POST UTME RSU 2022 Chemistry | Objective

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Question 1
The rate cons\tant (k) of a first-order reaction is given by the equation: k = Ae^\( -Ea/RT \). If the activation energy (Ea) is 100 kJ/mol, the gas cons\tant (R) is 8.314 J/mol*K, and the temperature (T) is 300 K, calculate the value of k when A = 2.5 x 10^10 s^-1.
A. 1.2 x 10^7 s^-1
B. 2.5 x 10^10 s^-1
C. 3.2 x 10^8 s^-1
D. 4.1 x 10^9 s^-1
Question 2
A solution contains 0.2 M NaOH. What is the concentration of OH- ions?
A. 0.1
B. 0.2
C. 0.3
D. 0.4
Question 3
A solution contains 0.5 M NaCl. What is the concentration of Cl- ions?
A. 0.25
B. 0.5
C. 0.75
D. 1
Question 4
What is the oxidation number of chlorine in Cl2?
A. +1
B. +2
C. +3
D. +4
Question 5
The reaction of magnesium metal with hydrochloric acid is represented by the equation: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g). If 1.00 g of magnesium metal is added to 100.0 mL of 1.00 M hydrochloric acid solution, what is the volume of hydrogen gas produced?
A. 1.00 L
B. 2.00 L
C. 3.00 L
D. 4.00 L
Question 6
Determine the number of moles of electrons transferred in the electrolysis of 2.5 L of 0.5 M H2SO4.
A. 1.25 mol
B. 2.5 mol
C. 5.0 mol
D. 6.25 mol
Question 7
The diagram below shows a simple black and white chemistry apparatus showing a titration setup. What is the purpose of the pipette?
A. To measure the volume of the titrant
B. To measure the volume of the analyte
C. To mix the titrant and analyte
D. To measure the pH of the solution
Question 8
The diagram below shows a setup for a titration experiment.
A. The burette is used to measure the volume of the titrant.
B. The test tube is used to measure the volume of the titrant.
C. The burette is used to measure the volume of the analyte.
D. The test tube is used to measure the volume of the analyte.
Question 9
A sample of glu\cose (C6H12O6) is burned in a combustion calorimeter. What is the balanced equation for the reaction?
A. C6H12O6 + 6O2 → 6CO2 + 6H2O
B. C6H12O6 + 6H2O → 6CO2 + 12H2
C. C6H12O6 + 6CO2 → 6H2O + 12CO
D. C6H12O6 + 6H2O → 6CO + 12H2
Question 10
A 2.0 g sample of a metal hydroxide (MOH) is dissolved in water to produce a solution with a pH of 10.5. Calculate the molar mass of the metal (M).
A. 40 g/mol
B. 60 g/mol
C. 80 g/mol
D. 100 g/mol
Question 11
A 2.0 g sample of a metal carbonate (M2CO3) is heated to produce a metal oxide (MO). If the mass of the metal oxide produced is 1.2 g, calculate the molar mass of the metal (M).
A. 40 g/mol
B. 60 g/mol
C. 80 g/mol
D. 100 g/mol
Question 12
For the reaction 2NO(g) + O2(g) → 2NO2(g), the rate cons\tant (k) is 0.05 s^-1 at 298 K. Calculate the rate of reaction (r) when [NO] = 0.1 M, [O2] = 0.05 M, and the volume of the reaction mixture is 1 L.
A. 0.0025 M s^-1
B. 0.005 M s^-1
C. 0.01 M s^-1
D. 0.025 M s^-1
Question 13
A 1.0 L solution of 0.1 M H2SO4 is mixed with 1.0 L of 0.1 M NaOH. Calculate the number of moles of H2O produced.
A. 0.1 mol
B. 0.2 mol
C. 0.3 mol
D. 0.4 mol
Question 14
What is the molar mass of a compound containing 30% carbon and 70% oxygen by mass?
A. 30
B. 60
C. 90
D. 120
Question 15
A 0.1 M solution of HCl is titrated with 0.1 M NaOH. At the equivalence point, the pH of the solution is 7. Calculate the initial concentration of HCl if the initial concentration of NaOH is 0.1 M.
A. 0.05 M
B. 0.1 M
C. 0.15 M
D. 0.2 M

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