POST UTME MOUNTAIN TOP UNIVERSITY 2020 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
The solubility of silver chloride (AgCl) in water is 1.2 × 10^\( -10 \) mol/L. What is the molar solubility of AgCl?
A. 1.2 × 10^\( -10 \)
B. 1.2 × 10^\( -9 \)
C. 1.2 × 10^\( -8 \)
D. 1.2 × 10^\( -7 \)
Question 2
The atomic radius of an element increases down a group in the periodic table due to the addition of new energy levels. However, the atomic radius of an element decreases across a period due to the increase in effective nuclear charge. Which of the following elements has the largest atomic radius?
A. Rb
B. Cs
C. Fr
D. Ba
Question 3
A 10 mL sample of a solution containing 0.5 M NaOH is titrated with 0.1 M HCl. What is the pH of the solution after the titration?
A. 1
B. 2
C. 3
D. 4
Question 4
A 25.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. What is the pH of the solution after the reaction is complete?
A. 1
B. 7
C. 10
D. 12
Question 5
The s\tandard electrode potential of a metal is a measure of its t\endency to lose electrons. Which of the following metals has the highest s\tandard electrode potential?
A. Li
B. Na
C. K
D. Ca
Question 6
The reaction of hydrogen gas with oxygen gas is a classic example of a combustion reaction. Write the balanced chemical equation for this reaction.
A. 2H2 + O2 → 2H2O
B. H2 + O2 → H2O
C. 2H2 + O2 → H2O2
D. H2 + O2 → H2O2
Question 7
Calculate the s\tandard enthalpy change (ΔH°) for the reaction: 2Al(s) + Fe₂O₃(s) → 2Fe(s) + Al₂O₃(s). The s\tandard enthalpy of formation (ΔH°f) values are: Al₂O₃(s) = -1675.7 kJ/mol, Al(s) = 0 kJ/mol, Fe₂O₃(s) = -825.4 kJ/mol, and Fe(s) = 0 kJ/mol.
A. -1547.9 kJ/mol
B. -1547.1 kJ/mol
C. -1546.3 kJ/mol
D. -1545.5 kJ/mol
Question 8
A solution of H2SO4 is titrated with a solution of NaOH. If 30 cm3 of the H2SO4 solution requires 40 cm3 of the NaOH solution for neutralization, calculate the concentration of the H2SO4 solution.
A. 0.2 M
B. 0.5 M
C. 1 M
D. 2 M
Question 9
A 2.5 g sample of an organic compound is dissolved in 25 mL of ethanol. What is the molarity of the solution?
A. 0.1 M
B. 0.2 M
C. 0.3 M
D. 0.4 M
Question 10
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 the copper ion in the product?
A. 0
B. +2
C. -2
D. +1
Question 11
The electrolysis of a solution of CuSO4 in water produces Cu metal and SO2 gas. If the current used is 2.5 A and the time taken is 3 hours, calculate the mass of Cu metal deposited at the cathode.
A. 0.25 kg
B. 0.5 kg
C. 1 kg
D. 2 kg
Question 12
The reaction of sodium hydroxide with acetic acid is a classic example of a neutralization reaction. Write the balanced chemical equation for this reaction.
A. NaOH + CH3COOH → NaCH3COO + H2O
B. NaOH + CH3COOH → NaCH3COOH + H2O
C. NaOH + CH3COOH → CH3COONa + H2O
D. NaOH + CH3COOH → NaOH + CH3COOH
Question 13
A diagram of a titration setup is shown below.
A. The burette contains the acid.
B. The beaker contains the acid.
C. The burette contains the base.
D. The beaker contains the base.
Question 14
A 0.500 M solution of NaOH is mixed with a 0.500 M solution of HCl. What is the resulting pH?
A. 1.00
B. 2.00
C. 3.00
D. 4.00
Question 15
A 2.0 g sample of an organic compound is burned in a bomb calorimeter. The heat released is 12.5 kJ. What is the enthalpy change per mole of the compound?
A. -6000 J/mol
B. -8000 J/mol
C. -10000 J/mol
D. -12000 J/mol

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