Which process is not an application of electrolysis?
a ) electroplating
b) cleaning toxic wastes
c ) separating metals from ores
d) creating synthetic diamonds

The electrolysis of aqueous $\mathrm{NaCl}$ gives $\mathrm{NaOH}, \mathrm{Cl}_2$, and $\mathrm{H}_2$.
Write a balanced equation for the process.

(a) Significant evolution or deposition occurs in electrolysis only. if the overpotential exceeds about 0.6 V. To illustrate this criterion calculate the effect that increasing the overpotential from 0.40 V to 0.60 V has on the current density in the electrolysis of 1.0 M NaOH(aq), which is $1.0\ \mathrm{mA}\ \mathrm{cm}^{-2}$ at 0.4 V and $25^{\circ} \mathrm{C}.$ Take $\alpha=0.5.$ (b) Calculate the effect that increasing the overpotential from 0.50 V to 0.60 V has on the current density in the electrolysis of 1.0 M NaOH(aq), which is $1.22\ \mathrm{mA}\ \mathrm{cm}^{-2}$ at 0.50 V and $25^{\circ} \mathrm{C}.$ Take $\alpha=0.50.$

Write equations for the following processes, noting appropriate conditions: (a) electrolysis of water; (b) electrolysis of molten LiH; (c) $\mathrm{CaH}_2$ reacting with water; (d) Mg treated with dilute nitric acid; (e) combustion of $\mathrm{H}_2$; (f) reaction of $\mathrm{H}_2$ with $\mathrm{CuO}$.

How many grams of oxygen are liberated by the electrolysis of water with a current of $0.0565 \mathrm{~A}$ after $1.85 \times 10^4 \mathrm{~s}$ ?

predict the probable products when $\mathrm{Pt}$ electrodes are used in the electrolysis of
(a) $\mathrm{CuCl}_2(\mathrm{aq})$;

Jewelry is often manufactured by plating an expensive metal such as gold over a cheaper metal. How might such a process be set up as an electrolysis reaction?

The first electrolytic process to produce sodium metal used molten NaOH as the electrolyte. Write probable half-equations and an overall equation for this electrolysis.

Which product, $\mathrm{Ca}$ or $\mathrm{H}_2$, is more likely to form at the cathode in the electrolysis of $\mathrm{CaCl}_2$? Explain your reasoning.

Magnesium is produced commercially by electrolysis of molten magnesium chloride.

Write the overall cell reaction and individual half-reactions.

Magnesium is produced commercially by electrolysis of molten magnesium chloride.

What precautions would need to be taken with respect to the magnesium formed?

In the electrolysis of an aqueous solution containing both $\mathrm{Cd}^{2+}$ and $\mathrm{Sn}^{2+}$, what product do we expect at the cathode?