Question

Predict the sign of \(\Delta S\) for the following. (a) a lake freezing (b) precipitating lead chloride (c) a candle burning (d) weeding a garden

Short answer

Question: Predict the sign of the change in entropy (ΔS) for each of the following processes: (a) a lake freezing, (b) precipitating lead chloride, (c) a candle burning, and (d) weeding a garden. Answer: (a) ΔS is negative for a lake freezing, as the water molecules form a more ordered structure. (b) ΔS is negative for precipitating lead chloride, due to the formation of a more ordered solid precipitate. (c) ΔS is positive for a candle burning, as the system experiences an increase in disorder with the formation of gaseous products. (d) ΔS is negative for weeding a garden, as organizing the remaining plants reduces the disorder within the garden.

Step-by-step solution

(a) Predicting the sign of ΔS for a lake freezing.

As a lake freezes, the water molecules slow down and arrange themselves into a more ordered crystal lattice structure. This decrease in disorder means that ΔS will be negative for this process.

(b) Predicting the sign of ΔS for precipitating lead chloride.

In the precipitation of lead chloride, ions in an aqueous solution combine to form a solid precipitate with a more ordered structure. This leads to a decrease in disorder in the system, so ΔS will be negative for this process.

(c) Predicting the sign of ΔS for a candle burning.

Burning a candle involves the combustion of the wax, which is a hydrocarbon. During combustion, the hydrocarbon molecules react with oxygen to form carbon dioxide and water, which are released as gases. This transformation from solid wax and gaseous oxygen to gaseous carbon dioxide and water represents an increase in disorder in the system. Thus, ΔS will be positive for this process.

(d) Predicting the sign of ΔS for weeding a garden.

Weeding a garden involves removing unwanted plants and organizing the remaining plants. Although this process does not strictly involve a thermodynamic change, we can consider the change in disorder from an information perspective. By removing the weeds and organizing the remaining plants, one is reducing the disorder in the garden. Thus, ΔS will be negative for this process.

Key concepts

Thermodynamics and Entropy

Thermodynamics is a branch of physics that deals with heat, work, and energy. It helps us understand how energy changes form and the efficiency with which it is used. One key aspect of thermodynamics is entropy, often denoted by \( \Delta S \). Entropy measures the disorder or randomness in a system. A positive \( \Delta S \) indicates an increase in disorder, while a negative \( \Delta S \) implies a decrease.

• In thermodynamics, energy can neither be created nor destroyed.
• Processes occur spontaneously if they lead to an increase in the total entropy of a system.
• The Second Law of Thermodynamics states that the total entropy of an isolated system can never decrease over time.

Understanding how energy and entropy interact helps us predict how systems will behave under different conditions. Consider a lake freezing; here, entropy decreases as water transitions to a more ordered solid state.

Disorder in Chemical Processes

Disorder is a key concept when discussing entropy and thermodynamics. When a system's particles are more randomly arranged, the system has higher entropy. Thus, a decrease in disorder indicates a negative change in entropy.

• Disorder can be related to the freedom of movement of molecules.
• More disorder means particles are dispersed and moving more freely.
• An example of disorder decreasing is seen when a solution precipitates into a solid as in the formation of lead chloride.

In the case of lead chloride precipitation, ions are forming a structured solid, which implies that the system becomes more ordered and entropy decreases, indicating a negative \( \Delta S \). This process suggests a movement from a high disorder in a dissolved state to a low disorder in a solid form.

Phase Change and Entropy

Phase changes often involve significant changes in entropy since they involve a transformation in the molecular arrangement of a substance. When the phase of a substance changes, the disorder of its molecules can either increase or decrease.

• From solid to liquid: entropy increases as the system moves to a more disordered state.
• From liquid to solid: entropy decreases because molecules become more ordered.
• From liquid to gas: there is a large increase in disorder as molecules spread out and move freely.

Think about a candle burning. The wax melts and eventually combusts, transitioning from solid to liquid, then to gas. Here, entropy significantly increases, as solid wax becomes gaseous carbon dioxide and water, leading to a positive \( \Delta S \).

Combustion: Energy and Entropy

Combustion is a fascinating process that involves both energy release and changes in entropy. During combustion, a substance reacts typically with oxygen, and it forms new products with increased disorder.

• Combustion reactions transform chemical energy into heat and light.
• These reactions usually result in increased entropy due to the formation of gaseous products from solid fuels.
• A candle burning is an example where solid wax converts to gases with an increase in disorder.

In the combustion of candle wax, hydrocarbons react with oxygen from the air to produce carbon dioxide and water vapor. The transformation from solid wax and gaseous oxygen to gaseous products shows a clear rise in disorder, hence a positive \( \Delta S \), highlighting that combustion processes often lead to increased entropy.