What volume of $\mathrm { F } _ { 2 }$ gas, at $25 ^ { \circ } \mathrm { C }$ and 1.00 atm, is produced when molten KF is electrolyzed by a current of 10.0 A for 2.00 h? What mass of potassium metal is produced? At which electrode does each reaction occur?

What mass of each of the following substances can be produced in 1.0 h with a current of 15 A? Co from aqueous $\mathrm { Co } ^ { 2 + }$

What mass of each of the following substances can be produced in 1.0h with a current of 15A? Hf from aqueous $\mathrm { Hf } ^ { 4 + }$

Determine how the motion of an alpha particle is affected when it passes between a positively-charged electrode and a negatively charged electrode. How is the motion of a gamma ray affected?

If a lead storage battery is charged at too high a voltage, gases are produced at each electrode. (It is possible to recharge a lead-storage battery only because of the high overpotential for gas formation on the electrodes.)
(a) What are these gases?

Distinguish between *(a) voltammetry and amperometry. (b) linear-scan voltammetry and pulse voltammetry. *(c) differential-pulse voltammetry and square-wave voltammetry. (d) a rotating disk electrode and a ring-disk electrode. *(e) a limiting current and a diffusion current. (f) laminar flow and turbulent flow. *(g) the standard electrode potential and the halfwave potential for a reversible reaction at a working electrode. (h) stripping methods and standard voltammetry.

An active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode an anode or a cathode? Explain.

An aqueous solution of $\mathrm{Na}_2 \mathrm{~S}$ is placed in a beaker with two inert platinum electrodes. When the cell is attached to an external battery, electrolysis occurs.
Hydrogen gas and hydroxide ion form at the cathode. Write an equation for the half-reaction that occurs at this electrode.

Use electrode potentials to answer the following questions, assuming standard conditions. (a) Do you expect permanganate ion $\left(\mathrm{MnO}_4{ }^{-}\right)$to oxidize chloride ion to chlorine gas in acidic solution? (b) Will dichromate ion $\left(\mathrm{Cr}_2 \mathrm{O}_7^{2-}\right.$ ) oxidize chloride ion to chlorine gas in acidic solution?

An active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.

Use activities to calculate the electrode potential of a hydrogen electrode in which the electrolyte is $0.0100 \mathrm{M} \mathrm{HCl}$ and the activity of $\mathrm{H}_2$ is $1.00 \mathrm{~atm}$

What is the standard reduction potential of a standard hydrogen electrode?

In a Van de Graaff type generator a spherical metal shell is to be a $15 \times 10^6 \mathrm{~V}$ electrode. The dielectric strength of the gas surrounding the electrode is $5 \times 10^7 \mathrm{Vm}^{-1}$. What is the minimum radius of the spherical shell required? (You will learn from this exercise why one cannot build an electrostatic generator using a very small shell which requires a small charge to acquire a high potential.)

The masses of three electrodes (A, B, and C), each from three different galvanic cells, were measured before and after the cells were allowed to pass current for a while. The mass of electrode A increased, that of electrode B was unchanged, and that of electrode $\mathrm{C}$ decreased. Identify each electrode as active or inert, and note (if possible) whether it functioned as anode or cathode.