POST UTME FUTA 2022 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
The half-life of a radioactive subs\tance is 10.0 days. If 50 g of the subs\tance is initially present, calculate the amount of the subs\tance remaining after 20 days.
A. 12.5 g
B. 25.0 g
C. 50.0 g
D. 100 g
Question 2
A metal (M) reacts with oxygen (O2) to form a metal oxide (MO2). If the balanced equation for the reaction is: 4M + 3O2 → 2MO2, what is the mass of 2.0 moles of MO2?
A. 80 g
B. 120 g
C. 160 g
D. 200 g
Question 3
A solution contains 0.5 g of KNO3 per 100 mL. What is the concentration of the solution in g/L?
A. 0.5 g/L
B. 1 g/L
C. 2 g/L
D. 5 g/L
Question 4
Determine the molar mass of a polymer sample with the following composition: 85% polyethylene (C2H4)n, 10% polypropylene (C3H6)n, and 5% polystyrene (C6H5CHCH3)n. Given that the molar mass of polyethylene is 14.0 g/mol, the molar mass of polypropylene is 42.1 g/mol, and the molar mass of polystyrene is 104.2 g/mol.
A. 170.0 g/mol
B. 200.0 g/mol
C. 220.0 g/mol
D. 250.0 g/mol
Question 5
A 0.5 M solution of sodium carbonate (Na2CO3) is mixed with a 0.5 M solution of hydrochloric acid (HCl). If the reaction is complete, what is the concentration of the remaining Na2CO3 solution?
A. 0.0 M
B. 0.25 M
C. 0.5 M
D. 0.75 M
Question 6
A 2.5 L sample of a 0.25 M glu\cose solution is diluted to 5 L. What is the new concentration of the solution?
A. 0.0625 M
B. 0.125 M
C. 0.25 M
D. 0.5 M
Question 7
A 1.0 M solution of H2SO4 is electrolyzed u\sing a platinum electrode. If the electrolysis is carried out for 2 hours, and the current is 5.0 A, what is the mass of hydrogen gas collected at the cathode?
A. 0.50 g
B. 1.0 g
C. 2.0 g
D. 4.0 g
Question 8
The half-life of a radioactive subs\tance is 5.0 days. If 100 g of the subs\tance is initially present, calculate the amount of the subs\tance remaining after 20 days.
A. 12.5 g
B. 25.0 g
C. 50.0 g
D. 100 g
Question 9
A solution contains 0.1 M HCl and 0.1 M NaOH. Determine the pH of the solution.
A. 1
B. 2
C. 3
D. 4
Question 10
A 1.0 M solution of sodium carbonate (Na2CO3) is titrated with 1.0 M hydrochloric acid (HCl) until the equivalence point is reached. Calculate the volume of hydrochloric acid required to reach the equivalence point.
A. 100 mL
B. 200 mL
C. 300 mL
D. 400 mL
Question 11
The reaction of hydrogen gas with oxygen gas is represented by the equation: 2H2(g) + O2(g) → 2H2O(l). Calculate the volume of oxygen gas required to react with 2.0 L of hydrogen gas at STP.
A. 1.0 L
B. 2.0 L
C. 3.0 L
D. 4.0 L
Question 12
Determine the number of moles of glu\cose (C6H12O6) that can be obtained from 2.5 L of a 0.25 M glu\cose solution.
A. 0.0625 mol
B. 0.125 mol
C. 0.25 mol
D. 0.5 mol
Question 13
Calculate the molarity of a solution containing 2.5 g of NaCl in 250 mL of water.
A. 0.1 M
B. 0.2 M
C. 0.3 M
D. 0.4 M
Question 14
A 3.0 M solution of potassium nitrate (KNO3) is mixed with a 2.0 M solution of sodium chloride (NaCl). Calculate the concentration of the resulting solution.
A. 1.5 M
B. 2.0 M
C. 2.5 M
D. 3.0 M
Question 15
A 0.500 M solution of sodium hydroxide (NaOH) is titrated with 0.250 M hydrochloric acid (HCl) until the equivalence point is reached. Calculate the volume of hydrochloric acid required to reach the equivalence point.
A. 100 mL
B. 200 mL
C. 300 mL
D. 400 mL

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