POST UTME VERITAS UNIVERSITY 2017 Chemistry | Objective

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Question 1
A metal M reacts with chlorine gas to form a white solid MX. The molar mass of M is 55.85 g/mol, and the molar mass of Cl is 35.45 g/mol. Calculate the molar mass of MX.
A. 90.3
B. 91.3
C. 92.3
D. 93.3
Question 2
Calculate the s\tandard enthalpy of formation of CO2(g) from the following equation: C(s) + O2(g) → CO2(g). The s\tandard enthalpy of formation of C(s) is -393.5 kJ/mol, and the s\tandard enthalpy of formation of O2(g) is 0 kJ/mol.
A. -393.5 kJ/mol
B. -393.5 kJ/mol + 0 kJ/mol
C. -393.5 kJ/mol + 0 kJ/mol + 0 kJ/mol
D. -393.5 kJ/mol + 0 kJ/mol + 0 kJ/mol + 0 kJ/mol
Question 3
A diagram of a polymer chain is shown below. If the chain has a molecular weight of 100,000 g/mol and the density of the polymer is 1.5 g/mL, what is the volume of the polymer chain?
A. 0.1 mL
B. 0.5 mL
C. 1 mL
D. 5 mL
Question 4
Determine the pH of a 0.1 M solution of HCl at 25°C, given that the dissociation cons\tant of HCl is 10^\( -7 \) and the temperature dep\endence of the dissociation cons\tant is given by the equation \( K = K_0 \times 10^{\( 0.01 \times (T - 25 \ \))} ).
A. 1
B. 2
C. 3
D. 4
Question 5
A solution of sodium chloride (NaCl) is prepared by dissolving 35.5 g of NaCl in 100 mL of water. Calculate the molar concentration of the solution. Assume the density of the solution is 1.02 g/mL.
A. 0.5 M
B. 1.0 M
C. 1.5 M
D. 2.0 M
Question 6
Determine the structure of the compound formed by the reaction of 2-methylpropane with chlorine gas, given that the reaction is a free-radical ha\logenation.
A. \( \text{CH}_3 \text{CH}_2 \text{CH}_2 \text{Cl} \)
B. \( \text{CH}_3 \text{CH}_2 \text{CH}_2 \text{CH}_2 \text{Cl} \)
C. \( \text{CH}_3 \text{CH}_2 \text{CH}\( \text{Cl})\text{CH}_3 \ \)
D. \( \text{CH}_3 \text{CH}\( \text{Cl})\text{CH}_2 \text{CH}_3 \ \)
Question 7
A 25.0 mL sample of 0.1 M HCl is titrated with 0.1 M NaOH. Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.0025
B. 0.005
C. 0.0075
D. 0.01
Question 8
Determine the number of moles of oxygen gas (O2) produced at STP when 2.5 moles of hydrogen gas (H2) react with oxygen gas according to the equation: 2H2 + O2 → 2H2O.
A. 1.25 moles
B. 2.5 moles
C. 5 moles
D. 10 moles
Question 9
A 100.0 mL sample of a 0.1 M solution of NaOH is titrated with a 0.1 M solution of HCl. Calculate the volume of HCl required to reach the equivalence point.
A. 50.0 mL
B. 75.0 mL
C. 100.0 mL
D. 125.0 mL
Question 10
A sample of sulfur dioxide (SO2) gas is collected over water at a temperature of 25°C and a pressure of 1 atm. Calculate the volume of the gas at s\tandard temperature and pressure (STP).
A. V = \frac{1 atm \times 2 L \times 273 K}{1 atm \times 298 K}
B. V = \frac{1 atm \times 2 L \times 298 K}{1 atm \times 273 K}
C. V = \frac{1 atm \times 2 L \times 273 K}{1 atm \times 298 K} \times \frac{273 K}{298 K}
D. V = \frac{1 atm \times 2 L \times 298 K}{1 atm \times 273 K} \times \frac{298 K}{273 K}
Question 11
A 2.5 g sample of a polymer is dissolved in 50 mL of solvent. If the solution has a density of 1.2 g/mL, what is the concentration of the polymer solution in g/L?
A. 0.1 g/L
B. 0.5 g/L
C. 1 g/L
D. 5 g/L
Question 12
The reaction between nitrogen dioxide (NO2) and ozone (O3) is a key process in the formation of smog. Write the balanced chemical equation for this reaction, including the correct coefficients.
A. 2NO_2 + O_3 \rightarrow 2NO + 2O_2
B. 2NO_2 + O_3 \rightarrow 2NO + O_2
C. NO_2 + O_3 \rightarrow NO + O_2
D. 2NO_2 + O_3 \rightarrow 2NO + 3O_2
Question 13
A solution contains 0.1 M HCl and 0.2 M NaOH. Calculate the pH of the solution.
A. 1.0
B. 2.0
C. 3.0
D. 4.0
Question 14
The periodic table below shows the position of the elements in the periodic table. What is the atomic number of the element in group 17, period 3?
A. 17
B. 18
C. 19
D. 20
Question 15
A diagram of a titration apparatus is shown below. If the burette contains 25 mL of 0.5 M HCl and the equivalence point is reached at 50 mL, what is the concentration of the NaOH solution?
A. 0.1 M
B. 0.25 M
C. 0.5 M
D. 1 M

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