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Homework answers / question archive / University of Texas, Arlington COURSE TITLE: CHEM 1442 Chapter 18 Questions 3                                                                                                    4 1)In the following reaction, determine which element is the oxidizing agent and which element is oxidized

University of Texas, Arlington COURSE TITLE: CHEM 1442 Chapter 18 Questions 3                                                                                                    4 1)In the following reaction, determine which element is the oxidizing agent and which element is oxidized

Chemistry

University of Texas, Arlington

COURSE TITLE: CHEM 1442

Chapter 18 Questions

3                                                                                                    4
1)In the following reaction, determine which element is the oxidizing agent and which element is oxidized. XeF2 + BrO - + H2O ? Xe + 2 HF + BrO -
  1.  

4
Balance the following equation in acidic and then basic solution: MnO - + Fe2+ ? Mn2+ + Fe3+
  1. Which statement is correct? (a) the reducing agent is reduced in a reaction (b)                        the reducing agent may lose oxygen in the reaction (e) the reducing agent must                              not contain any oxygen.

 

  1. A species that has a strong affinity for gaining electrons would be: (a) oxidizing                 agent (b) reducing agent (c) easily oxidized (d) difficult to reduce (e) none

 

  1. Given the following half-cells below, what reaction occurs when the half-cells are suitably connected at standard conditions? Ti2+ + 2 e ? Ti Eo = -1.63 V

CdS + 2 e ? Cd + S2- Eo = -1.21 V

  1. Given the two half-cell reactions below, what will the standard EMF of the cell be when the half-cells are suitably connected at standard conditions? Is the reaction spontaneous?

Pd2+ + 2e ? Pd Eo = .99 V                          Ag+ + e ? Ag            Eo = 0.8 V

  1. Calculate E for the following cell: Fe + Sn2+ ? Fe2+ + Sn Useful Information: Fe2+ + 2e ? Fe E o = -0.44 V

Sn2+ + 2e ? Sn Eo = -0.14 V

[ Fe2+ ] = 0.5 M           [ Sn2+ ] = 0.001 M

  1. Eo for the reaction: 2 Mn3+ + 2 H2O ? Mn2+ + MnO2 + 4 H+ is 0.5 V. Calculate ?G for the process under standard conditions. ( F = 96,500C)
  2. A constant current of 10 amps was passed through a solution of NiCl2 for 10 minutes. How many grams of Ni metal plated out on the cathode?

 

  1.  

3                2                        2                  2
Eo for the process: NO - + H O + H ? NO - + 2 OH- + 2 H+ is

0.01 volts under standard conditions. What is the value of K?

 

  1. The relevant reduction potentials are: Ag+ + e ? Ag Eo = 0.8 V

Zn2+ + 2e ? Zn Eo = -0.76 V

Which of the following statements is False? (a) the silver electrode is the cathode (b) increasing the Zn2+ will increase the cell voltage (c) electrons in the external circuit will flow from Zn to Ag (d) Standard conditions prevail in the cell (e) Zn is the anode

 

 

  1. Solid nickel will spontaneously reduce which of the following?
    1. Fe2+      II. Zn2+      III. Pb2+         IV. Cu2+

a)I and II     b) III and IV c) II only d) I, III, and IV e) none

 

  1. Which of the following is the best oxidizing agent under standard conditions at 25°C?

 

a)      Cu2+(aq) b) I-(aq) c) Pb(s) d) Mg2+ (aq) e) Cd2+ (aq)

 

  1. Which of the following is the best reducing agent under standard conditions at 25°C?

 

a)      Cu2+(aq) b) I-(aq) c) Pb(s) d) Mg2+ e) Cd2+(aq)

 

  1. What is the appropriate cell notation for a galvanic cell utilizing the reaction below?

 

 

7

Cr2O 2–(aq) + 6Fe2+(aq) + 14H+(aq) ? 2Cr3+(aq) + 6Fe3+(aq) + 7H2O(l)

 

7

a)   Fe(s) | Fe2+(aq), Fe3+(aq) || Cr2O 2-(aq), Cr3+(aq) | Cr(s)

 

7

b) Cr(s) | Cr2O 2-(aq), Cr3+(aq) || Fe2+(aq), Fe3+(aq) | Fe(s)

 

7

c) Pt(s) | Cr2O 2-(aq), Cr3+(aq) || Fe2+(aq), Fe3+(aq) | Pt(s)

 

7

d) Pt(s) | Fe2+(aq) | Fe3+(aq) || Cr2O 2-(aq) | Cr3+(aq) | Pt(s)

 

7

e) Pt(s) | Fe2+(aq), Fe3+(aq) || Cr2O 2-(aq), Cr3+(aq) | Pt(s)

 

  1. What substances are produced at the anode and cathode when an aqueous solution of MgF2 is electrolyzed?

 

  1. F2(g) is produced at the anode, and Mg(s) is produced at the cathode.
  2. Mg(s) is produced at the anode, and F2(g) is produced at the cathode.
  3. F2(g) is produced at the anode, and H2(g) is produced at the cathode.
  4. O2(g) is produced at the anode, and Mg(s) is produced at the cathode.
  5. O2(g) is produced at the anode, and H2(g) is produced at the cathode.

 

  1. Electrolysis of a molten salt with the formula MCl, using a current of 3.86 A for 972 s, deposits 1.52 g of the metal. Identify the metal.

a)      Li b) Na c) K d) Rb e) Cs

 

Chapter 18 Useful information

 

?G = ?Go + RT lnQ                  Ecell = E oxidation + E reduction

 

 

cell

cell

?G = -nFE cell ( F = 96,500 C)                       logK = nEo          / 0.0592V Ecell = Eo                                       - 0.0592V/n log Q

it = nFe       i = amps        t= seconds n= moles an element

e= moles of electrons transferred in the reaction

 

 

 

Rules for Balancing Redox Reactions: (1) write the two half-reactions (2) Balance all elements except H and O (3) balance O with water (4) Balance H with H+ (5) balance charge with e- (6) multiply by a factor which will make the electrons equal in both half reactions (7) Combine like terms

If in basic solution only: Add a number of OH- to each side equal to the H+. On the side with the H+, the H+ + OH- ? H2O. Then recombine waters.

 

Rules for assigning oxidation numbers: (1) Group IA and II A are always +1 and +2 respectively. (2) F is always -1 (3) Give H a +1 ( it can be -1 if combines with group IA or II A)   (4) Give ) a -2 ( as a peroxide it can be -1) (5) elements by themselves have an oxidation number of 0.

 

 

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