POST UTME VERITAS UNIVERSITY 2018 Chemistry | Objective

Practice these randomly selected questions to test your readiness.

Question 1
A 2.5 M solution of sodium hydroxide (NaOH) is mixed with a 1.0 M solution of hydrochloric acid (HCl). What is the resulting concentration of the sodium chloride (NaCl) solution?
A. 1.5 M
B. 2.0 M
C. 2.5 M
D. 3.0 M
Question 2
A 0.500 L flask contains 0.100 mol of CO2 at 25°C. What is the partial pressure of CO2 in the flask?
A. 0.500 atm
B. 1.00 atm
C. 1.50 atm
D. 2.00 atm
Question 3
A 1.00 L of 0.100 M HCl is titrated with 0.100 M NaOH. What is the pH of the solution after 50.0 mL of NaOH has been added?
A. 3.00
B. 4.00
C. 5.00
D. 6.00
Question 4
A sample of oxygen gas occupies a volume of 2.5 L at a pressure of 1.5 atm and a temperature of 300 K. What is the new volume of the gas if the pressure is increased to 3.0 atm and the temperature is decreased to 200 K?
A. 1.2 L
B. 2.0 L
C. 2.5 L
D. 3.0 L
Question 5
The reaction between sodium and chlorine produces a compound with the formula NaCl. What is the type of bond that exists between the sodium and chlorine atoms?
A. ionic
B. covalent
C. metallic
D. hydrogen
Question 6
The energy of an electron in the nth orbit of a hydrogen atom is given by the equation \( E_n = -\frac{13.6}{n^2} \) eV. What is the energy of an electron in the 3rd orbit?
A. -3.4
B. -1.5
C. 1.1
D. 13.6
Question 7
A solution contains 2.5 g of glu\cose (C6H12O6) dissolved in 100 mL of water. What is the molarity of the solution?
A. 0.25 M
B. 0.50 M
C. 1.0 M
D. 2.0 M
Question 8
A 1.00 L sample of a 0.100 M solution of NaOH is mixed with 1.00 L of a 0.100 M solution of HCl. Calculate the pH of the resulting solution.
A. 7.00
B. 8.00
C. 9.00
D. 10.00
Question 9
A 2.50 g sample of an unknown hydrocarbon is burned in a combustion calorimeter, producing 8.00 mL of CO2 gas at STP. If the molar mass of the hydrocarbon is 84.0 g/mol, what is its empirical formula?
A. C2H4
B. C3H6
C. C4H8
D. C5H10
Question 10
A solution of HCl is added to a solution of NaOH. The reaction is as follows: 2NaOH + HCl → NaCl + 2H2O. If 25.0 mL of 0.100 M HCl is added to 25.0 mL of 0.100 M NaOH, what is the concentration of the resulting solution?
A. 0.0500 M
B. 0.100 M
C. 0.150 M
D. 0.200 M
Question 11
A 2.50 g sample of an unknown hydrocarbon is burned in a combustion calorimeter, producing 8.00 mL of CO2 gas at STP. If the molar mass of the hydrocarbon is 84.0 g/mol, what is its empirical formula?
A. C2H4
B. C3H6
C. C4H8
D. C5H10
Question 12
A sample of 1.00 L of 0.100 M HCl is titrated with 0.100 M NaOH. What is the pH of the solution after 25.0 mL of NaOH has been added?
A. 2.00
B. 3.00
C. 4.00
D. 5.00
Question 13
A sample of an ideal gas at 27°C and 1.00 atm is heated to 127°C at cons\tant pressure. Calculate the final volume of the gas, given that the initial volume is 2.50 L.
A. 3.00 L
B. 4.00 L
C. 5.00 L
D. 6.00 L
Question 14
Determine the number of moles of oxygen gas (O2) that will react with 2.50 moles of hydrogen gas (H2) according to the balanced equation: 2H2 + O2 → 2H2O.
A. 1.25 moles
B. 2.50 moles
C. 3.75 moles
D. 5.00 moles
Question 15
A 2.00 L flask contains 0.500 mol of an ideal gas at 25°C. What is the pressure of the gas in the flask?
A. 1.00 atm
B. 2.00 atm
C. 3.00 atm
D. 4.00 atm

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