Applications of Thermodynamics

Molarity (M)

Normality (N)

Mass percent (%)

Molality (m)

The overall ΔG is averaged between two reactions leading to an intermediate value.

The overall ΔG becomes zero as both reactions neutralize each other's effects on free energy change.

The overall ΔG can become negative if coupled with a sufficiently exergonic reaction.

The overall ΔG remains positive since individual reactions preserve their own free energy changes.

Reversing the direction of the cell reaction.

Adding an inert electrolyte to increase the conductivity of the solution.

Decreasing temperature assuming that both enthalpy and entropy changes are positive.

Increasing the concentration of reactants and decreasing the concentration of products.

The additional He gas absorption lowers active participant concentrations indirectly speeding up atomic collisions necessary for promoting quicker reestablishment of altered states compared to the pre-intervention baselines accordingly overall.

Helium doesn't participate directly in chemical interactions nor impact total number particles, affecting neither volume nor partial pressures existing species present regardless overall pressure rise included along addition inert element itself inherently.

The presence of extra gas diversifies kinetic energies distributed among different types, altering the pathway activation needed to surpass energy barriers in transition phases effectively expediting any notable changes in equilibration pace generally expected under normal circumstances alike comparison to others of a similar nature that necessarily must be factored in the analysis perspective consideration.

Increasing the total number of molecules inside promotes expansion thus driving decomposition of HI favorably opposed to synthesis as suggested in the preceding context given the scenario to overcome otherwise stable standing arrangements outrightly.

The equilibrium shifts toward the reactants.

The rate of the reverse reaction decreases only.

The equilibrium shifts toward the products.

The equilibrium remains unchanged.

K decreases

K increases

There is no effect on K or ΔG.

ΔG decreases

Iodine (I2)

Carbon dioxide (CO2)

Water (H2O)

Oxygen gas (O2)

Spontaneity can only be determined by considering changes in enthalpy independently from entropy factors under these circumstances.

Spontaneity depends on pressure changes under standard conditions rather than temperature changes solely due to ΔS° being positive.

The reaction is nonspontaneous at all temperatures under standard conditions.

The reaction is spontaneous at all temperatures under standard conditions.

ΔG° = -RT ln Q at equilibrium.

The relationship between ΔG and Q depends on the specific reaction.

ΔG = ΔG° - RT ln Q at equilibrium.

ΔG = ΔG° + RT ln Q at equilibrium.

The relationship between ΔG and the temperature dependence of K depends on the specific reaction.

ΔG has no effect on the temperature dependence of K.

A positive ΔG indicates that K increases as temperature increases.

A negative ΔG indicates that K decreases as temperature increases.