POST UTME SUMMIT UNIVERSITY 2025 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A 1.00 g sample of a metal is heated in a crucible until it is completely oxidized. If the mass of the oxide produced is 2.50 g, what is the empirical formula of the metal?
A. Fe
B. Cu
C. Zn
D. Mg
Question 2
A 2.5 M solution of HCl is mixed with a 1.0 M solution of NaOH. Calculate the number of moles of HCl that react with NaOH.
A. 0.005 mol
B. 0.01 mol
C. 0.015 mol
D. 0.02 mol
Question 3
A 2.50 g sample of a hydrocarbon is burned in a bomb calorimeter, relea\sing 12.5 kJ of heat. If the heat of combustion of the hydrocarbon is 46.0 kJ/g, what is the empirical formula of the hydrocarbon?
A. C_(2)H_(6)
B. C_(3)H_(8)
C. C_(4)H_(10)
D. C_(5)H_(12)
Question 4
The s\tandard enthalpy of formation of H2O(l) is -285.8 kJ/mol. Calculate the s\tandard enthalpy of combustion of 1.0 mol of C6H12O6(s).
A. -2800.0 kJ/mol
B. -2800.5 kJ/mol
C. -2801.0 kJ/mol
D. -2801.5 kJ/mol
Question 5
A solution contains 0.020 M HCl and 0.030 M NaOH. What is the pH of the solution?
A. ( 2.0 )
B. ( 3.0 )
C. ( 4.0 )
D. ( 5.0 )
Question 6
The enthalpy of combustion of glu\cose is -2800 kJ/mol. What is the enthalpy of combustion of 2.00 g of glu\cose?
A. -5.60 kJ
B. -11.2 kJ
C. -17.6 kJ
D. -23.9 kJ
Question 7
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of formation of H2O(l) from the following reaction: CO(g) + H2(g) → H2O(l) + 393.5 kJ.
A. -285.8 kJ/mol
B. -241.8 kJ/mol
C. -393.5 kJ/mol
D. -285.8 kJ/mol
Question 8
A 2.50 L flask contains 0.250 mol of N2 gas at 298 K. Calculate the partial pressure of N2 gas in the flask.
A. 0.101 kPa
B. 0.202 kPa
C. 0.303 kPa
D. 0.404 kPa
Question 9
A 2.0 L flask contains 0.10 mol of an ideal gas at 298 K. What is the pressure of the gas in the flask?
A. \( 1.01 \times 10^{5} \) Pa
B. \( 2.02 \times 10^{5} \) Pa
C. \( 3.03 \times 10^{5} \) Pa
D. \( 4.04 \times 10^{5} \) Pa
Question 10
A 1.00 L flask contains 0.500 mol of CO2 gas at 298 K. Calculate the partial pressure of CO2 gas in the flask.
A. 0.101 kPa
B. 0.202 kPa
C. 0.303 kPa
D. 0.404 kPa
Question 11
A diagram of a chromatography setup is shown below. If the mobile phase is 0.100 M NaCl and the stationary phase is 0.0500 M NaOH, what is the pH of the resulting solution?
A. 9.25
B. 9.50
C. 9.75
D. 10.00
Question 12
A 0.50 M solution of NaOH is mixed with a 0.75 M solution of HCl. What is the resulting concentration of NaOH?
A. ( 0.25 ) M
B. ( 0.50 ) M
C. ( 0.75 ) M
D. ( 1.0 ) M
Question 13
A 1.00 g sample of a non-metallic element has a mass of 1.00 g. If the density of the element is 4.00 g/cm^3, what is the volume of the sample?
A. 0.250 cm^3
B. 0.500 cm^3
C. 1.00 cm^3
D. 2.00 cm^3
Question 14
A 1.00 M solution of HCl is mixed with a 1.00 M solution of NaOH. If the reaction is allowed to go to completion, what is the concentration of the resulting solution?
A. 0.50 M
B. 1.00 M
C. 1.50 M
D. 2.00 M
Question 15
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of formation of CO(g) and O2(g) from their elements at 298 K.
A. -110.5 kJ/mol
B. -393.5 kJ/mol
C. -74.8 kJ/mol
D. -285.8 kJ/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: