JAMB UTME - Chemistry - 1979
Question 2 Report
In the extraction of aluminum from purified bauxite by electrolysis, cryolite is used because
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Question 3 Report
0.1 Faraday of electricity was passed through a solution of copper (ll) sulphate. The maximum weight of copper deposited on the cathode would be [Cu = 64]
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Question 4 Report
\(50cm^{3}\) of hydrogen are sparked with \(20cm^{3}\) of oxygen at \(100°C\) and \(1atm\) . The total volume of the residual gases in
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Question 5 Report
When a piece of charcoal enclosed in a cylinder containing air is ignited
Question 6 Report
Calcium hydroxide and ammonium chloride when heated together will give an important product. This compound may be obtained dry by
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Question 7 Report
Which are the correct IUPAC names for H-CO2CH3 and CH = CH
Question 9 Report
The solution of a sample in a tube will be identified as a chloride if it gives
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The solution of a sample in a tube will be identified as a chloride if it gives a white precipitate when acidified with dilute HNO3 and then AgNO3 solution is added. This is because the test is a confirmatory test for chloride ions, and the white precipitate formed is silver chloride (AgCl). Chloride ions react with silver nitrate (AgNO3) to form a white precipitate of AgCl, which is insoluble in water and dilute nitric acid.
Question 10 Report
Indicate which of the following statements is not true as we move from left to right along the periodic Table:
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Question 11 Report
The reaction between hydrogen and iodine may be represented by the equation H2(g)+ I2(g) → 2HI(g), and is exothermic. Therefore
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Question 12 Report
If chlorine gas is bubbled into water and then this yellowish-green coloured solution is exposed to bright sunlight for a while
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Question 13 Report
Which of the following raw materials would be required from the smelting of iron ore in a blast furnace?
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Question 14 Report
Which of the following statements applies during the electroysis of sodium hydroxide sodium hydroxide solution using platinum electrodes?
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Question 16 Report
On heating anhydrous iron (ll) sulphate, in addition to producing iron (iii) oxide, which of the following is produced?
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Question 17 Report
Phosphorus burns in oxygen according to the equation P4 + 502 → P4O10. How many litres of oxygen will be required at S.T.P for complete oxidation of 12.4g of phosphorus? [P = 31,O = 16 and molar volume of a gas at S.T.P = 22.4 litres]
Question 18 Report
In which of the following reactions is sulphur dioxide acting as an oxidizing agent?
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Question 20 Report
When ammonium, potassium and calcium carbonates are each separately heated
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Question 21 Report
A gas occupies 30.0 dm3 at S.T.P. What volume would it occupy at 91oC and 380 mm Hg?
Question 22 Report
In the manufacture of iron in the blast furnace, iron (lll) oxide is mixed with coke and limestone, and different reactions occur in the process. Which of the following statements is true with respect to these reactions?
Question 23 Report
Methanoic acid mixes with water in all proportions and has about the same boiling point as water which of the following methods would you adopt to obtain pure water from a mixture of stand, water and methanoic acid?
Question 26 Report
the vapour density of a gas may be defined as
Question 28 Report
When excess ethanol is heated to 145 oC in the presence of concentrated sulphuric acid, the product is
Question 29 Report
The IUPAC name for
Question 31 Report
How many grams of HBr would exactly be required to react with 2 g of propyne? (C =12, H=1, Br = 80)
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Question 32 Report
Which one of these compounds will NOT give an oxygen gas on heating?
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Question 33 Report
Consider the following exothermic reaction 2SO2(g) + O2(g) = 2SO3 (g) . If the temperature of the reaction is reduced from 800oC to 500oC, and no other change takes place, then
Question 34 Report
The reaction of zinc with copper (ll) ions in aqueous solution can be represented as follows: Cu 2+(aq) +Zn (s) → Cu(s) + Zn 2+(aq).Which of the following is the most complete description of this reaction?
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Question 35 Report
A piece of metal (M) is dissolved in nitric acid and the resulting solution is treated with a small quantity of sodium hydroxide to produce a white precipitate (B) which redissolves on the addition of excess alkali. The precipitate (B)when ignited in a crucible produces the oxide of the metal(m). The METAL M is
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Question 36 Report
An organic compound X has the following properties: I. It is not miscible with water. ll. lt has boiling point of 77oC lll. lt has a sweet odour lV. lt is insoluble in sodium hydrogen carbonate solution . V lt does not decolourize bromine water X is therefore
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Question 37 Report
Weighed salts Y and Z were left exposed in the laboratory overnight. In the morning Y had gained weight, and Z had become liquid. What conclusion could be drawn about the nature of the two salts?
Question 39 Report
Which of the following statements is true?
Question 40 Report
Hydrogenation may be effected by
Question 41 Report
Which of the following substances are all made by the process of polymerization?
Question 42 Report
In the electrolysis of dilute sulphuric acid using platinum electrodes, the products obtained at the anode and cathode are:
Anode Cathode
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Question 43 Report
Which of the following statements is true? When the potassium atom forms its ion
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Question 45 Report
12 g of solid protassium chlorate (KCIO) were added to 40 g of water and heated to dissolve all the solid. As the solution cools, crystals of potassium chlorate at 66 oC. The solubility of potassium chlorate at 66 oC is therefore
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Question 46 Report
One of the following techniques can be used to show that chlorophyll pigment is a mixture of chemical compounds and not a single coloured compound
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Question 47 Report
The empirical formula of an oxide of nitrogen containing 30.4 per cent of nitrogen is (N=14.0,O=16.0)
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Question 48 Report
When carbondioxide is bubbled into limewater a white precipitate is formed. If the passage of the gas is continued, the precipitate disappears. The reason for this is
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Question 49 Report
The reaction 3C(s) + 2Fe2O3(s) = 4Fe(s) + 3CO2(g): \(\Delta\)H =46.0 kJ is
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