POST UTME NILE UNIVERSITY 2017 Chemistry | Objective

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Question 1
A solution of $CH_3CH_2OH$ is 0.5 M. What is the concentration of $H^+$ ions in the solution?
A. 0.1 M
B. 0.2 M
C. 0.3 M
D. 0.4 M
Question 2
A diagram of a thermodynamic cycle is shown below. If the efficiency of the cycle is 40%, what is the work done by the system?
A. 100J
B. 200J
C. 300J
D. 400J
Question 3
A solution of $K_2Cr_2O_7$ in $H_2SO_4$ is used to oxidize $Fe^{2+}$ ions to $Fe^{3+}$ ions. The reaction is as follows: $K_2Cr_2O_7 + 7H_2SO_4 + 6FeSO_4 \rightarrow K_2SO_4 + 3Cr^3+ + 7H_2O + 6Fe^{3+} + 8SO_4^{2-}$.
A. Cr^3+
B. Fe^{3+}
C. SO_4^{2-}
D. H_2O
Question 4
The reaction between H2O2 and NaOH is represented by the equation: H2O2 + 2NaOH → Na2O2 + 2H2O. What is the limiting reac\tant if 25.0 mL of 0.100 M H2O2 is mixed with 25.0 mL of 0.100 M NaOH?
A. H2O2
B. NaOH
C. Na2O2
D. H2O
Question 5
The reaction between CH4 and O2 is represented by the equation: CH4 + 2O2 → CO2 + 2H2O. What is the limiting reac\tant if 25.0 mL of 0.100 M CH4 is mixed with 25.0 mL of 0.100 M O2?
A. CH4
B. O2
C. CO2
D. H2O
Question 6
A 50 mL sample of a solution containing 0.1 M HCl is titrated with 0.1 M NaOH. Calculate the pH of the solution at the equivalence point.
A. 1
B. 2
C. 3
D. 4
Question 7
A solution of a non-electrolyte solute in water is 0.5 M. What is the expected freezing point of the solution?
A. 0.5°C
B. 1.0°C
C. 1.5°C
D. 2.0°C
Question 8
A 25.0 mL sample of 0.100 M HCl is titrated with 0.0500 M NaOH. Calculate the pH of the solution after 15.0 mL of NaOH has been added.
A. 2.00
B. 2.50
C. 3.00
D. 3.50
Question 9
A metal alloy is composed of 80% copper and 20% zinc. If 100g of the alloy is heated to 1000°C, what is the maximum temperature that the copper can reach?
A. 900°C
B. 950°C
C. 1000°C
D. 1050°C
Question 10
A 10.0 g sample of sulfur is burned in oxygen to produce sulfur dioxide. Calculate the volume of oxygen gas consumed at STP.
A. 2.00 L
B. 4.00 L
C. 6.00 L
D. 8.00 L
Question 11
A sample of nitrogen gas occupies a volume of 2.50 L at a pressure of 1.00 atm and a temperature of 298 K. Calculate the number of moles of nitrogen gas present.
A. 0.0100 mol
B. 0.0200 mol
C. 0.0300 mol
D. 0.0400 mol
Question 12
Determine the number of moles of ΔH2O produced when 2.5 g of H2SO4 reacts with an excess of NaOH in the following reaction: H2SO4 + 2NaOH → Na2SO4 + ΔH2O. The molar mass of H2SO4 is 98.08 g/mol.
A. 0.025 mol
B. 0.050 mol
C. 0.075 mol
D. 0.100 mol
Question 13
A diagram of a titration setup is shown below. If 25mL of 0.1M HCl is added to 25mL of 0.1M NaOH, what is the pH of the resulting solution?
A. 7
B. 8
C. 9
D. 10
Question 14
A 0.1 M solution of a weak acid HA has a pH of 4.5. Calculate the concentration of the conjugate base A-.
A. 0.01 M
B. 0.1 M
C. 1 M
D. 10 M
Question 15
A solution of 0.1M NaCl is prepared by dissolving 6.0g of NaCl in 100g of water. What is the concentration of the solution in mol/L?
A. 0.1M
B. 0.2M
C. 0.3M
D. 0.4M

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