POST UTME REDEEMERS UNIVERSITY 2022 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
The following diagram represents a simple apparatus for measuring the rate of reaction. Identify the part labeled B.
A. B is the measuring cylinder
B. B is the thermometer
C. B is the reaction vessel
D. B is the stirrer
Question 2
A 2.50 M solution of sodium hydroxide (NaOH) is prepared by dissolving 50.0 g of NaOH in 1.00 L of water. What is the concentration of the solution in terms of molarity?
A. 1.00 M
B. 2.00 M
C. 2.50 M
D. 5.00 M
Question 3
A 1.0 M solution of a weak acid, HA, has a pH of 4.5. What is the concentration of the acid if the pH is decreased to 3.5 by the addition of 20 cm³ of 0.1 M NaOH?
A. 0.5 M
B. 0.75 M
C. 1.0 M
D. 1.25 M
Question 4
A sample of a gas at 300K and 1 atm occupies a volume of 2L. What is the new volume of the gas at 400K and 2 atm?
A. 1L
B. 2L
C. 4L
D. 8L
Question 5
A sample of 1.0 L of a gas at 2.0 atm and 25°C is allowed to expand to 2.0 L. What is the final pressure of the gas?
A. 1.0 atm
B. 1.5 atm
C. 2.0 atm
D. 2.5 atm
Question 6
The following equation represents a chemical reaction involving sulfur and oxygen gases. Write the balanced chemical equation for this reaction, including the state of each subs\tance.
A. S + O2 → SO2
B. S + O2 → SO3
C. S + O2 → SO4
D. S + O2 → SO5
Question 7
A 0.500 M solution of HCl is titrated with a 0.500 M solution of NaOH. If 25.0 mL of NaOH is required to reach the equivalence point, what is the volume of HCl required to reach the equivalence point?
A. 25.0 mL
B. 50.0 mL
C. 75.0 mL
D. 100 mL
Question 8
The following equation represents a chemical reaction involving nitrogen and oxygen gases. Write the balanced chemical equation for this reaction, including the state of each subs\tance.
A. N2 + O2 → 2NO
B. N2 + O2 → 2NO2
C. N2 + O2 → 2N2O
D. N2 + O2 → 2NO3
Question 9
Determine the number of unpaired electrons in the ground state of a neutral atom of the element with atomic number 13.
A. 4
B. 6
C. 8
D. 10
Question 10
A sample of a metal oxide has a mass of 25.0 g and a volume of 2.50 cm3. If the density of the metal oxide is 5.00 g/cm3, what is the molar mass of the metal oxide?
A. 100 g/mol
B. 150 g/mol
C. 200 g/mol
D. 250 g/mol
Question 11
The half-life of a radioactive subs\tance is 5 years. If 100g of the subs\tance initially exists, what is the mass of the subs\tance remaining after 10 years?
A. 25g
B. 50g
C. 75g
D. 100g
Question 12
A 2.50 g sample of a metal carbonate is heated to produce a metal oxide and carbon dioxide gas. If the mass of the metal oxide produced is 1.75 g, calculate the mass of carbon dioxide gas produced.
A. 1.25 g
B. 1.75 g
C. 2.00 g
D. 2.50 g
Question 13
The atomic number of an element is 12. What is the number of protons in the nucleus of an atom of this element?
A. 10
B. 12
C. 14
D. 16
Question 14
A 10.0 mL sample of a solution containing 0.1 M HCl is titrated with 0.1 M NaOH. What is the pH of the solution after the titration?
A. 7
B. 8
C. 9
D. 10
Question 15
The following diagram represents a simple electrolysis setup. Identify the part labeled A.
A. A is the cathode
B. A is the anode
C. A is the electrolyte
D. A is the power source

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