POST UTME AFE BABALOLA UNIVERSITY 2017 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
The diagram below shows the titration of a strong acid with a strong base. What is the pH of the solution after the equivalence point?
A. 7
B. 10
C. 12
D. 14
Question 2
A solution contains 0.1 M sodium chloride (NaCl) and 0.2 M calcium chloride (CaCl2). Calculate the molarity of the chloride ions \( Cl- \) in the solution.
A. 0.1 M
B. 0.2 M
C. 0.3 M
D. 0.4 M
Question 3
The following table shows the atomic radii of some elements in the periodic table. Identify the element with the largest atomic radius.
A. Group 1
B. Group 2
C. Group 17
D. Group 18
Question 4
Determine the rate cons\tant (k) for the reaction: 2NO(g) + O2(g) → 2NO2(g), given that the initial concentrations of NO and O2 are 0.5 M and 0.2 M, respectively, and the rate of reaction is 0.01 M/s after 10 minutes. The rate law is first order with respect to NO and second order with respect to O2.
A. 0.05 M^-1 s^-1
B. 0.1 M^-1 s^-1
C. 0.2 M^-1 s^-1
D. 0.5 M^-1 s^-1
Question 5
A 2.5 L flask contains 0.5 mol of an ideal gas at 298 K. Calculate the pressure of the gas u\sing the ideal gas law.
A. 1.01 × 10^5 Pa
B. 2.02 × 10^5 Pa
C. 3.03 × 10^5 Pa
D. 4.04 × 10^5 Pa
Question 6
A 0.5 M solution of NaOH is mixed with a 0.5 M solution of HCl. Calculate the pH of the resulting solution.
A. 1
B. 2
C. 3
D. 4
Question 7
In the electrolysis of a solution of copper(II) sulfate, what is the primary product at the cathode?
A. Cu
B. Cu2+
C. H2
D. O2
Question 8
The rate cons\tant for a first-order reaction is 0.05 min^-1. If the initial concentration of the reac\tant is 0.1 M, what is the concentration after 10 minutes?
A. 0.05 M
B. 0.025 M
C. 0.1 M
D. 0.5 M
Question 9
What is the major product of the reaction between 2-methylpropane and chlorine?
A. 2-chloro-2-methylpropane
B. 2,2-dichloro-2-methylpropane
C. 2-chloro-2-methyl-1-propane
D. 2-chloro-2-methyl-2-propane
Question 10
The reaction of zinc metal with copper(II) sulfate solution is a classic example of a redox reaction. Write the balanced chemical equation for this reaction, including the state of each subs\tance.
A. Zn + CuSO4 → ZnSO4 + Cu
B. Zn + CuSO4 → ZnSO4 + Cu2O
C. Zn + CuSO4 → ZnO + Cu
D. Zn + CuSO4 → ZnSO4 + CuSO3
Question 11
A 2.5 L flask contains 0.5 mol of an ideal gas at 27°C. Calculate the pressure of the gas in pascals.
A. 101325 Pa
B. 202650 Pa
C. 303875 Pa
D. 405100 Pa
Question 12
The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of combustion of 1 mol of C(s) to form CO2(g).
A. -393.5 kJ/mol
B. -393.5 kJ/mol + 0.5 kJ/mol
C. -393.5 kJ/mol - 0.5 kJ/mol
D. -393.5 kJ/mol + 1 kJ/mol
Question 13
The following diagram shows a setup for a titration experiment. Identify the subs\tance being titrated.
A. Acid
B. Base
C. Salt
D. Water
Question 14
Determine the number of moles of nitrogen gas (N2) produced when 2.5 g of ammonia (NH3) is decomposed at cons\tant pressure and temperature.
A. 0.05 mol
B. 0.1 mol
C. 0.15 mol
D. 0.2 mol
Question 15
A 2.5 L flask contains 0.5 mol of an ideal gas at 298 K. Calculate the pressure of the gas u\sing the ideal gas law.
A. 1.01 × 10^5 Pa
B. 2.02 × 10^5 Pa
C. 3.03 × 10^5 Pa
D. 4.04 × 10^5 Pa

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