POST UTME BOWEN UNIVERSITY 2022 Chemistry | Objective

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Question 1 View Details
Determine the s\tandard enthalpy of formation of CO2(g) from the following data: ΔH°(C(s) + O2(g) → CO2(g)) = -393.5 kJ/mol and ΔH°(CO(g) + 1/2O2(g) → CO2(g)) = -283.0 kJ/mol.
A. -394.5 kJ/mol
Correct B. -393.5 kJ/mol
C. -283.0 kJ/mol
D. -176.5 kJ/mol

Correct Answer: B

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Question 2 View Details
A 2.5 L flask contains 0.25 mol of an ideal gas at 25°C. What is the pressure of the gas?
A. 1.01 atm
Correct B. 2.01 atm
C. 3.01 atm
D. 4.01 atm

Correct Answer: B

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Question 3 View Details
A solution contains 0.2 M NaCl and 0.1 M CaCl2. What is the concentration of Cl- ions?
A. 0.2 M
Correct B. 0.3 M
C. 0.4 M
D. 0.5 M

Correct Answer: B

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Question 4 View Details
A 2.5 L flask contains 0.25 mol of an ideal gas at 25°C. What is the pressure of the gas?
A. 1.01 atm
Correct B. 2.01 atm
C. 3.01 atm
D. 4.01 atm

Correct Answer: B

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Question 5 View Details
A solution contains 0.2 M NaCl and 0.1 M CaCl2. What is the concentration of Cl- ions?
A. 0.2 M
Correct B. 0.3 M
C. 0.4 M
D. 0.5 M

Correct Answer: B

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Question 6 View Details
The reaction between nitrogen dioxide and water is represented by the equation: 3NO2 + H2O → 2HNO3 + NO. If 2.5 moles of NO2 react with excess water, what is the limiting reac\tant?
Correct A. NO2
B. H2O
C. HNO3
D. NO

Correct Answer: A

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Question 7 View Details
A solution of 0.5 M HCl is titrated with 0.2 M NaOH. If 25 mL of HCl is required to reach the equivalence point, what is the number of moles of NaOH used?
A. 0.0125
Correct B. 0.025
C. 0.05
D. 0.1

Correct Answer: B

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Question 8 View Details
The s\tandard enthalpy of formation of CO2 is -393.5 kJ/mol. What is the s\tandard enthalpy of combustion of 1 mole of methane (CH4) if the reaction is: CH4 + 2O2 → CO2 + 2H2O?
Correct A. -890.3
B. -393.5
C. -74.8
D. -50.5

Correct Answer: A

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Question 9 View Details
A solution of 0.1 M NaOH is titrated with 0.2 M HCl. If 20 mL of HCl is required to reach the equivalence point, what is the pH of the resulting solution?
A. 1
B. 2
C. 3
Correct D. 4

Correct Answer: D

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Question 10 View Details
The half-life of a radioactive subs\tance is 10 years. If 100 g of the subs\tance is present initially, what is the mass remaining after 20 years?
A. 50
B. 25
Correct C. 12.5
D. 6.25

Correct Answer: C

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Question 11 View Details
A sample of an ideal gas at 25°C and 1 atm is heated to 100°C at cons\tant pressure. What is the new volume of the gas?
A. 2.00 L
Correct B. 4.00 L
C. 6.00 L
D. 8.00 L

Correct Answer: B

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Question 12 View Details
A solution of HCl is titrated with a solution of NaOH. The initial pH of the HCl solution is 1.00. What is the pH of the solution after the addition of 25.0 mL of 0.100 M NaOH?
A. 2.00
B. 3.00
Correct C. 4.00
D. 5.00

Correct Answer: C

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Question 13 View Details
A metal atom has an atomic number of 26 and an atomic mass of 55.85 g/mol. What is the number of protons and neutrons in the nucleus of this atom?
Correct A. 26 protons, 29 neutrons
B. 26 protons, 30 neutrons
C. 26 protons, 31 neutrons
D. 26 protons, 32 neutrons

Correct Answer: A

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Question 14 View Details
A 2.50 L sample of a gas at 27°C and 1.20 atm is compressed to 1.00 L at cons\tant temperature. What is the new pressure of the gas?
A. 2.40 atm
B. 2.50 atm
Correct C. 2.60 atm
D. 2.70 atm

Correct Answer: C

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Question 15 View Details
A solution of NaOH is titrated with a solution of HCl. The initial pH of the NaOH solution is 12.00. What is the pH of the solution after the addition of 20.0 mL of 0.100 M HCl?
A. 10.00
B. 11.00
C. 12.00
Correct D. 13.00

Correct Answer: D

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Question 16 View Details
The reaction of zinc metal with copper(II) sulfate solution is represented by the equation: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s). What is the oxidation state of copper in the product Cu(s)?
A. 0
B. +1
Correct C. +2
D. -1

Correct Answer: C

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Question 17 View Details
A 2.5-g sample of a non-metallic element, X, reacts with oxygen gas to form 3.2 g of X2O5. What is the empirical formula of the compound X2O5?
Correct A. X2O5
B. X2O3
C. XO2
D. XO3

Correct Answer: A

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Question 18 View Details
The diagram below shows a titration setup.
A. The burette contains the acid.
B. The beaker contains the acid.
Correct C. The burette contains the base.
D. The beaker contains the base.

Correct Answer: C

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Question 19 View Details
A 1.5-g sample of a metal, M, is heated in a crucible until it melts. The mass of the crucible and the melted metal is 2.2 g. What is the molar mass of the metal M?
A. 50 g/mol
Correct B. 60 g/mol
C. 70 g/mol
D. 80 g/mol

Correct Answer: B

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Question 20 View Details
The diagram below shows a simple black and white chemistry apparatus showing a titration setup.
A. The burette contains the acid.
B. The beaker contains the acid.
Correct C. The burette contains the base.
D. The beaker contains the base.

Correct Answer: C

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Question 21 View Details
Determine the pH of a 0.1 M solution of HCl after 10 mL of 1 M NaOH has been added to 20 mL of the HCl solution. Assume the volume of the resulting solution is 30 mL.
A. 1
Correct B. 2
C. 3
D. 4

Correct Answer: B

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Question 22 View Details
A 25 mL sample of a 0.5 M solution of NaOH is titrated with 1 M HCl. Calculate the volume of HCl required to reach the equivalence point.
A. 10 mL
Correct B. 20 mL
C. 25 mL
D. 30 mL

Correct Answer: B

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Question 23 View Details
A 50 mL sample of a 0.2 M solution of H2SO4 is titrated with 1 M NaOH. Calculate the volume of NaOH required to reach the equivalence point.
A. 20 mL
Correct B. 25 mL
C. 30 mL
D. 35 mL

Correct Answer: B

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Question 24 View Details
A 100 mL sample of a 0.1 M solution of HCl is titrated with 1 M NaOH. Calculate the volume of NaOH required to reach the equivalence point.
A. 50 mL
Correct B. 60 mL
C. 70 mL
D. 80 mL

Correct Answer: B

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Question 25 View Details
A 50 mL sample of a 0.2 M solution of H2SO4 is titrated with 1 M NaOH. Calculate the volume of NaOH required to reach the equivalence point.
A. 25 mL
Correct B. 30 mL
C. 35 mL
D. 40 mL

Correct Answer: B

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