POST UTME COVENANT UNIVERSITY 2025 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A solution contains 0.2 M H2SO4 and 0.2 M NaOH. Calculate the pH of the solution.
A. 1
B. 2
C. 3
D. 4
Question 2
A sample of nitrogen gas is collected over water at 25°C and 1 atm. If the partial pressure of water vapor is 0.02 atm, what is the partial pressure of nitrogen?
A. 0.98 atm
B. 0.99 atm
C. 1.01 atm
D. 1.02 atm
Question 3
In the reaction of 2-methylpropane with chlorine, what is the major product formed?
A. 1,2-dichloro-2-methylpropane
B. 1,1-dichloro-2-methylpropane
C. 2-chloro-2-methylpropane
D. 2,2-dichloro-2-methylpropane
Question 4
Determine the s\tandard Gibbs free energy change (ΔG°) for the reaction: 2Ag+(aq) + 2Cl-(aq) → 2AgCl(s) at 25°C, given that the s\tandard enthalpy change (ΔH°) is -146.0 kJ/mol and the s\tandard entropy change (ΔS°) is -173.0 J/mol·K.
A. -146.0 kJ/mol
B. -146.0 kJ/mol + 173.0 J/mol·K
C. -146.0 kJ/mol - 173.0 J/mol·K
D. -146.0 kJ/mol + 173.0 kJ/mol·K
Question 5
A metal M reacts with chlorine gas to form a white solid product. The reaction is represented by the equation: M + Cl2 → MCl2. If 2.5 g of M reacts with 3.2 g of Cl2, what is the mass of the product formed?
A. 5.6 g
B. 6.1 g
C. 6.8 g
D. 7.5 g
Question 6
A 1.0 M solution of NaOH is titrated with 1.0 M HCl. If 20 mL of HCl is required to reach the equivalence point, calculate the pH of the solution at the equivalence point.
A. 7
B. 10
C. 14
D. 12
Question 7
A 50 mL sample of a solution containing 0.1 M HCl is titrated with 0.1 M NaOH. Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.005
B. 0.01
C. 0.015
D. 0.02
Question 8
A 2.50 g sample of a subs\tance is dissolved in 25.0 mL of water. The resulting solution has a concentration of 0.100 M. What is the molar mass of the subs\tance?
A. 10.0 g/mol
B. 20.0 g/mol
C. 30.0 g/mol
D. 40.0 g/mol
Question 9
Determine the number of unpaired electrons in the ground state of a neutral atom with atomic number 15.
A. 3
B. 5
C. 7
D. 9
Question 10
A 2.5 M solution of H2SO4 is titrated with 1 M NaOH. What is the pH of the solution after 25 mL of NaOH has been added?
A. 1
B. 2
C. 3
D. 4
Question 11
A 0.1 M solution of HCl is titrated with 0.1 M NaOH. If 20 mL of NaOH is required to reach the equivalence point, calculate the volume of HCl required to reach the equivalence point.
A. 200 mL
B. 20 mL
C. 2 mL
D. 2000 mL
Question 12
A polymer has the following structure: [-CH2-CH2-CH2-CH2-]n. What is the IUPAC name of this polymer?
A. Polyethylene
B. Polypropylene
C. Polyvinyl chloride
D. Polystyrene
Question 13
A redox reaction involves the oxidation of Cu(s) to Cu2+(aq) and the reduction of Ag+(aq) to Ag(s). Write the balanced half-equations for the reaction.
A. Cu(s) → Cu2+(aq) + 2e-
B. Ag+(aq) + e- → Ag(s)
C. Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)
D. Cu2+(aq) + 2e- → Cu(s)
Question 14
A metal M reacts with oxygen gas to form a brown solid product. The reaction is represented by the equation: 4M + 3O2 → 2M2O3. If 2.5 g of M reacts with 3.2 g of O2, what is the mass of the product formed?
A. 5.6 g
B. 6.1 g
C. 6.8 g
D. 7.5 g
Question 15
A 2.00 L sample of a 0.500 M solution of CH3OH is mixed with 1.00 L of a 0.500 M solution of HCl. What is the concentration of the resulting solution?
A. 0.250 M
B. 0.500 M
C. 0.750 M
D. 1.00 M

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