Applications of Thermodynamics

The cell potential increases.

The cell potential remains constant.

No reaction occurs as a result of the change in concentration.

The cell potential decreases.

Reaction direction reverses given a new pathway for reaction.

Increase - cell potential reaches equilibrium faster.

Decrease - decreased activation energy affects kinetics only.

No change occurs to either standard or non-standard cell potentials.

The standard EMF remains unchanged because equal reductions cancel each other out mathematically when calculating net EMF.

The relationship between half-cell potentials and standard EMFs requires kinetic data beyond mere concentration considerations.

The standard EMF decreases owing to diminished half-cell potentials limiting overall electron transfer efficiency.

The standard EMF would become negative indicating reversal of spontaneity direction for overall redox processes.

The reaction spontaneously stops at lower temperatures.

The cell potential decreases.

There is no effect on the cell potential.

The cell potential increases.

Pressure impacts only solid or liquid phase reactions, not gaseous reactants.

Increased pressure has no effect due to constant volume conditions in cells.

Increased pressure increases reactant concentration affecting potential via Le Chatelier’s Principle.

Decreased pressure uniformly lowers electron flow thus reducing potential.

The Nernst equation is not affected by changes in temperature.

An increase in temperature will always decrease the value of Q in the Nernst equation.

An increase in temperature will always increase the value of Q in the Nernst equation.

The effect of temperature on the value of Q in the Nernst equation depends on the specific reaction.

Coulombs (C)

Amperes (A)

Ohms (Ω)

Volts (V)

ΔG is zero, indicating that the system is at equilibrium.

The sign of ΔG cannot be determined without additional information.

ΔG is positive, indicating a non-spontaneous reaction.

ΔG is negative, indicating a spontaneous reaction.

The effect of temperature on the cell potential is negligible.

The effect of temperature on the cell potential depends on the specific reaction.

An increase in temperature will always decrease the cell potential.

An increase in temperature will always increase the cell potential.

Has no effect on standard cell potentials because they are measured at specific conditions (25°C).

Causes standard cell potential to vary widely depending on the exothermic or endothermic nature of reactions.

Decreases standard cell potential as heat may drive reaction in the opposite direction.

Increases standard cell potential due to higher kinetic energy of particles.