POST UTME KSU 2022 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
The compound 2,2-dimethylpropane is an example of a branched alkane. Draw the structure of this compound.
A. CH3CH2CH3
B. CH3CH2CH2CH3
C. CH3C(CH3)2CH3
D. CH3CH(CH3)CH3
Question 2
A 0.500 M solution of NaOH is mixed with a 0.500 M solution of HCl. What is the pH of the resulting solution?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 3
A diagram of a titration setup is shown below. If 25.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the concentration of the HCl solution?
A. 0.100 M
B. 0.200 M
C. 0.500 M
D. 1.00 M
Question 4
A 2.5 g sample of an unknown hydrocarbon is burned in a combustion calorimeter. The temperature of the calorimeter increases by 23.5°C. If the calorimeter cons\tant is 2.5 J/g°C, what is the heat of combustion of the hydrocarbon, assuming it is a pure subs\tance?
A. 100 kJ/mol
B. 200 kJ/mol
C. 300 kJ/mol
D. 400 kJ/mol
Question 5
At 298 K, the s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of formation of CO(g) if the s\tandard enthalpy of formation of O2(g) is 0 kJ/mol.
A. -110.5 kJ/mol
B. -393.5 kJ/mol
C. 110.5 kJ/mol
D. 393.5 kJ/mol
Question 6
A solution contains 0.1 M NaCl. If 10 mL of this solution is diluted to 100 mL, what is the concentration of the resulting solution?
A. 0.01 M
B. 0.1 M
C. 1 M
D. 10 M
Question 7
The reaction of potassium dichromate with sulfuric acid in the presence of iron(II) sulfate is an example of a redox reaction. Write the balanced half-equations for the oxidation and reduction reactions.
A. Cr2O72- + 14H+ + 6e- → 2Cr3+ + 7H2O
B. Cr2O72- + 14H+ + 6e- → 2Cr3+ + 7H2O
C. Fe2+ → Fe3+ + e-
D. Cr3+ + 3e- → Cr
Question 8
The compound 1,2-dimethylcyclohexane is an example of a branched alkane. Draw the structure of this compound.
A. CH3CH2CH2CH3
B. CH3C(CH3)2CH3
C. CH3CH(CH3)CH3
D. CH3CH2CH(CH3)CH3
Question 9
A diagram of a titration setup is shown below. If 35.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the concentration of the HCl solution?
A. 0.100 M
B. 0.200 M
C. 0.500 M
D. 1.00 M
Question 10
A diagram of a titration setup is shown below.
A. Titration of HCl with NaOH
B. Titration of NaOH with HCl
C. Titration of H2SO4 with NaOH
D. Titration of NaOH with H2SO4
Question 11
The reaction of chlorine with sodium hydroxide is an example of a redox reaction. Write the balanced equation for this reaction.
A. 2NaOH + Cl2 → NaCl + NaClO + H2O
B. 2NaOH + Cl2 → NaCl + NaClO + H2O
C. 2NaOH + Cl2 → NaCl + NaClO + H2O
D. 2NaOH + Cl2 → NaCl + NaClO + H2O
Question 12
The s\tandard electrode potential of the Zn^2+/Zn couple is -0.76 V. If the s\tandard electrode potential of the Cu^2+/Cu couple is +0.34 V, what is the s\tandard cell potential of the cell consisting of these two couples?
A. -1.1 V
B. -0.4 V
C. +0.4 V
D. +1.1 V
Question 13
A sample of a metal oxide, MO, has a mass of 25 g. The metal has a molar mass of 50 g/mol and the oxide has a molar mass of 100 g/mol. What is the empirical formula of the metal oxide?
A. MO
B. M2O
C. M3O2
D. M4O3
Question 14
The periodic table is arranged in a way that elements with similar properties are placed in the same group. What is the name of the group that contains the noble gases?
A. Group 1
B. Group 2
C. Group 18
D. Group 17
Question 15
A 0.1 M solution of K2Cr2O7 is treated with 10 mL of 1 M HCl. If the reaction is complete, what is the concentration of Cr3+ ions in the solution?
A. 0.01 M
B. 0.02 M
C. 0.03 M
D. 0.04 M

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