows the behavior of a fixed mass of a gas at constant temperature.
- What is the relationship between the volume and the pressure of the gas? (1 mark)
At constant temperature, the volume of a fixed mass of gas is inversely proportional to pressure or V α 1/p , V = K/P
- 60 cm3 of oxygen gas diffused through a porous partition in 50 seconds. How long would it take 60 cm3 of sulphur (IV) oxide gas to diffuse through the same partition under the same conditions? (S = 32.), O = 16.0) (3 marks)
- What is the relationship between the volume and the pressure of the gas? (1 mark)
- State and explain the observation made when a moist red litmus paper is put in a gas jar of dry chlorine gas. (2 marks)
The red litmus paper is bleached. This is because chlorine gas has bleaching property.
- When extinguishing a fire caused by burning kerosene, carbon (IV) oxide is preferred to water. Explain. (2 marks)
Kerosene floats on water therefore it continues to burn. Carbon (IV) oxide cuts off the supply of oxygen.
- Write the formula of the oxide of carbon which is ‘silent killer’. (1 mark)
CO
- When extinguishing a fire caused by burning kerosene, carbon (IV) oxide is preferred to water. Explain. (2 marks)
- Explain why chlorine is a gas while iodine is a solid at room temperature. (2 marks)
The molecules of chlorine are smaller compared to those of iodine; thus the strength of the intermolecules forces of attraction in iodine are much stronger than in chlorine.
- Apart from their location, state any two differences between a proton and an electron. (2 marks)
A proton is positively charged whereas an electron is negatively charged.
The mass of a proton is/atomic mass units whereas that of an electron is 1/1840 a.m.u - What term is given to: The amount of energy given out when a neutral atom in gaseous state gains an electron? (1 mark)
Electron affinity
- A certain fertilizer is suspected to be containing nitrate ions. Describe how the presence of nitrate ions can be determined in such fertilizer. (3 marks)
Add water to a small sample of the fertilizer in a test tube and shake well. Filter to obtain a solution. To the solution add some freshly prepared ion (II) sulphate solution and shake well. With a test tube in a slanting position, add concentrated sulphuric (VI) acid to the mixture carefully along one side of the tube. A brown ring between two layers indicates the presence of nitrate ions.
- Write balanced chemical equations to show the action of heat on the following nitrates.
- Lead (II) nitrate (1 mark)
2Pb(NO3)2 (s) 2PbO(s) + 4NO2(s) + O2(g)
- Silver nitrate (1 mark)
2Ag NO3(s) ---------> 2Ag(s) +2NO2(g) + O2(g)
- Lead (II) nitrate (1 mark)
- What is an amphoteric oxide? (1 mark)
An oxide that behaves as an acid or a base in chemical reactions.
- Starting with zinc carbonate solid describe how zinc hydroxide can be prepared in the laboratory. (3 marks)
Heat the zinc carbonate solid in a test tube to obtain zinc oxide. To a certain volume of dilute nitric (V) acid the zinc oxide a little at a time while stirring till in excess. Filter the unreacted zinc oxise. To the filtrate add aqueous
- Below is a scheme of some reactions starting with but-z-yne. Study it and answer the questions that follow.
- Name Y, X and T (1 ½ marks)
Y Chlorine gas
X Hydrogen gas
T Butyl hydrogen sulphate
- Give the name of the following organic compounds. ( ½ mark)
Ethanoic acid
Ethylpropanoate
Sodium ethanoate
- Name Y, X and T (1 ½ marks)
- The following results were obtained during an experiment to determine the solubility of potassium nitrate in water at 30oC. Mass of dish = 15.86g, mass of dish + saturated
solution at 30oC = 26.86g, mass of dish + solid KNO3 after evaporation to dryness = 16.7g. Calculate the mass of saturated solution containing 60.0g of water at 30o C. (3 marks)
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