POST UTME JOSEPH AYO BABALOLA UNIVERSITY 2025 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
Determine the number of moles of carbon dioxide produced when 2.5 g of calcium carbonate is heated in a crucible.
A. 0.05 mol
B. 0.1 mol
C. 0.15 mol
D. 0.2 mol
Question 2
A 2.00 g sample of a nonmetal (X) is burned in the presence of oxygen (O2) to produce 3.00 g of X2O3. What is the empirical formula of the nonmetal?
A. X2O3
B. XO2
C. X2O
D. XO
Question 3
A 2.5 M solution of a weak acid HA has a pH of 4.5. What is the concentration of the acid?
A. 0.01 M
B. 0.1 M
C. 0.5 M
D. 1 M
Question 4
A solution contains 0.1 M HCl. What is the concentration of H+ ions in the solution?
A. 0.05 M
B. 0.1 M
C. 0.15 M
D. 0.2 M
Question 5
A 2.5 L flask contains 0.5 mol of an ideal gas at 300 K. What is the pressure of the gas?
A. 0.5 atm
B. 1 atm
C. 1.5 atm
D. 2 atm
Question 6
A 2.5 L flask contains 0.5 mol of an ideal gas at 300 K. What is the pressure of the gas?
A. 0.5 atm
B. 1 atm
C. 1.5 atm
D. 2 atm
Question 7
The rate cons\tant (k) for a first-order reaction is 0.05 min^-1. If the initial concentration of the reac\tant is 0.1 M, calculate the concentration after 10 minutes.
A. 0.01
B. 0.02
C. 0.03
D. 0.04
Question 8
A 1.00 M solution of NaOH is titrated with 0.500 M HCl. What is the pH of the solution after 50.0 mL of HCl has been added?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 9
A gas at 300 K has a volume of 2.5 L. If the temperature is increased to 400 K, what is the new volume?
A. 3.2 L
B. 4.0 L
C. 4.8 L
D. 5.6 L
Question 10
A 2.5 L sample of a 0.2 M solution of sodium carbonate (Na2CO3) is mixed with 1.5 L of a 0.1 M solution of hydrochloric acid (HCl). Calculate the pH of the resulting solution.
A. 1
B. 2
C. 3
D. 4
Question 11
A 2.00 M solution of HCl is titrated with 0.500 M NaOH. What is the pH of the solution after 25.0 mL of NaOH has been added?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 12
A 25 mL sample of 0.5 M acetic acid (CH3COOH) is titrated with 1 M sodium hydroxide (NaOH). Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.025
B. 0.05
C. 0.075
D. 0.1
Question 13
Determine the number of moles of sulfur trioxide (SO3) produced when 2.50 g of sulfur (S) is burned in the presence of oxygen (O2) according to the equation: 2S + 3O2 → 2SO3.
A. 0.0500 mol
B. 0.100 mol
C. 0.150 mol
D. 0.200 mol
Question 14
Determine the molar mass of a polymer with the following composition: 60% polyethylene (C2H4), 20% polypropylene (C3H6), and 20% polyvinyl chloride (C2H3Cl).
A. 60 g/mol
B. 80 g/mol
C. 100 g/mol
D. 120 g/mol
Question 15
A 0.500 M solution of a weak acid (HA) is titrated with a 0.500 M solution of a strong base (NaOH). What is the pH of the resulting solution after the reaction is complete?
A. 1.00
B. 2.00
C. 3.00
D. 4.00

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