POST UTME IMS U 2020 Chemistry | Objective

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Question 1
A 25.0 mL sample of a solution containing 0.100 M NaOH is titrated with 0.100 M HCl. Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.00250 mol
B. 0.00275 mol
C. 0.00300 mol
D. 0.00325 mol
Question 2
A 1.0 M solution of a salt, NaCl, is mixed with 1.0 M HCl. What is the pH of the resulting solution?
A. 1.0
B. 2.0
C. 3.0
D. 4.0
Question 3
A sample of a solid is placed in a beaker and 20 mL of 2.0 M sodium hydroxide (NaOH) is added. The resulting solution is heated to 373 K. What is the resulting solution?
A. A solution of sodium hydroxide and water
B. A solution of sodium hydroxide and the solid
C. A solution of water and the solid
D. A solution of the solid and the beaker
Question 4
Determine the s\tandard enthalpy of formation of CaCO3(s) from the following data: ΔHf(CaO(s)) = -635.09 kJ/mol, ΔHf(CO2(g)) = -393.51 kJ/mol, ΔHf(Ca(s)) = -178.2 kJ/mol.
A. -1206.8 kJ/mol
B. -1206.9 kJ/mol
C. -1206.7 kJ/mol
D. -1206.6 kJ/mol
Question 5
The reaction between CH3OH(l) and HCl(aq) is catalyzed by H+ ions. If the initial concentration of CH3OH is 0.5 M and the initial concentration of HCl is 0.2 M, calculate the concentration of CH3OH after 10 minutes if the rate cons\tant is 0.05 min^-1.
A. 0.3 M
B. 0.4 M
C. 0.5 M
D. 0.6 M
Question 6
A sample of nitrogen gas at 25°C and 1 atm is placed in a container with a volume of 2 L. What is the number of moles of nitrogen gas present in the container?
A. \( \frac{1 \times 2}{22.4} \)
B. \( \frac{1 \times 2}{24.4} \)
C. \( \frac{1 \times 2}{20.4} \)
D. \( \frac{1 \times 2}{18.4} \)
Question 7
A 2.5 L flask contains 0.5 mol of an ideal gas at a temperature of 298 K. The gas is heated to a temperature of 373 K. Calculate the new volume of the gas, assuming that the amount of gas remains cons\tant.
A. 3.5 L
B. 4.5 L
C. 5.5 L
D. 6.5 L
Question 8
A 0.1 M solution of a weak base, B, is titrated with 0.1 M HCl. If the initial pH of the solution is 9.5, what is the pH after the addition of 20 mL of 0.1 M HCl?
A. 7.5
B. 8.5
C. 9.5
D. 10.5
Question 9
A 2.5 M solution of H2O2 is electrolyzed u\sing a platinum electrode. If the electrolysis is carried out for 2 hours, and the volume of O2 gas collected is 1.2 L at 25°C and 1 atm, calculate the number of moles of O2 gas collected.
A. 0.06 mol
B. 0.07 mol
C. 0.08 mol
D. 0.09 mol
Question 10
A 0.1 M solution of a weak acid, HA, is titrated with 0.1 M NaOH. If the initial pH of the solution is 3.5, what is the pH after the addition of 20 mL of 0.1 M NaOH?
A. 4.5
B. 5.5
C. 6.5
D. 7.5
Question 11
The boiling point of a solution containing 10.0 g of glu\cose (C6H12O6) in 100.0 g of water is 99.5°C. Calculate the molality of the solution.
A. 0.500 m
B. 0.600 m
C. 0.700 m
D. 0.800 m
Question 12
The diagram below shows the structure of a ha\logen. What is the type of bond that exists between the central atom and the outer atoms?
A. Covalent bond
B. Ionic bond
C. Polar covalent bond
D. Hydrogen bond
Question 13
The diagram below shows a titration setup. Identify the part labeled A.
A. A burette
B. A pipette
C. A flask
D. A beaker
Question 14
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. What is the s\tandard enthalpy of formation of H2O(l) if the s\tandard enthalpy of formation of H2(g) is 0 kJ/mol and the s\tandard enthalpy of formation of O2(g) is 0 kJ/mol?
A. \( -285.8 \)
B. \( -241.8 \)
C. \( -393.5 \)
D. \( -285.8 + 393.5 \)
Question 15
A sample of a gas at 25°C and 1 atm is collected over water at 25°C. If the vapor pressure of water at 25°C is 23.8 mmHg, determine the partial pressure of the gas.
A. 760 mmHg
B. 737 mmHg
C. 760 - 23.8 = 736.2 mmHg
D. 760 - 23.8 = 736.2 mmHg

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