Applications of Thermodynamics

The addition of the catalyst might lead to greater buildup of intermediates reducing the rate of reaction

The catalyst could potentially decrease overall electrical resistance leading to faster charge flow

This could induce a change in the surface area for specific adsorption which can alter current density

This can increase the rate of reaction by providing an alternative pathway with lower activation energy

The amount of substance produced during electrolysis is always less than the stoichiometric amount.

The amount of substance produced during electrolysis is always greater than the stoichiometric amount.

The amount of substance produced during electrolysis is always equal to the stoichiometric amount.

The relationship between the amount of substance produced during electrolysis and the stoichiometry of the reaction depends on the specific reaction and the experimental conditions.

London dispersion forces in diethyl ether are weaker.

Dipole-dipole interactions in diethyl ether are more dominant.

Hydrogen bonding is stronger in ethylene glycol than in diethyl ether due to the presence of two -OH groups.

Dipole-dipole interactions in ethylene glycol are less significant.

Coulomb

Volt

Ohm

Ampere

Time elapsed

Number of electrons transferred

Battery size

Charge of ionic species

Different substances may be produced in amounts proportional to their equivalent weights and valences.

Only the identity of the substance determines the mass produced, independent of charge passed.

Mass production is directly related to charge with no variation between different substances.

All substances are produced in equal masses regardless of their chemical properties.

No significant change occurs as mass deposition rate depends primarily on current passed through the system not concentration.

Increased concentration leads directly proportional increase in mass deposition.

Decreased concentration increases resistance thereby reducing overall deposition rates.

Limited solute availability causes dramatic spike followed drop due saturation effects near electrode surfaces.

The current is directly proportional to the amount of product formed.

The relationship between the current and the amount of product formed depends on the specific reaction.

The current and the amount of product formed are not related.

The current is inversely proportional to the amount of product formed.

A charge double that needed for depositing 0.54 g of copper from a copper(II) nitrate solution.

Half the charge required for depositing 1 gram-equivalent mass of silver.

A charge exactly equal to the quantity of electricity that corresponds to one mole of electrons.

A charge equal to two times the quantity of electricity that corresponds to one mole of electrons.

The effect of increasing the concentration of the electrolyte on the rate of electrolysis depends on the specific electrolyte and the nature of the electrode materials.

Increasing the concentration of the electrolyte will always decrease the rate of electrolysis.

Increasing the concentration of the electrolyte will always increase the rate of electrolysis.

Increasing the concentration of the electrolyte has no effect on the rate of electrolysis.