POST UTME CALEB UNIVERSITY 2022 Chemistry | Objective

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Question 1
A sample of 1.0 g of an unknown metal is heated in a crucible until it melts. The mass of the crucible and metal is 1.5 g, and the mass of the crucible alone is 1.2 g. Calculate the density of the metal.
A. 8.3
B. 9.2
C. 10.1
D. 11.0
Question 2
A 2.0 L sample of a gas at 25°C and 1.0 atm is compressed to 2.5 atm at cons\tant temperature. Calculate the new volume of the gas.
A. 1.6
B. 1.8
C. 2.0
D. 2.2
Question 3
A 0.500 M solution of 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 4
A 1.0 M solution of $H_2SO_4$ is mixed with a 1.0 M solution of $NaOH$. If the reaction is allowed to go to completion, what is the concentration of the resulting solution?
A. 0.5 M
B. 1.0 M
C. 1.5 M
D. 2.0 M
Question 5
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(s)) = 0 kJ/mol.
A. -1206.60 kJ/mol
B. -1206.19 kJ/mol
C. -1206.11 kJ/mol
D. -1206.31 kJ/mol
Question 6
A 100.0 mL sample of a solution containing 0.0500 M NaOH is titrated with 0.100 M HCl. If 50.0 mL of HCl is required to reach the equivalence point, what is the volume of the NaOH solution?
A. 50.0 mL
B. 100.0 mL
C. 150.0 mL
D. 200.0 mL
Question 7
A 1.0 M solution of $HCl$ is mixed with a 1.0 M solution of $NaOH$. If the reaction is allowed to go to completion, what is the concentration of the resulting solution?
A. 0.5 M
B. 1.0 M
C. 1.5 M
D. 2.0 M
Question 8
A 2.50 g sample of a metal (M) is dissolved in 50.0 mL of 0.100 M HCl. The resulting solution is then titrated with 0.0500 M NaOH. If 25.0 mL of NaOH is required to reach the equivalence point, what is the identity of the metal?
A. Zn
B. Fe
C. Cu
D. Ag
Question 9
A 25 mL sample of 0.5 M HCl is titrated with 0.5 M NaOH. Calculate the number of moles of NaOH required to reach the equivalence point.
A. 0.0125
B. 0.025
C. 0.0375
D. 0.05
Question 10
A 25.0-mL sample of a solution containing 0.100 M NaOH is titrated with 0.100 M HCl. What is the pH of the solution after the titration?
A. 7.00
B. 8.00
C. 9.00
D. 10.0
Question 11
A 3.00 L flask contains 0.200 mol of an ideal gas at 37°C. Calculate the temperature of the gas in Kelvin.
A. 300 K
B. 400 K
C. 500 K
D. 600 K
Question 12
A 2.00 g sample of a metal carbonate is heated to produce a 0.500 g sample of the metal oxide. What is the molar mass of the metal carbonate?
A. 100.0 g/mol
B. 200.0 g/mol
C. 300.0 g/mol
D. 400.0 g/mol
Question 13
A 2.50 L flask contains 0.150 mol of an ideal gas at 27°C. Calculate the pressure of the gas in pascals.
A. 1.01 × 10^5 Pa
B. 2.02 × 10^5 Pa
C. 3.03 × 10^5 Pa
D. 4.04 × 10^5 Pa
Question 14
A sample of CO2 gas is collected over water at a temperature of 25°C and a pressure of 1.00 atm. What is the partial pressure of CO2 in the gas mixture?
A. 0.800 atm
B. 0.900 atm
C. 1.00 atm
D. 1.10 atm
Question 15
At 25°C, the equilibrium cons\tant (Kp) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) is 0.032. Calculate the partial pressure of NH3(g) when the partial pressures of N2(g) and H2(g) are 0.500 atm and 1.00 atm, respectively.
A. 0.010 atm
B. 0.032 atm
C. 0.064 atm
D. 0.125 atm

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