Predict the sign of ΔS sys for each of the following processes: (b) Gaseous Cl 2 dissociates in the stratosphere to form gaseous Cl atoms.

Identify the type of process: The dissociation of Cl_{2} into Cl atoms is a decomposition reaction, where a single molecule breaks down into simpler substances.. Consider the molecular complexity before and after the reaction: Initially, there is one type of molecule, Cl_{2}. After the reaction, there are individual Cl atoms.. Analyze the change in the number of particles: The dissociation of Cl_{2} results in an increase in the number of gaseous particles. One Cl_{2} molecule produces two Cl atoms.. Relate the change in particle number to entropy: An increase in the number of gas particles generally leads to an increase in entropy ($$\Delta S \u003e 0) $$because there are more ways to arrange and distribute the energy among the particles.. Predict the sign of $$\Delta S_{\text{sys}}$$: Since the number of particles increases, the system's entropy likely increases, indicating that $$\Delta S_{\text{sys}} is $$positive.

Predict the sign of ΔSsys for each of the following processes: (b) Gaseous Cl2 dissociates in the stratosphere to form gaseous Cl atoms.

Identify the type of process: The dissociation of Cl_{2} into Cl atoms is a decomposition reaction, where a single molecule breaks down into simpler substances. Consider the molecular complexity before and after the reaction: Initially, there is one type of molecule, Cl_{2}. After the reaction, there are individual Cl atoms. Analyze the change in the number of particles: The dissociation of Cl_{2} results in an increase in the number of gaseous particles. One Cl_{2} molecule produces two Cl atoms. Relate the change in particle number to entropy: An increase in the number of gas particles generally leads to an increase in entropy ($$\Delta S \u003e 0) $$because there are more ways to arrange and distribute the energy among the particles. Predict the sign of $$\Delta S_{\text{sys}}$$: Since the number of particles increases, the system's entropy likely increases, indicating that $$\Delta S_{\text{sys}} is $$positive.

Ch.19 - Chemical Thermodynamics

Brown - Chemistry: The Central Science 15th Edition

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Ch.19 - Chemical Thermodynamics

Problema 42b

Capitolo 19, Problema 42b

Predict the sign of ΔS_sys for each of the following processes: (b) Gaseous Cl₂ dissociates in the stratosphere to form gaseous Cl atoms.

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Identify the type of process: The dissociation of Cl₂ into Cl atoms is a decomposition reaction, where a single molecule breaks down into simpler substances.

Consider the molecular complexity before and after the reaction: Initially, there is one type of molecule, Cl₂. After the reaction, there are individual Cl atoms.

Analyze the change in the number of particles: The dissociation of Cl₂ results in an increase in the number of gaseous particles. One Cl₂ molecule produces two Cl atoms.

Relate the change in particle number to entropy: An increase in the number of gas particles generally leads to an increase in entropy ($\Delta S > 0$) because there are more ways to arrange and distribute the energy among the particles.

Predict the sign of $\Delta S_{\text{sys}}$: Since the number of particles increases, the system's entropy likely increases, indicating that $\Delta S_{\text{sys}}$ is positive.

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Entropy (ΔS)

Entropy, denoted as ΔS, is a measure of the disorder or randomness in a system. In chemical processes, an increase in the number of gas molecules typically leads to an increase in entropy, as gases have higher disorder compared to solids or liquids. Understanding how changes in the state of matter affect entropy is crucial for predicting the sign of ΔS.

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Entropy in Thermodynamics

Dissociation of Gases

Dissociation refers to the process where a compound breaks down into its constituent atoms or simpler molecules. In the case of gaseous Cl2 dissociating into Cl atoms, the reaction increases the number of gaseous particles in the system. This increase in the number of particles generally contributes to a positive change in entropy (ΔS > 0).

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Percent Dissociation Example

System vs. Surroundings

In thermodynamics, it is essential to distinguish between the system (the part of the universe being studied) and the surroundings (everything else). The change in entropy of the system (ΔSsys) reflects the disorder within the system itself. For the dissociation of Cl2, the increase in gaseous Cl atoms signifies an increase in the system's entropy, leading to a positive ΔSsys.

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Entropy of Surroundings Formula

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