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CHEM102 Final Exam - General Chemistry II
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MCQS on the chemical principles and theories that are used in a variety of practical applications. Topics include chemical kinetics, solution chemistry, chemical equilibrium, acids, bases, and buffers, electrochemistry, nuclear chemistry, and an introduction to organic chemistry.

CHEM102 Final Exam - General Chemistry II
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25 Questions

1. Which of the following has the least number of C-O bonds?
2. Given the following two half reactions,
Cd2+(aq) + 2e- → Cd(s) E° = -0.40 V
2 Ag+(aq) + 2e- → 2 Ag(s) E° = 0.80 V
determine E° and the spontaneity of the following reaction:
2 Ag+(aq) + Cd(s) → 2 Ag(s) + Cd2+(aq)
3. H3PO4 is a stronger acid than NH4+. What is the direction of the equilibrium of the following reaction?
NH4+(aq) + H2PO4-(aq) → NH3(aq) + H3PO4(aq)
4. What is the correct balanced equation for the following oxidation-reduction reaction?
Cr2O72- + C2O42- → Cr3+ + CO2
5. A solution contains 0.0128 g of HCl in 450. mL of solution. What is the pH of this solution at 25 °C?
6. The voltaic cell Cd | Cd2+|| Ni2+ (1.0M)| Ni has an electromotive force of 0.240 V at 25 °C. What is the concentration of cadmium ion? (Please note that E° = 0.170 V.)
7. What is a Brønsted-Lowry base?
8. An important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. The pH of blood is 7.44. What is the pH of blood, if 25% of the hydrogen phosphate is converted to dihydrogen phosphate? The value of Ka for H2PO4- is 6.2 x 10-2.
9. Use the solubility rules. Which salt is insoluble in water?
10. Calculate the emf for a cell operating with the following reaction:
Cr2O72-(aq) + 6 I-(aq) + 14 H+(aq) → 2 Cr3+(aq) + 3 I2(s) + 7 H2O(l),
where [Cr2O72-] = 0.020 M, [I-] = 0.015 M, [Cr3+] = 0.20 M and [H+] = 0.50 M, using the following standard reduction potentials:
Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr3+(aq) + 7 H2O(l) E° = +1.33 V
I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V
11. At 10 °C, Kw = 2.9 x 10-15. What is [OH-] in neutral water at 10 °C?
12. Which type of radiation has the most penetrating ability?
13. Calculate the equilibrium constant K for the following reaction at 25 °C.
2 Fe3+(aq) + Cu(s) → 2 Fe2+(aq) + Cu2+(aq) E° = +0.43 V
14. Solution A contains 0.1 mol of sucrose, C12H22O11, dissolved in 500 g of water. Solution B contains 0.1 mol of sodium chloride, NaCl, in 500 g of water. Which of the following statements about these solutions is true?
15. Which of the following has the greatest number of C-O bonds?
16. A particular voltaic cell operates on the following reaction.
Zn(s) + Cl2(g) → Zn2+(aq) + 2 Cl-(aq)
Given an emf of 0.853 V, calculate the maximum electrical work generated when 20.0 g of zinc metal is consumed.

17. What is the name of the following molecule?
CH3-(CH2)7-CH3
18. Given the two following half reactions,
Sn2+(aq) + 2e- → Sn(s) E° = -0.14 V
Cu2+(aq) + 2e- → Cu(s) E° = +0.34 V
calculate the standard emf for the following reaction:
Sn(s) + Cu2+(aq) → Sn2+(aq) + Cu(s).
19. A certain reaction is zero order in reactant A and second order in reactant B.What happens to the reaction rate when the concentrations of both reactants are doubled?
20. What is the new concentration of a nitric acid made by diluting 50. mL of a 12.0 M solution to 250. mL?
21. Cadmium reacts spontaneously with copper(II) ion.
Cd(s) + Cu2+(aq) → Cd2+(aq) + Cu(s)
What are the half reactions for this reaction?
22. Teflon is an example of which of the following?
23. How can one prepare a 1.00 L of a 0.125 M H2SO4 solution?
24. What is the total concentration of ions in a 0.0360 M solution of Na3PO4?
25. If two molecules collide softly, what will most likely happen to the molecules?

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