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General Chemistry 2: Electrochemistry

Determine the oxidation state of S in Na2_2SO4_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?

Cr3+^{3+} + Pb \longrightarrow Cr + Pb2+^{2+}

Balance the redox reaction below

Sn + Ag+^+ \longrightarrow Sn2+{^2+} + Ag

The following reaction takes place under acidic conditions. Assign oxidation numbers and balance the oxidation reduction reaction using the half reaction method.

HNO3_3 + Fe2+^{2+} \longrightarrow Fe3+^{3+} + NO2_2

Balance the following redox reaction given acidic conditions, using the half reaction method.

S(s)+NO2+(aq)SO2(aq)+NO(g)S (s) + NO_2^+ (aq) \longrightarrow SO_2^- (aq) + NO (g) .

A voltaic cell is constructed using a Cd/Cd2+^{2+} half cell and a Sn2+^{2+}/Sn half cell. Write out the balanced equation, determine E^\circ, and calculate the cell potential at 25^\circC if [Cd2+^{2+}] = 0.50 M and [Sn2+^{2+}] = 0.30 M.

What is the standard free energy change, G\triangle G ^\circ for the following reaction at 25^\circ

Cu2+(aq)+Fe(s)Cu(s)+Fe2+(aq)Cu ^{2+} (aq) + Fe (s) \longrightarrow Cu (s) + Fe ^{2+} (aq)