The entropy change for the mixing of two ideal gases at constant temperature is ΔS = nR ln(2) for equal moles of each gas.

The change in entropy at constant volume is given by ΔS = nC_v ln(T2/T1). For 1 mole, ΔS = R ln(T2/T1).

The change in entropy when heating an ideal gas at constant volume is given by ΔS = nC_v ln(T2/T1). For 1 mole, it simplifies to ΔS = R ln(T2/T1).

The phase change from ice to water at 0°C involves an increase in disorder, thus resulting in a positive change in entropy.

The change in entropy for an isothermal compression is ΔS = nR ln(V1/V2). For 2 moles, ΔS = 2R ln(V1/V2), which is negative since V1 < V2.

A higher entropy generally indicates a spontaneous process, as spontaneous processes tend to increase the overall disorder of the system.

Entropy generally increases with increasing temperature due to increased molecular motion and disorder.

The reaction decreases the number of gas molecules from 3 to 2, leading to a decrease in disorder and thus a negative ΔS°.

The reaction results in a decrease in the number of gas molecules (from 3 to 2), leading to a negative change in entropy.

The reaction decreases the number of gas molecules from 3 to 2, leading to a decrease in entropy.

Standard molar entropy is defined as the entropy of 1 mole of a substance at 25 °C and 1 atm pressure.

While temperature, volume, and the nature of the substance affect entropy, pressure does not directly affect the entropy of a system in a significant way.

Steam has the highest entropy at 25°C because it is in the gaseous state, which has more disorder compared to solid (ice) and liquid (water).

Water vapor has the highest entropy because gases have greater disorder compared to liquids and solids.

Water vapor has the highest entropy due to its gaseous state, which has more disorder compared to solids and liquids.

Water vapor at 100 °C has the highest entropy due to its gaseous state, which has more disorder compared to the liquid and solid states.

H2O(l) has a higher standard molar entropy than the diatomic gases due to its molecular complexity and interactions.

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.

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

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.

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.

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

Entropy is a state function, meaning it depends only on the state of the system and not on how it reached that state.