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POST UTME FUTA 2022 Chemistry | Objective

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Question 1 View Details

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

Correct B. 0.125 mol

C. 0.25 mol

D. 0.5 mol

Correct Answer: B

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Question 2 View Details

A 25 mL sample of a 0.1 M NaOH solution is titrated with 0.1 M HCl. Calculate the number of moles of HCl required to neutralize the NaOH.

A. 0.0025 mol

Correct B. 0.005 mol

C. 0.01 mol

D. 0.02 mol

Correct Answer: B

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Question 3 View Details

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

Correct B. 1 g/L

C. 2 g/L

D. 5 g/L

Correct Answer: B

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Question 4 View Details

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

Correct B. 0.125 M

C. 0.25 M

D. 0.5 M

Correct Answer: B

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Question 5 View Details

A 25 mL sample of a 0.1 M NaOH solution is titrated with 0.1 M HCl. Calculate the pH of the solution after the titration.

A. 7

Correct B. 8

C. 9

D. 10

Correct Answer: B

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Question 6 View Details

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

Correct B. 200.0 g/mol

C. 220.0 g/mol

D. 250.0 g/mol

Correct Answer: B

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Question 7 View Details

A 2.5 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 oxygen gas collected at the anode?

A. 0.25 g

B. 0.50 g

Correct C. 1.0 g

D. 2.0 g

Correct Answer: C

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Question 8 View Details

A 0.1 M solution of NaCl is mixed with 10 mL of 0.1 M AgNO3. What is the concentration of the resulting solution?

A. 0.05 M

B. 0.10 M

Correct C. 0.15 M

D. 0.20 M

Correct Answer: C

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Question 9 View Details

A 1.0 L solution of 0.1 M NaOH is mixed with 1.0 L of 0.1 M HCl. What is the pH of the resulting solution?

A. 7.0

Correct B. 7.5

C. 8.0

D. 9.0

Correct Answer: B

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Question 10 View Details

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

Correct B. 1.0 g

C. 2.0 g

D. 4.0 g

Correct Answer: B

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Question 11 View Details

The rate cons\tant (k) of a first-order reaction is given by the equation: k = Ae^\( -Ea/RT \). If the activation energy (Ea) is 100 kJ/mol, the gas cons\tant (R) is 8.314 J/mol*K, and the temperature (T) is 300 K, what is the value of the rate cons\tant (k) if the pre-exponential factor (A) is 1.0 x 10^10 s^-1?

A. 1.0 x 10^7 s^-1

B. 1.0 x 10^8 s^-1

Correct C. 1.0 x 10^9 s^-1

D. 1.0 x 10^10 s^-1

Correct Answer: C

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Question 12 View Details

A 2.0 M solution of hydrochloric acid (HCl) is mixed with a 2.0 M solution of sodium hydroxide (NaOH). If the reaction is complete, what is the concentration of the remaining HCl solution?

Correct A. 0.0 M

B. 1.0 M

C. 2.0 M

D. 4.0 M

Correct Answer: A

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Question 13 View Details

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

Correct C. 160 g

D. 200 g

Correct Answer: C

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Question 14 View Details

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

Correct B. 0.25 M

C. 0.5 M

D. 0.75 M

Correct Answer: B

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Question 15 View Details

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 M?

A. 80 g

Correct B. 120 g

C. 160 g

D. 200 g

Correct Answer: B

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Question 16 View Details

Determine the pH of a solution containing 0.1 M HCl and 0.1 M NaOH.

A. 1

Correct B. 2

C. 3

D. 4

Correct Answer: B

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Question 17 View Details

Calculate the molarity of a solution containing 2.5 g of NaCl in 250 mL of water.

A. 0.1 M

Correct B. 0.2 M

C. 0.3 M

D. 0.4 M

Correct Answer: B

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Question 18 View Details

Identify the type of chemical reaction represented by the equation: 2NaOH + H2SO4 → Na2SO4 + 2H2O.

A. Synthesis

B. Decomposition

Correct C. Neutralization

D. Combustion

Correct Answer: C

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Question 19 View Details

A 2.5 L flask contains 0.5 mol of CO2 at 298 K. Calculate the partial pressure of CO2.

A. 10 atm

Correct B. 20 atm

C. 30 atm

D. 40 atm

Correct Answer: B

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Question 20 View Details

A solution contains 0.1 M HCl and 0.1 M NaOH. Determine the pH of the solution.

A. 1

Correct B. 2

C. 3

D. 4

Correct Answer: B

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Question 21 View Details

The reaction of zinc metal with copper(II) sulfate solution is represented by the equation: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s). Calculate the number of moles of copper metal deposited from a solution containing 2.5 g of copper(II) sulfate.

A. 0.0156 mol

B. 0.0312 mol

Correct C. 0.0625 mol

D. 0.125 mol

Correct Answer: C

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Question 22 View Details

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

Correct B. 200 mL

C. 300 mL

D. 400 mL

Correct Answer: B

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Question 23 View Details

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.

Correct A. 12.5 g

B. 25.0 g

C. 50.0 g

D. 100 g

Correct Answer: A

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Question 24 View Details

A 2.0 M solution of potassium nitrate (KNO3) is mixed with a 3.0 M solution of sodium chloride (NaCl). Calculate the concentration of the resulting solution.

A. 1.5 M

Correct B. 2.0 M

C. 2.5 M

D. 3.0 M

Correct Answer: B

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Question 25 View Details

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

Correct C. 3.0 L

D. 4.0 L

Correct Answer: C

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