Electrochemistry

Determine the oxidation state of S in Na\(_2\)SO\(_4\)
Assign oxidation numbers for the species below. Determine which species is the oxidizing agent and which is the reducing agent. Which species is being oxidized? Which species is being reduced?

Cr\(^{3+}\) + Pb \(\longrightarrow\) Cr + Pb\(^{2+}\)
Balance the redox reaction below

Sn + Ag\(^+\) \(\longrightarrow\) Sn\({^2+}\) + Ag
The following reaction takes place under acidic conditions. Assign oxidation numbers and balance the oxidation reduction reaction using the half reaction method.

HNO\(_3\) + Fe\(^{2+}\) \(\longrightarrow\) Fe\(^{3+}\) + NO\(_2\)
Balance the following redox reaction given acidic conditions, using the half reaction method.

S (s) +NO\(_2^+\) (aq) \(\longrightarrow\) SO\(_2^-\) (aq) + NO (g)
A voltaic cell is constructed using a Cd/Cd\(^{2+}\) half cell and a Sn\(^{2+}\)/Sn half cell. Write out the balanced equation, determine E\(^\circ\), and calculate the cell potential at 25\(^\circ\)C if [Cd\(^{2+}\)] = 0.50 M and [Sn\(^{2+}\)] = 0.30 M.
What is the standard free energy change, \(\triangle\)G\(^\circ\), for the following reaction at 25\(^\circ\)

Cu\(^{2+}\) (aq) + Fe (s) \(\longrightarrow\) Cu (s) + Fe\(^{2+}\) (aq)