Enthalpy can be expressed in Joules, Calories, and Kilojoules.

Photosynthesis is an endothermic process as it absorbs energy from sunlight.

Volume is an extensive property, as it depends on the amount of substance present.

Entropy is a measure of disorder in a system, and it tends to increase in spontaneous processes.

Heat capacity depends on the amount of substance; it is not a constant value.

In an endothermic reaction, heat is absorbed, resulting in a positive ΔH.

Dissolving salt in water is a spontaneous process at standard conditions, resulting in a negative ΔG.

Photosynthesis is an endothermic process that requires energy, resulting in a positive ΔG.

Sublimation of dry ice (solid CO2) to gas increases disorder, resulting in a positive change in entropy.

Sublimation of dry ice (solid CO2) to gas increases entropy as the gas phase has higher disorder than the solid phase.

An isobaric process is characterized by constant pressure.

Dissolving salt in water is an endothermic process that increases the disorder of the system, thus increasing entropy.

Dissolving ammonium nitrate in water absorbs heat, making it an endothermic process.

The combustion of methane is an exothermic process, releasing heat.

Sublimation of solid iodine to gas involves a phase change from solid to gas, which has a significant increase in disorder, thus the largest increase in entropy.

Dissolving salt in water increases the number of particles in solution, leading to a significant increase in entropy.

Free expansion of gas is an irreversible process that leads to an increase in entropy as the gas expands into a vacuum.

Allowing a gas to expand slowly while maintaining constant temperature is an isothermal process.

A spontaneous process at constant temperature and pressure is characterized by an increase in entropy.

Isobaric heating increases the temperature and volume of the gas, leading to an increase in entropy.

Respiration is an exothermic reaction that releases energy, resulting in a negative enthalpy change.

The decomposition of hydrogen peroxide is non-spontaneous under standard conditions, resulting in a positive ΔG.

Sublimation of dry ice (solid CO2 to gas) has a positive ΔH (endothermic) and a positive ΔS (increase in disorder).

The combustion of propane releases a large amount of energy, resulting in the highest enthalpy change among the options.

The decomposition of liquid water into gaseous hydrogen and oxygen increases the number of gas molecules, leading to a positive change in entropy.

The combustion of hydrocarbons is highly exothermic and typically has a negative ΔG, indicating spontaneity.

A reaction with ΔH < 0 and ΔS > 0 is spontaneous at all temperatures because it results in a negative ΔG.

Endothermic reactions with positive ΔS can have a negative ΔG at high temperatures due to the TΔS term becoming significant.

The enthalpy change for a reaction at constant pressure is represented by ΔH.

Enthalpy is an extensive property, meaning it depends on the amount of substance present.