POST UTME ESUT 2024 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A solution contains 0.100 M HCl and 0.100 M NaOH. Calculate the pH of the solution after mixing 50.0 mL of each solution.
A. ( 7.00 )
B. ( 7.50 )
C. ( 8.00 )
D. ( 9.00 )
Question 2
A solution of hydrochloric acid has a pH of 2. What is the concentration of the acid in moles per liter?
A. 0.01 M
B. 0.1 M
C. 1.0 M
D. 10 M
Question 3
A 2.50-L flask contains 0.150 mol of an ideal gas at 298 K. Calculate the pressure of the gas, assuming that the gas behaves ideally.
A. \( \frac{0.150 \times 8.314 \times 298}{2.50} \)
B. \( \frac{0.150 \times 8.314 \times 298}{2.50 \times 10^{-3}} \)
C. \( \frac{0.150 \times 8.314 \times 298}{2.50 \times 10^{3}} \)
D. \( \frac{0.150 \times 8.314 \times 298}{2.50 \times 10^{-5}} \)
Question 4
The reaction of an alkane with chlorine gas in the presence of light produces a dichloroalkane. What is the name of the reaction?
A. Ha\logenation
B. Oxidation
C. Reduction
D. Substitution
Question 5
The diagram below shows a titration setup. What is the purpose of the burette?
A. To measure the volume of the acid
B. To measure the volume of the base
C. To mix the acid and base
D. To measure the pH of the solution
Question 6
A solution contains 0.100 M HCl and 0.100 M NaOH. Calculate the pH of the solution after mixing 50.0 mL of each solution.
A. ( 7.00 )
B. ( 7.50 )
C. ( 8.00 )
D. ( 9.00 )
Question 7
The reaction of sulfuric acid with sodium hydroxide produces water and sodium sulfate. What is the balanced chemical equation for this reaction?
A. H_2SO_4 + NaOH \rightarrow Na_2SO_4 + H_2O
B. H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O
C. H_2SO_4 + NaOH \rightarrow NaHSO_4 + H_2O
D. H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + H_2O
Question 8
A sample of nitrogen gas occupies a volume of 2.5 L at a pressure of 1.5 atm and a temperature of 300 K. What is the new volume of the gas if the pressure is increased to 3.0 atm and the temperature is decreased to 200 K?
A. 1.2 L
B. 1.5 L
C. 1.8 L
D. 2.0 L
Question 9
A 2.00-L flask contains 0.150 mol of an ideal gas at 298 K. Calculate the pressure of the gas, assuming that the gas behaves ideally.
A. \( \frac{0.150 \times 8.314 \times 298}{2.00} \)
B. \( \frac{0.150 \times 8.314 \times 298}{2.00 \times 10^{-3}} \)
C. \( \frac{0.150 \times 8.314 \times 298}{2.00 \times 10^{3}} \)
D. \( \frac{0.150 \times 8.314 \times 298}{2.00 \times 10^{-5}} \)
Question 10
At 298 K, the s\tandard Gibbs free energy change for the reaction 2NO(g) + O2(g) → 2NO2(g) is -111.3 kJ/mol. Calculate the equilibrium cons\tant (K) for this reaction.
A. \( e^{-\frac{-111300}{8.314 \times 298}} \)
B. \( e^{\frac{-111300}{8.314 \times 298}} \)
C. \( e^{-\frac{111300}{8.314 \times 298}} \)
D. \( e^{\frac{111300}{8.314 \times 298}} \)

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