# Electrochemistry (Worksheet)

Name: ______________________________

Section: _____________________________

Student ID#:__________________________

Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.

### Q1

Write the cell diagram for the $$Cu^{+2}$$/$$Cu$$ and $$Al^{+3}$$/$$Al$$ half-cells and calculate the $$E^{o}$$.

### Q2

Write the cell diagram and calculate the $$E^o$$ for the $$Zn$$/ $$Zn^{+2}$$ and $$Ca$$/$$Ca^{+2}$$ half-cells.

### Q3

1. Will $$I^-$$ react with $$Br_2$$?
2. Will $$Ni^{+2}$$ react with $$Br_2$$?
3. Will $$Ni$$ react with $$Br_2$$?
4. Will $$Co^{+2}$$ react with $$Br_2$$ to give $$Co^{+3}$$?

### Q4

Rank the following ions from strongest to weakest oxidizing agents:

$$Li^+$$ ; $$Al^{+3}$$ ; $$Ag^+$$ ; $$Pb^{+2}$$ ; $$Sr^{+2}$$

### Q5

Determine the $$E$$ for the $$Ag^+$$/$$Ag$$ and $$Sn^{+2}$$/$$Sn$$ half-cells if the $${[Ag^+]} = 1.0\, M$$ and the $${[Sn^{+2}]} = 0.25\, M$$.

### Q6

Is the reaction below spontaneous as written?  Calculate the $$E^o$$.

$Pb^{+2} + Cu \rightarrow Pb + Cu^{+2}$

### Q7

Determine the $$\Delta{G^o}$$ for the $$Ag^+$$/$$Ag$$ and $$Sn^{+2}$$/$$Sn$$ half-cells.

### Q8

Calculate $$\Delta G^o$$ for $$Cu^{+2}$$/$$Cu$$ and $$Mn^{+2}$$/$$Mn$$ half-cells. Is this reaction spontaneous?

### Q9

Calculate $$\Delta G$$ for $$Ni^{+2}$$/$$Ni$$ and $$Fe^{+2}$$/$$Fe$$ half-cells if the $$[Ni^{+2}] = 0.25\, M$$ and the $$[Fe^{+2}] = 0.50\, M$$.

### Q10

Determine the $$\Delta G$$ for the $$Al^{+3}$$/$$Al$$ and $$Ni^{+2}$$/$$Ni$$ half-cells if the $$[Al^{+3}] = 0.50\, M$$ and the $$[Ni^{+2}] = 0.25\, M$$.