POST UTME RHEMA UNIVERSITY 2018 Chemistry | Objective

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Question 1
A 2.5 g sample of a polymer was dissolved in 100 mL of a solvent. The solution was then titrated with 0.1 M HCl. The volume of HCl required to reach the equivalence point was 20 mL. Calculate the molar mass of the polymer.
A. 500
B. 1000
C. 1500
D. 2000
Question 2
A solution containing 0.10 M NaCl is prepared by dissolving 10 g of NaCl in 1 L of water. What is the concentration of the chloride ion in the solution?
A. 0.05 M
B. 0.10 M
C. 0.15 M
D. 0.20 M
Question 3
A 2.5 g sample of a non-metallic oxide was heated in a stream of hydrogen gas. The mass of the oxide was found to decrease by 1.5 g. Calculate the empirical formula of the oxide.
A. SO2
B. SO3
C. P2O5
D. P4O10
Question 4
The reaction of sodium with water is highly exothermic, producing hydrogen gas and sodium hydroxide. What is the balanced chemical equation for this reaction?
A. 2Na + 2H2O → 2NaOH + H2
B. 2Na + H2O → 2NaOH + H2
C. Na + H2O → NaOH + H2
D. 2Na + H2O → NaOH + 2H2
Question 5
A diagram of a chemical apparatus setup is shown below. What is the purpose of the apparatus?
A. To measure the volume of a liquid
B. To measure the mass of a solid
C. To separate a mixture of two subs\tances
D. To determine the concentration of a solution
Question 6
A 2.5 g sample of nitrogen gas is collected over water at a temperature of 25°C and a pressure of 1 atm. Calculate the volume of the nitrogen gas collected, assuming that the nitrogen gas behaves ideally.
A. 0.050 L
B. 0.100 L
C. 0.150 L
D. 0.200 L
Question 7
A 2.5 g sample of sodium chloride (NaCl) is dissolved in 100 mL of water. What is the concentration of the resulting solution in molarity?
A. 0.2 M
B. 0.43 M
C. 0.6 M
D. 0.8 M
Question 8
A 25 mL sample of a 0.1 M solution of NaOH is mixed with 25 mL of a 0.1 M solution of HCl. What is the pH of the resulting solution?
A. 7
B. 8
C. 9
D. 10
Question 9
The reaction between chlorine gas and sodium hydroxide solution is a classic example of a redox reaction. Write the balanced chemical equation for the reaction, including the state of each reac\tant and product.
A. 2NaOH(l) + Cl2(g) → NaCl(aq) + NaClO(aq) + H2O(l)
B. 2NaOH(l) + Cl2(g) → NaClO(aq) + NaCl(aq) + H2O(l)
C. 2NaOH(l) + Cl2(g) → NaClO3(aq) + NaCl(aq) + H2O(l)
D. 2NaOH(l) + Cl2(g) → NaCl(aq) + NaOH(aq) + H2O(l)
Question 10
A solution of 0.1 M NaOH was titrated with 0.1 M HCl. The pH of the solution at the equivalence point is 7. Calculate the pH of the solution at the half-equivalence point.
A. 6.5
B. 7.5
C. 8.5
D. 9.5
Question 11
Determine the number of moles of glu\cose (C6H12O6) produced from the complete oxidation of 2.5 g of ethane (C2H6) according to the equation: C2H6 + 7/4 O2 → 2C6H12O6 + 3H2O. The molar mass of glu\cose is 180 g/mol.
A. 0.023 mol
B. 0.038 mol
C. 0.025 mol
D. 0.042 mol
Question 12
The reaction of cyclohexane with bromine in the presence of light produces a mixture of 1,2-dibromocyclohexane and 1,4-dibromocyclohexane. What is the major product of this reaction?
A. 1,2-dibromocyclohexane
B. 1,4-dibromocyclohexane
C. cis-1,2-dibromocyclohexane
D. trans-1,4-dibromocyclohexane
Question 13
A diagram of a titration setup is shown below. What is the volume of the titrant (NaOH) required to reach the equivalence point?
A. 20 mL
B. 30 mL
C. 40 mL
D. 50 mL
Question 14
A 500 mL sample of a solution containing 0.20 M HCl is titrated with 0.10 M NaOH. What is the pH of the solution after the titration?
A. 1
B. 2
C. 3
D. 4
Question 15
A solution containing 0.1 M NH3 and 0.1 M NH4Cl is titrated with 0.1 M HCl. Calculate the pH of the solution after the addition of 50 mL of 0.1 M HCl.
A. 9.25
B. 9.50
C. 9.75
D. 10.00

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