A battery is assembled using tin and mercury, which have the following reduction half-reactions:

$$\begin{array}{l} \mathrm{Sn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn} \\ \mathrm{Hg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg} \end{array}$$

What is the cell potential?

A battery is assembled using tin and mercury, which have the following reduction half-reactions:

$$\begin{array}{l} \mathrm{Sn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn} \\ \mathrm{Hg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg} \end{array}$$

Write a balanced equation for the cell’s reaction.

Suppose in galvanization, copper was plated on iron instead of zinc. Would copper continue to protect the iron from corrosion, as zinc does, if the copper coating became broken or cracked? Explain.

Calculate the cell potential to determine if each of the following balanced redox reactions is spontaneous as written. $2 S O_{4}^{2-}(a q)+Co^{2+}(a q) \rightarrow C o(s)+S_{2} O_{8}^{2-}(a q)$

During electrolysis, an electrolytic cell releases bromine vapor and hydrogen gas. After electrolysis, the cell is found to contain a concentrated solution of potassium hydroxide. What was the composition of the cell before electrolysis began?

The potential of a half-cell varies with concentration of reactants and products. For this reason, standard potentials are measured at 1M concentration. Maintaining a pressure of 1 atm is especially important in half-cells that involve gases as reactants or products. Suggest a reason why gas pressure is critical in these cells.

Suppose that you have a voltaic cell in which one half-cell is made up of a strip of tin immersed in a solution of tin(II) ions. How could you tell by simple observation whether the tin strip was acting as a cathode or an anode?

Suppose that you have a voltaic cell in which one half-cell is made up of a strip of tin immersed in a solution of tin(II) ions. How could you tell by measuring voltage whether the tin strip was acting as a cathode or an anode in the cell?

Suppose that scientists had chosen the $C u^{2+} | Cu$ half-cell as a standard instead of the $H^+ | H_2$ half-cell? What would the potential of the hydrogen electrode be if the copper electrode were the standard? How would the relationships among the standard reduction potentials change?

Lead-acid batteries and other rechargeable batteries are sometimes called storage batteries. What is being stored in these batteries?

In the electrolytic refining of copper, what factor determines which piece of copper is the anode and which is the cathode?

Explain how the oxidation of hydrogen in a fuel cell differs from the oxidation of hydrogen when it burns in air.

The space shuttle uses a $H_2 / O_2$ fuel cell to produce electricity. What is the standard cell potential for the fuel cell?

The space shuttle uses a $H_2 / O_2$ fuel cell to produce electricity. What is the reaction at the anode? At the cathode?