POST UTME GREENFIELD UNIVERSITY 2017 Chemistry | Objective

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Question 1
The reaction between chlorine gas and sodium hydroxide solution is a classic example of a redox reaction. Write the balanced chemical equation for this reaction.
A. \text{Cl}_2 + 2\text{NaOH} \rightarrow 2\text{NaCl} + \text{H}_2\text{O}
B. \text{Cl}_2 + 2\text{NaOH} \rightarrow \text{NaCl} + \text{NaOCl} + \text{H}_2\text{O}
C. \text{Cl}_2 + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O}
D. \text{Cl}_2 + 2\text{NaOH} \rightarrow \text{NaCl} + \text{NaOCl}
Question 2
A 25.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the pH of the solution after 25.0 mL of NaOH has been added.
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 3
The reaction of an alkene with bromine produces a dibromide. What is the type of reaction that occurred?
A. Addition reaction
B. Elimination reaction
C. Substitution reaction
D. Oxidation reaction
Question 4
A 5.00 g sample of a non-metallic oxide is dissolved in 25.0 mL of water to give a solution with a pH of 3.00. Calculate the molar mass of the oxide.
A. 50.0 g/mol
B. 75.0 g/mol
C. 100 g/mol
D. 125 g/mol
Question 5
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of combustion of 1.5 g of carbon at 298 K.
A. -589.25 kJ
B. -589.75 kJ
C. -590.25 kJ
D. -590.75 kJ
Question 6
The half-life of a radioactive subs\tance is 5 years. If 100 g of the subs\tance is initially present, how much will remain after 20 years?
A. 12.5 g
B. 25.0 g
C. 37.5 g
D. 50.0 g
Question 7
A 2.50 L sample of a gas at 25°C and 1 atm is collected over water at 25°C. If the partial pressure of water vapor is 0.031 atm, what is the volume of the gas at STP?
A. 2.50 L
B. 2.50 L - 0.031 L
C. 2.50 L + 0.031 L
D. 2.50 L x \( 1 atm / 1 atm \)
Question 8
A 10.0 mL sample of a 0.100 M solution of a strong acid is titrated with 0.100 M NaOH. Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.0050 mol
B. 0.010 mol
C. 0.015 mol
D. 0.020 mol
Question 9
A 1.00 L sample of a gas at 25°C and 1 atm is collected over water at 25°C. If the partial pressure of water vapor is 0.031 atm, what is the volume of the gas at STP?
A. 1.00 L
B. 1.00 L - 0.031 L
C. 1.00 L + 0.031 L
D. 1.00 L x \( 1 atm / 1 atm \)
Question 10
A 10.0 mL sample of a 0.100 M solution of a strong acid is titrated with 0.100 M NaOH. Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.0050 mol
B. 0.010 mol
C. 0.015 mol
D. 0.020 mol
Question 11
A 5.00 g sample of a non-metallic oxide is dissolved in 25.0 mL of water to give a solution with a pH of 3.00. Calculate the molar mass of the oxide.
A. 50.0 g/mol
B. 75.0 g/mol
C. 100 g/mol
D. 125 g/mol
Question 12
A 2.5 M solution of sodium hydroxide is prepared by dissolving 12.5 g of sodium hydroxide in 250 mL of water. What is the concentration of the solution in moles per liter?
A. 0.1 M
B. 0.5 M
C. 1.0 M
D. 2.5 M
Question 13
A sample of a polymer has a molecular weight of 50,000 g/mol. If 2.5 g of the polymer is dissolved in 100 mL of solvent, what is the concentration of the solution in g/L?
A. 0.05 g/L
B. 0.10 g/L
C. 0.20 g/L
D. 0.50 g/L
Question 14
A 25.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the pH of the solution after 25.0 mL of NaOH has been added.
A. 2.00
B. 2.00
C. 2.00
D. 2.00
Question 15
A 1.0 M solution of hydrochloric acid is prepared by dissolving 36.5 g of hydrochloric acid in 250 mL of water. What is the concentration of the solution in moles per liter?
A. 0.1 M
B. 0.5 M
C. 1.0 M
D. 2.5 M

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