POST UTME UI 2025 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
The reaction of hydrogen gas with oxygen gas yields water. What is the balanced chemical equation for this reaction?
A. 2H2 + O2 → 2H2O
B. H2 + O2 → H2O
C. 2H2 + 2O2 → 2H2O
D. H2 + 2O2 → 2H2O
Question 2
A sample of carbon dioxide gas is collected over water at a temperature of 25°C and a pressure of 1 atm. If the partial pressure of water vapor is 0.031 atm, what is the mole \fraction of carbon dioxide in the sample?
A. 0.95
B. 0.96
C. 0.97
D. 0.98
Question 3
The reaction of cyclohexane with bromine in the presence of light yields a mixture of 1,2-dibromocyclohexane and 1,4-dibromocyclohexane. What is the major product of this reaction?
A. 1,2-dibromocyclohexane
B. 1,4-dibromocyclohexane
C. cis-1,2-dibromocyclohexane
D. trans-1,2-dibromocyclohexane
Question 4
The reaction between hydrogen gas and chlorine gas is highly exothermic. Write the balanced equation for the reaction: H_(2)(g) + Cl_(2)(g) → HCl(g).
A. 2H_(2)(g) + Cl_(2)(g) → 2HCl(g)
B. H_(2)(g) + Cl_(2)(g) → HCl(g)
C. 2H_(2)(g) + 2Cl_(2)(g) → 4HCl(g)
D. H_(2)(g) + 2Cl_(2)(g) → 2HCl(g)
Question 5
The diagram below shows a titration setup. Identify the part labeled A.
A. The burette
B. The pipette
C. The Erlenmeyer flask
D. The thermometer
Question 6
A solution of 0.1 M sodium chloride is prepared by dissolving 6.0 g of sodium chloride in 100 mL of water. What is the concentration of the solution in g/L?
A. 0.6 g/L
B. 0.7 g/L
C. 0.8 g/L
D. 0.9 g/L
Question 7
A 1.0 M solution of H2SO4 is prepared by dissolving 98.0 g of H2SO4 in 1.0 L of water. What is the concentration of H+ ions in the solution?
A. 0.5 M
B. 1.0 M
C. 1.5 M
D. 2.0 M
Question 8
A metal M reacts with chlorine gas to form a white solid MX. If 2.5 g of M is used and 3.2 g of MX is formed, what is the percentage yield of MX?
A. 80%
B. 85%
C. 90%
D. 95%
Question 9
The diagram below shows a setup for the reaction between sulfuric acid and sodium hydroxide. What is the purpose of the beaker?
A. To mix the acid and base
B. To measure the volume of the acid
C. To measure the volume of the base
D. To filter the solution
Question 10
A sample of a polymer has a molecular weight of 100,000 g/mol. If the polymer is composed of 80% monomer A and 20% monomer B, what is the average molecular weight of the polymer?
A. 80,000 g/mol
B. 90,000 g/mol
C. 100,000 g/mol
D. 110,000 g/mol
Question 11
A non-metal 'X' reacts with oxygen to form a compound 'Y'. The compound 'Y' has a molecular formula of X2O5. Identify the non-metal 'X' and the compound 'Y'.
A. X = S, Y = SO2
B. X = P, Y = P2O5
C. X = Cl, Y = Cl2O5
D. X = Br, Y = Br2O5
Question 12
The element with atomic number 36 is _______.
A. Krypton
B. Strontium
C. Barium
D. Radium
Question 13
Determine the s\tandard enthalpy of formation of the compound C2H6O (ethanol) from the following data: ΔHf(C2H6O) = -234.7 kJ/mol, ΔHf(C2H6) = -84.7 kJ/mol, ΔHf(O2) = 0 kJ/mol. Assume that the reaction is carried out at 298 K.
A. -150.0 kJ/mol
B. -200.0 kJ/mol
C. -250.0 kJ/mol
D. -300.0 kJ/mol
Question 14
A 0.5 M solution of HCl is titrated with 0.5 M NaOH. If 25 mL of HCl is required to reach the equivalence point, what is the number of moles of HCl used?
A. 0.125 mol
B. 0.25 mol
C. 0.375 mol
D. 0.5 mol
Question 15
A solution of NaOH is used to titrate a solution of HCl. If 25 mL of HCl is required to reach the equivalence point and the concentration of HCl is 0.5 M, what is the concentration of NaOH?
A. 0.25 M
B. 0.5 M
C. 0.75 M
D. 1 M

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