Chemistry, 1999, JAMB Exam, Exam, Paper 1 | Objectives

Paper Info

Year :

1999

Title :

Chemistry

Exam :

JAMB Exam

Paper 1 | Objectives

21 - 30 of 49 Questions

#	Question	Ans
21.	2SO_2(g) + O_2(g) ↔ 2SO_3(g). In the chemical reaction above, the substance that will increase the rate of production of sulphur (VI) oxide is A. manganese (IV) oxide B. finely divided iron C. vanadium (V) oxide D. nickel	C
22.	N₂O_4(g) ↔ 2NO_2(g). Increase in total pressure of the equilibrium reaction above will A. produce more of NO_2(g) in the mixture B. convert all of N₂O_4(g) to NO_2(g) C. have no effect on the concentrations of NO_2(g)and N₂O_4(g) D. produce more of N₂O_4(g) in the mixture	D
23.	What quantity of electricity will liberate 0.125 mole of oxygen molecules during the electrolysis of dilute sodium chloride solution? [ F = 96 5000 C mol^-1 ] A. 24 125 coulombs B. 48 250 coulombs C. 72 375 coulombs D. 96 500 coulombs Show Content Detailed Solution 4 Faradays of electricity is required to liberate one mole of oxygen gas ∴ quantity of electricity required = 0.125 * 4 * 96500 = 48250 coulombs	B
24.	X + Y → Z. The rate equation for the chemical reaction above is \(\frac{-Δx}{Δt}\) = K[X]\(^2\)[Y]. The overall order of the reaction is? A. 0.0 B. 1.0 C. 2.0 D. 3.09	D
25.	When a current I was passed through an electrolyte solution for 40 minutes, a mass X g of a univalent metal was deposited at the cathode. What mass of the metal will be deposited when a current 2I is passed through the solution for 10 minutes? A. X/4 g B. X/2 g C. 2X g D. 4X g Show Content Detailed Solution From M = zit Where M = to the mass of the metal liberated z = Is the electrochemical equivalent ∴ X g = 1 * 1 * 40 * 60 X g = 2400 I Let Y represent the new mass Y = 12I 10 * 60 Y = 1200 I Y/(X g) = 1200 I/2400 I Y = X/2 g	B
26.	RS_(aq) + HF_(aq) → RF_(s) + HS_(aq) ΔH = -65.7 kj mol^(-1). From the equation above, it can be deduced that A. the heat content of the reactants is lower than that of the products B. the heat content of the reactants is higher than that of the products C. the reaction is slow D. a large amount of heat is absorbed	B
27.	Which of the following statement is true of the electrochemical series? A. Electropositivity of metals increase down the series B. Electropositivity of non-metals decrease down the series C. Electronegativity of non-metals decrease down the series D. Electropositivity of metals decreases down the series	D
28.	The gas that will form a white precipitate with acidified silver trioxonitrate (v) is A. NH₃ B. SO₂ C. CO₂ D. HCL	D
29.	Chlorine, bromine and iodine resemble one another in that they A. dissolve in alkalis B. react violently with hydorgen without heating C. are liquids D. displace one another from solutiions of their salts	D
30.	The salt that reacts with dilute hydrochloric acid to produce a pungent smelling gas which decolourizes acidified purple potassium tetraoxomanganate (VII) solution is A. Na₂SO₄ B. Na₂SO₃ C. Na₂S D. Na₂CO₃	B

21.	2SO_2(g) + O_2(g) ↔ 2SO_3(g). In the chemical reaction above, the substance that will increase the rate of production of sulphur (VI) oxide is A. manganese (IV) oxide B. finely divided iron C. vanadium (V) oxide D. nickel	C
22.	N₂O_4(g) ↔ 2NO_2(g). Increase in total pressure of the equilibrium reaction above will A. produce more of NO_2(g) in the mixture B. convert all of N₂O_4(g) to NO_2(g) C. have no effect on the concentrations of NO_2(g)and N₂O_4(g) D. produce more of N₂O_4(g) in the mixture	D
23.	What quantity of electricity will liberate 0.125 mole of oxygen molecules during the electrolysis of dilute sodium chloride solution? [ F = 96 5000 C mol^-1 ] A. 24 125 coulombs B. 48 250 coulombs C. 72 375 coulombs D. 96 500 coulombs Show Content Detailed Solution 4 Faradays of electricity is required to liberate one mole of oxygen gas ∴ quantity of electricity required = 0.125 * 4 * 96500 = 48250 coulombs	B
24.	X + Y → Z. The rate equation for the chemical reaction above is \(\frac{-Δx}{Δt}\) = K[X]\(^2\)[Y]. The overall order of the reaction is? A. 0.0 B. 1.0 C. 2.0 D. 3.09	D
25.	When a current I was passed through an electrolyte solution for 40 minutes, a mass X g of a univalent metal was deposited at the cathode. What mass of the metal will be deposited when a current 2I is passed through the solution for 10 minutes? A. X/4 g B. X/2 g C. 2X g D. 4X g Show Content Detailed Solution From M = zit Where M = to the mass of the metal liberated z = Is the electrochemical equivalent ∴ X g = 1 * 1 * 40 * 60 X g = 2400 I Let Y represent the new mass Y = 12I 10 * 60 Y = 1200 I Y/(X g) = 1200 I/2400 I Y = X/2 g	B

26.	RS_(aq) + HF_(aq) → RF_(s) + HS_(aq) ΔH = -65.7 kj mol^(-1). From the equation above, it can be deduced that A. the heat content of the reactants is lower than that of the products B. the heat content of the reactants is higher than that of the products C. the reaction is slow D. a large amount of heat is absorbed	B
27.	Which of the following statement is true of the electrochemical series? A. Electropositivity of metals increase down the series B. Electropositivity of non-metals decrease down the series C. Electronegativity of non-metals decrease down the series D. Electropositivity of metals decreases down the series	D
28.	The gas that will form a white precipitate with acidified silver trioxonitrate (v) is A. NH₃ B. SO₂ C. CO₂ D. HCL	D
29.	Chlorine, bromine and iodine resemble one another in that they A. dissolve in alkalis B. react violently with hydorgen without heating C. are liquids D. displace one another from solutiions of their salts	D
30.	The salt that reacts with dilute hydrochloric acid to produce a pungent smelling gas which decolourizes acidified purple potassium tetraoxomanganate (VII) solution is A. Na₂SO₄ B. Na₂SO₃ C. Na₂S D. Na₂CO₃	B