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POST UTME CALEB UNIVERSITY 2022 Chemistry | Objective

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Question 1 View Details

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.

Correct A. -1206.60 kJ/mol

B. -1206.19 kJ/mol

C. -1206.11 kJ/mol

D. -1206.31 kJ/mol

Correct Answer: A

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Question 2 View Details

A 0.500 M solution of NaCl is prepared by dissolving 0.500 g of NaCl in 100.0 mL of water. What is the concentration of Na+ ions in the solution?

Correct A. 0.250 M

B. 0.500 M

C. 0.750 M

D. 1.00 M

Correct Answer: A

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Question 3 View Details

A diagram of a titration setup is shown below. If 25.0 mL of 0.100 M HCl is required to reach the equivalence point, what is the concentration of the NaOH solution?

A. 0.0500 M

Correct B. 0.100 M

C. 0.200 M

D. 0.500 M

Correct Answer: B

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Question 4 View Details

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

Correct B. 200.0 g/mol

C. 300.0 g/mol

D. 400.0 g/mol

Correct Answer: B

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Question 5 View Details

A diagram of a simple distillation setup is shown below. If the vapor pressure of the solvent at 25°C is 760 mmHg, what is the boiling point of the solution?

A. 80.0°C

B. 90.0°C

Correct C. 100.0°C

D. 110.0°C

Correct Answer: C

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Question 6 View Details

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

A. 7

B. 10

C. 14

Correct D. 12

Correct Answer: D

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Question 7 View Details

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

Correct B. 0.025

C. 0.0375

D. 0.05

Correct Answer: B

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Question 8 View Details

The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of formation of CH4(g) if the s\tandard enthalpy of formation of C(s) is -710.4 kJ/mol and the s\tandard enthalpy of formation of H2(g) is 0 kJ/mol.

Correct A. -74.8

B. -50.5

C. -20.4

D. -10.2

Correct Answer: A

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Question 9 View Details

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

Correct B. 9.2

C. 10.1

D. 11.0

Correct Answer: B

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Question 10 View Details

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

Correct C. 2.0

D. 2.2

Correct Answer: C

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Question 11 View Details

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

Correct C. 0.064 atm

D. 0.125 atm

Correct Answer: C

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Question 12 View Details

The s\tandard enthalpy of formation of CO2(g) is -393.5 kJ/mol. Calculate the s\tandard enthalpy of combustion of 1.00 mol of C6H12O6(s) at 25°C.

A. -2800 kJ

B. -2900 kJ

Correct C. -3000 kJ

D. -3100 kJ

Correct Answer: C

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Question 13 View Details

A 2.50-g sample of a non-metallic oxide is found to contain 0.750 g of oxygen. What is the empirical formula of the oxide?

A. MgO

Correct B. SiO2

C. CO2

D. SO3

Correct Answer: B

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Question 14 View Details

The pH of a 0.100 M solution of HCl is 1.00. What is the concentration of H+ ions in the solution?

Correct A. 0.100 M

B. 0.100 M

C. 0.100 M

D. 0.100 M

Correct Answer: A

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Question 15 View Details

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?

Correct A. 7.00

B. 8.00

C. 9.00

D. 10.0

Correct Answer: A

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Question 16 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). If 25.0 mL of 0.100 M CuSO4(aq) is reacted with 5.00 g of zinc metal, calculate the number of moles of copper metal produced.

A. 0.0015 mol

Correct B. 0.0025 mol

C. 0.0035 mol

D. 0.0045 mol

Correct Answer: B

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Question 17 View Details

A 2.50 L flask contains 0.150 mol of an ideal gas at 27°C. Calculate the pressure of the gas in pascals.

Correct A. 1.01 × 10^5 Pa

B. 2.02 × 10^5 Pa

C. 3.03 × 10^5 Pa

D. 4.04 × 10^5 Pa

Correct Answer: A

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Question 18 View Details

A solution contains 5.00 g of glu\cose (C6H12O6) per 100.0 mL of solution. Calculate the molarity of the solution.

A. 0.250 M

Correct B. 0.500 M

C. 0.750 M

D. 1.00 M

Correct Answer: B

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Question 19 View Details

The half-life of a radioactive subs\tance is 5.00 days. If 100.0 mg of the subs\tance initially exists, calculate the amount of the subs\tance remaining after 20.0 days.

A. 12.5 mg

Correct B. 25.0 mg

C. 37.5 mg

D. 50.0 mg

Correct Answer: B

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Question 20 View Details

A 2.00 L flask contains 0.150 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 2.00 atm.

A. 0.0100 mol

Correct B. 0.0200 mol

C. 0.0300 mol

D. 0.0400 mol

Correct Answer: B

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Question 21 View Details

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

Correct C. 500 K

D. 600 K

Correct Answer: C

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Question 22 View Details

A 2.00 L flask contains 0.150 mol of an ideal gas at 27°C. Calculate the volume of the flask in liters.

A. 1.00 L

Correct B. 2.00 L

C. 3.00 L

D. 4.00 L

Correct Answer: B

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Question 23 View Details

A 3.00 L flask contains 0.200 mol of an ideal gas at 37°C. Calculate the pressure of the gas in pascals.

A. 1.01 × 10^5 Pa

B. 2.02 × 10^5 Pa

Correct C. 3.03 × 10^5 Pa

D. 4.04 × 10^5 Pa

Correct Answer: C

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Question 24 View Details

A solution of $CuSO_4$ is electrolyzed u\sing a platinum electrode. The anode reaction is $Cu(s) \rightarrow Cu^{2+}(aq) + 2e^-$. If the cell potential is 2.5 V, calculate the number of moles of $Cu^{2+}$ ions released at the anode in 2 hours.

A. 0.25 mol

B. 0.5 mol

Correct C. 1.0 mol

D. 1.5 mol

Correct Answer: C

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Question 25 View Details

The solubility product cons\tant $ $K_{sp}$ $ of $CaF_2$ is $3.45 \times 10^{-11}$. Calculate the molar solubility of $CaF_2$ in a 0.1 M $Ca$ NO_3 $_2$ solution.

A. 1.0 × 10^{-5} M

B. 2.0 × 10^{-5} M

Correct C. 3.0 × 10^{-5} M

D. 4.0 × 10^{-5} M

Correct Answer: C

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