A photographer was on a trip to an exotic place to capture stunning landscapes when the electrical system of his RV was knocked out. He tried to locate himself on the road using the maps app on his tablet but the tablet's battery was dead. In his RV, he found safety matches that he could use to make a 1.0 M KClO₃ solution. He bought his RV from an old photographer, so he was able to find a small amount of silver nitrate (AgNO₃) and made a 1.0 M solution. He was wearing a silver ring and had a \$100 American Platinum Eagle coin in his pocket. He used a paper towel dipped in salt solution as a salt bridge.
The battery in the tablet requires 5.0 V for charging. Can this battery charge his tablet?

A certain voltaic cell has a standard cell potential of 2.516 V and is given by the following overall reaction: AuBr₄^–(aq) + Al(s) → Au(s) + 4 Br^–(aq) + Al³⁺(aq). If the E°_red of Al is –1.662 V, determine the E°_red for the reaction associated with Au.

Which of the following images shows the correct electrolytic cell with labeled anode and cathode and indicated electron flow direction where Co is oxidized to Co²⁺ and Ni²⁺ is reduced to Ni? What are the half-reactions at the anode and the cathode? How much voltage is needed to run the reaction?

At 25°C, which of the following pairs would you predict to react spontaneously? 

Ba²⁺(aq) + 2e^- → Ba(s)                 E° = -2.90 V

Sn⁴⁺(aq) + 2e^- → Sn²⁺(aq)           E° = 0.15 V

Mg²⁺(aq) + 2e^- → Mg(s)               E° = -2.37 V

Zn²⁺(aq) + 2e^- → Zn(s)                 E° = -0.73 V

Na⁺(aq) + e^- → Na(s)                    E° = -2.71 V

Fe³⁺(aq) + 3e^- → Fe(s)                 E° = -0.036 V

Cr³⁺(aq) + 3e^- → Cr(s)                  E° = -0.73 V

Ni²⁺(aq) + 2e^- → Ni(s)                  E° = -0.23 V