issue 8 For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank. Na(s) + Br2(l) → NaBr(s)
issue 8
For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank.
Na(s) + Br2(l) → NaBr(s)
| Element | # oxy initial | # oxy final | e- lost or win | oxidized or reduced |
Oxidizing agent or Reducing agent |
|
| Na | → | |||||
| Br | → |
issue 13
Balance the reaction equation below using the half-reaction method.
Step 1: Write the two balanced half-reactions removing the spectator ions, if any.
Step 2: Balance the electrons.
Step 3: Add half-reactions by replacing spectator ions and/or recombining compounds.
Na + Br2 → NaBr
issue 14
Compare the two reactions below by calculating their potential difference. Which is a spontaneous reaction?
Use the table: Half-reaction potential.
2 Al(s) + 3 Zn2+(aq) → 2 Al3+(aq) + 3 Zn(s)
2 Al3+(aq) + 3 Cu(s) → 2 Al(s) + 3 Cu2+(aq)
issue 15
The reaction below takes place in a galvanic cell.
2 Fe(s) + 6H+(aq) → 2 Fe3+(aq) + 3 H2(g) E° = 0.04 V
You want to maximize the potential difference of the cell, but you can only replace one of the electrodes with another electrode. Therefore, the net reaction of the cell will need to be modified using a half reaction listed in Table 1.
a) Which would you choose?
b) Write the equation of the balanced reaction and the potential difference of this reaction.
c) Give the reason why it was necessary to use hydrogen as a standard to define the standard potential of half-reactions.
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