POST UTME IMS U 2018 Chemistry | Objective

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Question 1
The diagram below shows a titration setup. If 25.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the concentration of the HCl solution?
A. \( 0.0500 , \text{M} \)
B. \( 0.100 , \text{M} \)
C. \( 0.200 , \text{M} \)
D. \( 0.500 , \text{M} \)
Question 2
A 1.00 M solution of sodium hydroxide (NaOH) is mixed with a 1.00 M solution of hydrochloric acid (HCl) in a 1.00 L flask. If the reaction is complete, and the resulting solution is 1.00 M in sodium chloride (NaCl), calculate the concentration of hydroxide ions \( OH^- \) in the resulting solution.
A. 0.50 M
B. 0.75 M
C. 1.00 M
D. 1.25 M
Question 3
A 100.0 mL sample of a solution containing 0.500 M HCl is titrated with 1.00 M NaOH. If the initial pH of the solution is 2.00, what is the volume of NaOH required to reach the equivalence point?
A. 50.0 mL
B. 75.0 mL
C. 100.0 mL
D. 125.0 mL
Question 4
A 0.1 M solution of a strong acid, HA, has a pH of 2.5. If 10 mL of 0.1 M NaOH is added to 100 mL of the acid solution, what is the pH of the resulting solution?
A. 3.5
B. 4.2
C. 5.5
D. 6.0
Question 5
The diagram below shows a circuit setup. If the current in the circuit is 2.00 A, what is the potential difference across the resistor?
A. \( 10.0 , \text{V} \)
B. \( 20.0 , \text{V} \)
C. \( 30.0 , \text{V} \)
D. \( 40.0 , \text{V} \)
Question 6
Determine the type of reaction that occurs when 1-bu\tanol is heated with a strong acid.
A. Synthesis reaction
B. Substitution reaction
C. Elimination reaction
D. Decomposition reaction
Question 7
A 2.00 M solution of H2SO4 is titrated with a 2.00 M solution of NaOH. Calculate the number of moles of H2SO4 that react with 25.0 mL of NaOH.
A. 0.0500 mol
B. 0.100 mol
C. 0.150 mol
D. 0.200 mol
Question 8
A sample of 1.00 g of a compound containing only carbon and hydrogen is combusted in a bomb calorimeter. The heat released is 12.5 kJ. What is the empirical formula of the compound?
A. \( CH_4 \)
B. \( C_2H_6 \)
C. \( C_3H_8 \)
D. \( C_4H_{10} \)
Question 9
A 2.0 g sample of a compound containing only carbon and hydrogen is analyzed by combustion. The volume of CO2 produced is 1.2 L at 25°C and 1 atm. The volume of H2 produced is 0.6 L at the same conditions. What is the empirical formula of the compound?
A. CH4
B. C2H6
C. C3H8
D. C4H10
Question 10
The s\tandard electrode potential of the zinc/zinc ion couple is -0.76 V. What is the s\tandard electrode potential of the zinc/silver couple?
A. -0.76 V
B. -0.76 V + 0.80 V
C. -0.76 V - 0.80 V
D. 0.80 V
Question 11
A sample of a non-metal has a mass of 10.0 g. If the density of the non-metal is 2.50 g/cm3, what is the volume of the non-metal?
A. 4.00 cm3
B. 6.00 cm3
C. 8.00 cm3
D. 10.0 cm3
Question 12
A 1.0 g sample of a compound containing only carbon and oxygen is analyzed by combustion. The volume of CO2 produced is 0.8 L at 25°C and 1 atm. The volume of H2O produced is 0.4 L at the same conditions. What is the empirical formula of the compound?
A. CO
B. C2O
C. C3O2
D. C4O3
Question 13
Sulfur dioxide (SO2) reacts with oxygen to form sulfur trioxide (SO3). Write a balanced equation for this reaction.
A. \( 2SO_2 + O_2 \rightarrow 2SO_3 \)
B. \( SO_2 + O_2 \rightarrow SO_3 \)
C. \( 2SO_2 + O_2 \rightarrow 2SO_3 \)
D. \( SO_2 + O_2 \rightarrow 2SO_3 \)
Question 14
Determine the structure of the compound C4H10O that results from the reaction of 2-methylpropane with water in the presence of sulfuric acid.
A. \( CH_3CH_2CH_2OH \)
B. \( CH_3CH\( OH \ \)CH_3 )
C. \( CH_3COCH_3 \)
D. \( CH_3CH_2CH\( OH \ \)CH_3 )
Question 15
A 2.00 g sample of a metal is heated in air to produce a metal oxide. If the mass of the metal oxide produced is 3.00 g, what is the percentage yield of the reaction?
A. 50%
B. 60%
C. 70%
D. 80%

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