POST UTME JOSEPH AYO BABALOLA UNIVERSITY 2017 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A solution of acetic acid (CH3COOH) is prepared by dissolving 20 mL of CH3COOH in 250 mL of water. What is the pH of the solution?
A. 2.3
B. 2.5
C. 2.7
D. 2.9
Question 2
The electrolysis of water produces hydrogen gas at the cathode and oxygen gas at the anode. If 2.0 g of hydrogen gas is collected at the cathode, what is the volume of oxygen gas collected at the anode, assuming a cons\tant temperature and pressure?
A. 0.125 L
B. 0.25 L
C. 0.5 L
D. 1.0 L
Question 3
A 1.0 M solution of ethanol (C2H5OH) is mixed with a 2.0 M solution of water (H2O). If the resulting solution is 1.5 M, what is the mole \fraction of ethanol in the resulting solution?
A. 0.25
B. 0.33
C. 0.50
D. 0.67
Question 4
A 2.5 M solution of hydrochloric acid (HCl) is prepared by dissolving 25 g of HCl in 100 mL of water. Calculate the pKa of the solution.
A. 1.2
B. 1.6
C. 2.0
D. 2.4
Question 5
A solution of 0.1 M NaCl is electrolyzed u\sing a platinum electrode. What is the concentration of Cl2 at the anode after 10 minutes?
A. 0.01 M
B. 0.05 M
C. 0.1 M
D. 0.5 M
Question 6
The s\tandard Gibbs free energy of formation of a compound is related to its s\tandard enthalpy of formation and s\tandard entropy of formation by the equation: \Delta G_f^\circ = \Delta H_f^\circ - T\Delta S_f^\circ. If the s\tandard Gibbs free energy of formation of a compound is -100.5 kJ/mol at 298 K, and the s\tandard enthalpy of formation is -393.5 kJ/mol, calculate the s\tandard entropy of formation.
A. 1.33 kJ/mol*K
B. 1.33 kJ/mol*K
C. 1.33 kJ/mol*K
D. 1.33 kJ/mol*K
Question 7
A sample of hydrogen gas (H2) is collected over water at a temperature of 25°C and a pressure of 1 atm. If the volume of the gas is 2.5 L, calculate the partial pressure of the hydrogen gas.
A. 0.5 atm
B. 1.0 atm
C. 1.5 atm
D. 2.0 atm
Question 8
The s\tandard Gibbs free energy of formation of a compound is related to its s\tandard enthalpy of formation and s\tandard entropy of formation by the equation: \Delta G_f^\circ = \Delta H_f^\circ - T\Delta S_f^\circ. If the s\tandard Gibbs free energy of formation of a compound is -100.5 kJ/mol at 298 K, and the s\tandard enthalpy of formation is -393.5 kJ/mol, calculate the s\tandard entropy of formation.
A. 1.33 kJ/mol*K
B. 1.33 kJ/mol*K
C. 1.33 kJ/mol*K
D. 1.33 kJ/mol*K
Question 9
A 2.0 M solution of acetic acid (CH3COOH) is titrated with a 1.0 M solution of sodium hydroxide (NaOH). If 25.0 mL of NaOH is required to reach the equivalence point, what is the volume of acetic acid required to reach the equivalence point?
A. 12.5 mL
B. 25.0 mL
C. 50.0 mL
D. 100.0 mL
Question 10
In the electrolysis of a solution of copper(II) sulfate, what is the primary product at the cathode?
A. Oxygen gas
B. Hydrogen gas
C. Copper metal
D. Sulfuric acid
Question 11
A 2.5 M solution of ammonia (NH3) is prepared by dissolving 25 g of NH3 in 100 mL of water. Calculate the pOH of the solution.
A. 12
B. 13
C. 14
D. 15
Question 12
A 2.0 M solution of sodium hydroxide (NaOH) is mixed with a 1.0 M solution of acetic acid (CH3COOH). If the resulting solution is 1.5 M, what is the mole \fraction of sodium acetate (CH3COONa) in the resulting solution?
A. 0.25
B. 0.33
C. 0.50
D. 0.67
Question 13
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of formation of CaCO3(s) if the s\tandard enthalpy of formation of CaO(s) is -635.09 kJ/mol and that of CO2(g) is -393.5 kJ/mol.
A. -1207.19 kJ/mol
B. -1207.19 kJ/mol
C. -1207.19 kJ/mol
D. -1207.19 kJ/mol
Question 14
A solution of sodium chloride (NaCl) is prepared by dissolving 35.5 g of NaCl in 250 mL of water. What is the molarity of the solution?
A. 0.14 M
B. 0.18 M
C. 0.22 M
D. 0.26 M
Question 15
The s\tandard Gibbs free energy of formation of a compound is related to its s\tandard enthalpy of formation and s\tandard entropy of formation by the equation: \Delta G_f^\circ = \Delta H_f^\circ - T\Delta S_f^\circ. If the s\tandard Gibbs free energy of formation of a compound is -100.5 kJ/mol at 298 K, and the s\tandard enthalpy of formation is -393.5 kJ/mol, calculate the s\tandard entropy of formation.
A. 1.33 kJ/mol*K
B. 1.33 kJ/mol*K
C. 1.33 kJ/mol*K
D. 1.33 kJ/mol*K

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