A process involves 1.0 kg of steam condensing to water at 100^∘ C. (a) The change in entropy of

step 1 So in this problem we are given the mass of water is equal to 1 .0 KG and the temperature of wat

A process involves 1.0 kg of steam condensing to water at...

A process involves $1.0 \mathrm{~kg}$ of steam condensing to water at $100^{\circ} \mathrm{C}$. (a) The change in entropy of the steam (water) is (1) positive, (2) zero, (3) negative. Why? (b) What is the change in entropy of the steam (water)?

Key Concepts

Isothermal Process

An isothermal process is one that occurs at a constant temperature. In such processes, any heat transfer is directly linked to changes in entropy via the formula ?S = Q/T. This concept is essential when analyzing phase changes that occur at a constant temperature, helping to quantify the entropy change during the transition.

Latent Heat

Latent heat is the heat energy per unit mass absorbed or released during a phase change without a change in temperature. In the context of condensation, the latent heat is released when steam condenses into water. This release of heat is associated with a decrease in entropy of the system, as the disorder decreases when gas molecules become liquid.

Entropy

Entropy is a thermodynamic state function that quantifies the degree of disorder or randomness in a system. It determines the direction of spontaneous processes and is intimately related to the dispersal of energy in thermal systems. Changes in entropy can be calculated using the relation ?S = Q/T for processes occurring at a constant temperature, making it crucial for analyzing phase changes and heat exchanges.

Phase Transition

A phase transition is the transformation of a substance from one state of matter to another, such as from gas to liquid. During such transitions, energy is absorbed or released as latent heat, yet the temperature remains constant. This process inherently affects the system's entropy because the molecular organization changes significantly between phases.

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