POST UTME FUTO 2020 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A 10.0 mL sample of a solution containing 0.100 M HCl is titrated with 0.100 M NaOH. Calculate the volume of NaOH required to reach the equivalence point.
A. 10.0 mL
B. 20.0 mL
C. 30.0 mL
D. 40.0 mL
Question 2
A 2.5 L flask contains 0.5 mol of an ideal gas at 27°C. If the gas is heated to 127°C at cons\tant volume, what is the final pressure in atmospheres?
A. 1.5 atm
B. 2.0 atm
C. 2.5 atm
D. 3.0 atm
Question 3
The diagram below shows a simple black and white chemistry apparatus showing titration setup.
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 4
The diagram below shows a titration setup.
A. \( H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O \)
B. \( H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O + 2Na^+ \)
C. \( H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O + 2H^+ \)
D. \( H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O + 2OH^- \)
Question 5
Determine the number of moles of nitrogen gas (N2) produced when 2.5 moles of ammonia (NH3) react with 2.5 moles of oxygen gas (O2) according to the following equation: 4NH3 + 5O2 → 4N2 + 6H2O.
A. 1.25
B. 2.5
C. 3.75
D. 5.0
Question 6
The boiling point of a solution containing 10% ethanol (C2H5OH) and 90% water (H2O) is 78.5°C. What is the boiling point elevation of the solution?
A. 0.5°C
B. 1.0°C
C. 1.5°C
D. 2.0°C
Question 7
A 25.0 mL sample of a solution containing 0.100 M NaCl is titrated with 0.100 M AgNO_3. What is the pH of the solution after the reaction is complete?
A. \( pH = 7 \)
B. \( pH = 8 \)
C. \( pH = 9 \)
D. \( pH = 10 \)
Question 8
Determine the number of moles of oxygen gas (O2) produced at STP when 2.50 g of potassium chlorate (KClO3) is decomposed according to the equation: 2KClO3(s) → 2KCl(s) + 3O2(g).
A. 0.050 mol
B. 0.100 mol
C. 0.150 mol
D. 0.200 mol
Question 9
The diagram below shows a titration setup.
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 10
A 25.0 mL sample of 0.100 M NaOH is titrated with 0.0500 M HCl. Calculate the number of moles of HCl required to reach the equivalence point.
A. 0.00250 mol
B. 0.00500 mol
C. 0.00750 mol
D. 0.0100 mol
Question 11
The s\tandard Gibbs free energy change (ΔG°) for the reaction: 2NO(g) + O2(g) → 2NO2(g) is -111.3 kJ mol-1. Calculate the equilibrium cons\tant (K) for the reaction at 298 K.
A. 1.0 × 10^5
B. 1.0 × 10^6
C. 1.0 × 10^7
D. 1.0 × 10^8
Question 12
A 2.5 L flask contains 0.5 g of CO2 at 298 K. Calculate the partial pressure of CO2 in the flask.
A. 0.5 atm
B. 0.5 atm
C. 0.5 atm
D. 0.5 atm
Question 13
The reaction of potassium permanganate with hydrogen peroxide in acidic medium is a classic example of a redox reaction. What is the half-reaction that involves the reduction of permanganate ion \( MnO4- \)?
A. MnO4- + 8H+ + 5e- → Mn2+ + 4H2O
B. MnO4- + 8H+ + 5e- → MnO2 + 4H2O
C. MnO4- + 8H+ + 5e- → Mn2+ + 4H2O + 2H2
D. MnO4- + 8H+ + 5e- → MnO2 + 4H2O + 2H2
Question 14
A metal (M) reacts with oxygen to form a basic oxide. The reaction is represented by the equation: 4M + 3O2 → 2M2O3. If 2.5 g of M reacts with 1.5 g of O2, calculate the percentage yield of M2O3.
A. 85%
B. 85%
C. 85%
D. 85%
Question 15
Determine the s\tandard enthalpy of formation of CaCO3(s) from the following data: ΔHf(CaO(s)) = -635.09 kJ/mol, ΔHf(CO2(g)) = -393.51 kJ/mol. Assume the reaction is CaO(s) + CO2(g) → CaCO3(s).
A. -1783.6 kJ/mol
B. -1783.6 kJ/mol
C. -1783.6 kJ/mol
D. -1783.6 kJ/mol

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