POST UTME CALEB UNIVERSITY 2021 Chemistry | Objective

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Question 1
A solution of 0.100 M HCl is mixed with a solution of 0.100 M NaOH. If 25.0 mL of HCl is added to 50.0 mL of NaOH, what is the pH of the resulting solution?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 2
A 0.100 M solution of H2SO4 is titrated with a 0.100 M solution of NaOH. If 25.0 mL of NaOH is required to reach the equivalence point, what is the pH of the solution?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 3
A 2.00 M solution of H2SO4 is mixed with a 2.00 M solution of NaOH. If 25.0 mL of H2SO4 is added to 50.0 mL of NaOH, what is the concentration of the resulting solution?
A. 1.00 M
B. 1.50 M
C. 2.00 M
D. 2.50 M
Question 4
A 2.5 L flask contains 0.5 mol of CO2 at 298 K. Calculate the partial pressure of CO2 in the flask.
A. 1.01 atm
B. 1.02 atm
C. 1.03 atm
D. 1.04 atm
Question 5
A 2.5 L flask contains 0.5 mol of CO2 at 298 K. Calculate the mole \fraction of CO2 in the flask.
A. 0.2
B. 0.3
C. 0.4
D. 0.5
Question 6
A 2.00 M solution of HCl is mixed with a 2.00 M solution of NaOH. If 25.0 mL of HCl is added to 50.0 mL of NaOH, what is the concentration of the resulting solution?
A. 1.00 M
B. 1.50 M
C. 2.00 M
D. 2.50 M
Question 7
A 0.1 M solution of NaCl is prepared by dissolving 2.5 g of NaCl in 100 mL of water. Calculate the molarity of the solution after 10 mL of 1 M HCl is added to it.
A. 0.15 M
B. 0.20 M
C. 0.25 M
D. 0.30 M
Question 8
A polymer is formed from the reaction of 1,4-butadiene with sulfur dichloride (SCl2). The polymer has a molecular weight of 50,000 g/mol and a degree of polymerization of 200. What is the molar mass of the repeating unit?
A. 250 g/mol
B. 500 g/mol
C. 750 g/mol
D. 1000 g/mol
Question 9
A mixture of 1.00 g of an unknown metal chloride and 2.00 g of an excess of silver nitrate is dissolved in 10.0 mL of water. The resulting solution is then titrated with 0.100 M NaOH. If 25.0 mL of NaOH is required to reach the equivalence point, what is the molar mass of the metal chloride?
A. 100 g/mol
B. 150 g/mol
C. 200 g/mol
D. 250 g/mol
Question 10
A sample of $\text{H}_2$ gas occupies a volume of 3.00 L at a pressure of 0.500 atm. What is the volume of the gas at a pressure of 1.00 atm, assuming the temperature remains cons\tant?
A. 1.50 L
B. 2.00 L
C. 3.00 L
D. 4.00 L
Question 11
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of formation of CO(g) if the s\tandard enthalpy of formation of C(s) is 0 kJ/mol and the s\tandard enthalpy of formation of O2(g) is 0 kJ/mol.
A. -110.5 kJ/mol
B. -110.5 kJ/mol
C. -110.5 kJ/mol
D. -110.5 kJ/mol
Question 12
A 2.50 L flask contains 0.500 mol of an ideal gas at 25°C. If the gas is heated to 125°C at cons\tant volume, what is the new pressure in atm?
A. 2.00 atm
B. 2.50 atm
C. 3.00 atm
D. 3.50 atm
Question 13
A 2.00 M solution of HCl is prepared by dissolving 40.0 g of HCl in 1.00 L of water. What is the concentration of H+ ions in the solution?
A. 2.00 M
B. 4.00 M
C. 6.00 M
D. 8.00 M
Question 14
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of formation of CH4(g) if the s\tandard enthalpy of formation of C(s) is -394.4 kJ/mol and that of H2(g) is 0 kJ/mol.
A. -74.8 kJ/mol
B. -74.9 kJ/mol
C. -75.0 kJ/mol
D. -75.1 kJ/mol
Question 15
A 2.50 L flask contains 0.500 mol of an ideal gas at 25°C. If the gas is heated to 125°C at cons\tant pressure, what is the new volume in L?
A. 3.00 L
B. 3.50 L
C. 4.00 L
D. 4.50 L

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