POST UTME FUTO 2018 Chemistry | Objective

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Question 1
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, ΔHf(C) = 0 kJ/mol.
A. -1206.60 kJ/mol
B. -1206.61 kJ/mol
C. -1206.59 kJ/mol
D. -1206.62 kJ/mol
Question 2
A 2.0 g sample of a non-metal (X) is heated in a stream of oxygen to produce a gas (Y). The gas (Y) is collected over water and its density is found to be 1.2 g/L at 20°C. What is the identity of the gas (Y)?
A. CO2
B. H2O
C. SO2
D. Cl2
Question 3
A 2.0 M solution of H2SO4 is titrated with 0.5 M NaOH. If 30 mL of NaOH is required to reach the equivalence point, what is the number of moles of H2SO4?
A. 0.1 mol
B. 0.2 mol
C. 0.3 mol
D. 0.4 mol
Question 4
A 2.00 L flask contains 0.500 mol of SO2 gas at 25°C. Calculate the mole \fraction of SO2 in the flask.
A. 0.250
B. 0.500
C. 0.750
D. 1.00
Question 5
A 1.00 g sample of a non-electrolyte is dissolved in 100.0 mL of water. What is the boiling point elevation of the solution?
A. 0.500°C
B. 1.00°C
C. 1.50°C
D. 2.00°C
Question 6
A 10.0 g sample of sulfur is burned in oxygen to produce sulfur dioxide. If the reaction is 100% efficient, what is the volume of oxygen required?
A. 2.50 L
B. 5.00 L
C. 7.50 L
D. 10.0 L
Question 7
A 10 mL sample of a solution containing 0.5 M NaOH is mixed with 20 mL of a solution containing 0.2 M HCl. What is the pH of the resulting solution?
A. 1
B. 2
C. 3
D. 4
Question 8
The atomic radius of an element in the periodic table increases down a group due to the addition of new energy levels. However, the atomic radius of an element in the periodic table 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 9
A 5.00 L flask contains 0.250 mol of N2 gas at 25°C. Calculate the partial pressure of N2 in the flask.
A. 0.500 atm
B. 0.250 atm
C. 0.750 atm
D. 1.00 atm
Question 10
A 2.00 L flask contains 0.500 mol of an ideal gas at 27°C. Calculate the number of moles of gas that must be added to the flask to increase the pressure to 1.00 x 10^5 Pa.
A. 0.250 mol
B. 0.500 mol
C. 1.00 mol
D. 0.750 mol
Question 11
A 2.50 L sample of a gas at 27°C and 1.00 atm is compressed to 0.500 L at 35°C. What is the final pressure of the gas?
A. 1.50 atm
B. 2.50 atm
C. 3.00 atm
D. 4.00 atm
Question 12
Calculate the s\tandard enthalpy change for the reaction: 2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s). The s\tandard enthalpy of formation for Al2O3(s) is -1675 kJ/mol, and the s\tandard enthalpy of formation for Fe2O3(s) is -824 kJ/mol. The s\tandard enthalpy of formation for Al(s) is 0 kJ/mol, and the s\tandard enthalpy of formation for Fe(s) is 0 kJ/mol.
A. -1819 kJ/mol
B. -1599 kJ/mol
C. -2219 kJ/mol
D. -1419 kJ/mol
Question 13
A 1.00 g sample of a non-electrolyte is dissolved in 100.0 mL of water. What is the concentration of the solution?
A. 1.00 M
B. 2.00 M
C. 3.00 M
D. 4.00 M
Question 14
Determine the molar mass of a polymer with the repeating unit [C6H5C6H4]n. The molar mass of benzene (C6H6) is 78.11 g/mol.
A. [C6H5C6H4]n has a molar mass of 156.22 g/mol
B. [C6H5C6H4]n has a molar mass of 78.11 g/mol
C. [C6H5C6H4]n has a molar mass of 312.44 g/mol
D. [C6H5C6H4]n has a molar mass of 39.05 g/mol
Question 15
A solution contains 5.0 g of glu\cose (C6H12O6) per 100 mL of solution. What is the molarity of the solution?
A. 0.027 M
B. 0.054 M
C. 0.1 M
D. 0.2 M

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