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Electrochemistry (Worksheet)

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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 \([Ni^{+2}] = 0.25\, M\).