Solve problems involving standard cell potentials

Which one of the following types of elements is most likely to be a good oxidizing agent?

 Using Table 20.1, which substance can oxidize I-(aq) to I2(s)?

The standard cell potential (Eecell) for the voltaic cell based on the reaction below is __________ V.

The standard cell potential (Eecell) for the voltaic cell based on the reaction below is __________ V.

3Sn4+ (aq) + 2Cr (s) -> 2Cr3+ (aq) + 3Sn2+ (aq)

Which of the following reactions will occur spontaneously as written?

What is cell potential?

Which statement about a voltaic cell is not correct?

Given the electrochemical reaction shown, if the standard reduction potential of Ag+ -> Ag is +0.80 V, and the standard reduction potential of Cu2+ -> Cu is +0.34V, what is E˚ for the following? 

Cu / Cu 2+(aq) // Ag+ (aq) / A E˚ = ??? V

Given the electrochemical reaction shown, if the standard reduction potential of Zn2+ -> Zn is –0.76 V, what is the standard reduction potential of Mg2+ -> Mg? 

Mg / Mg 2+(aq) // Zn2+(aq) / Zn E˚ = +1.61 V

Identify the strongest reducing agent based on the following half-reactions. The standard reduction potentials are listed.

+1.22 V MnO2(s) + 4H+ (aq) + 2e– → Mn2+(aq) + 2H2O(l)

+0.61 V Hg2SO4(s) + 2e– → 2Hg(l) + SO4 2– (aq)

–0.95 V SnO2(s) + 2H2O() + 4e– → Sn(s) + 4OH– (aq)

–1.48 V Cr(OH)3(s) + 3e– → Cr(s) + 3OH– (aq)

The gain of electrons by an element is called __________.

 __________ is reduced in the following reaction: 

______is the oxidizing agent in the reaction below:

The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a __________ process.

The half-reaction occurring at the anode in the balanced reaction shown below is __________