POST UTME AFE BABALOLA UNIVERSITY 2019 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
Determine the number of moles of ethene (C2H4) produced when 2.50 g of C2H4 is decomposed at cons\tant pressure and temperature.
A. 0.0500 mol
B. 0.100 mol
C. 0.200 mol
D. 0.500 mol
Question 2
Determine the pH of a 0.1 M solution of hydrochloric acid (HCl).
A. 0.1
B. 1.0
C. 2.0
D. 3.0
Question 3
Calculate the number of moles of oxygen gas (O2) produced at STP when 2.5 moles of methane (CH4) react with excess oxygen gas according to the equation: CH4 + 2O2 → CO2 + 2H2O.
A. 1.25 moles
B. 2.5 moles
C. 3.75 moles
D. 5 moles
Question 4
Determine the number of moles of carbon dioxide produced from the combustion of 2.5 g of glu\cose (C6H12O6) according to the equation: C6H12O6 + 6O2 → 6CO2 + 6H2O.
A. 0.25 mol
B. 0.5 mol
C. 1.0 mol
D. 1.5 mol
Question 5
A 2.5 g sample of sulfur (S8) is burned in oxygen gas to produce sulfur dioxide gas. Calculate the volume of sulfur dioxide gas produced at STP.
A. 1.25 L
B. 2.5 L
C. 3.75 L
D. 5 L
Question 6
The s\tandard electrode potential of the zinc-zinc ion couple is -0.76 V. Calculate the s\tandard electrode potential of the copper-copper ion couple if the s\tandard electrode potential of the copper-copper ion couple is 0.34 V.
A. 0.10 V
B. 0.34 V
C. 0.50 V
D. 0.76 V
Question 7
A sample of nitrogen gas occupies a volume of 2.5 L at a pressure of 1.5 atm. What is the volume of the gas at a pressure of 3.0 atm, assuming the temperature remains cons\tant?
A. 1.0 L
B. 1.5 L
C. 2.0 L
D. 2.5 L
Question 8
A 2.5 M solution of hydrochloric acid (HCl) is mixed with a 2.5 M solution of sodium hydroxide (NaOH). Calculate the number of moles of water (H2O) produced after the reaction is complete.
A. 1.25 moles
B. 2.5 moles
C. 3.75 moles
D. 5 moles
Question 9
A solution of HCl is 0.100 M. What is the pH of the solution?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 10
A 2.5 M solution of sodium hydroxide (NaOH) is mixed with a 2.5 M solution of hydrochloric acid (HCl). Calculate the pH of the resulting solution after the reaction is complete.
A. 1
B. 2
C. 3
D. 4
Question 11
A sample of a gas has a volume of 2.50 L at a pressure of 1.00 atm. What is the volume of the gas at a pressure of 2.00 atm, assuming the temperature remains cons\tant?
A. 1.25 L
B. 2.50 L
C. 3.75 L
D. 5.00 L
Question 12
A sample of 0.500 L of a gas at 25°C and 1.00 atm is collected over water at 25°C. If the vapor pressure of water at 25°C is 23.8 mmHg, what is the partial pressure of the gas?
A. 0.977 atm
B. 0.983 atm
C. 0.987 atm
D. 0.993 atm
Question 13
A 2.50 g sample of a gas is collected over water at 25°C and 1.00 atm. If the vapor pressure of water at 25°C is 23.8 mmHg, what is the partial pressure of the gas?
A. 0.977 atm
B. 0.983 atm
C. 0.987 atm
D. 0.993 atm
Question 14
Calculate the s\tandard enthalpy change for the reaction: 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s). Given that ΔH°(Al2O3) = -1675 kJ/mol and ΔH°(Fe) = 0 kJ/mol.
A. -3350 kJ/mol
B. -1675 kJ/mol
C. -335 kJ/mol
D. -1675 kJ/mol
Question 15
A 2.50 g sample of a polymer is dissolved in 100.0 mL of a solvent. If the polymer is 95% soluble, what is the molar mass of the polymer?
A. 1.00 x 10^4 g/mol
B. 2.00 x 10^4 g/mol
C. 3.00 x 10^4 g/mol
D. 4.00 x 10^4 g/mol

Master the Exam!

You've seen a preview, but there are thousands more questions plus AI tutor to break down complex solutions.

Unlock Full Access Available for Android & Windows
Help others prepare! Share this practice hub: