Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
**Determining the Change in Entropy (ΔS) for Chemical Reactions** In thermodynamics, entropy (S) is a measure of the randomness or disorder of a system. The change in entropy (ΔS) of a reaction can be described as: - **ΔS > 0**: Indicates an increase in disorder. - **ΔS < 0**: Indicates a decrease in disorder. - **Too close to zero to decide**: Indicates that the change in disorder is negligible or not easily discernible. Below are several reactions for which we'll predict whether the entropy change (ΔS) will be greater than zero, less than zero, or too close to zero to decide. ### Reactions 1. **\( \mathrm{H_2(g) + Cl_2(g) \rightarrow 2HCl(g)} \)** 2. **\( \mathrm{PCl_5(g) \rightarrow PCl_3(g) + Cl_2(g)} \)** 3. **\( \mathrm{2HBr(g) + Cl_2(g) \rightarrow 2HCl(g) + Br_2(g)} \)** 4. **\( \mathrm{2H_2S(g) + 3O_2(g) \rightarrow 2H_2O(g) + 2SO_2(g)} \)** 5. **\( \mathrm{2H_2O_2(l) \rightarrow 2H_2O(l) + O_2(g)} \)** ### Categories for Entropy Change (ΔS) - **\( \Delta S > 0 \)**: The reaction leads to an increase in disorder. - **\( \Delta S < 0 \)**: The reaction leads to a decrease in disorder. - **Too close to zero to decide**: The change in disorder is minimal or uncertain. ### Analysis of Reactions 1. **\( \mathrm{H_2(g) + Cl_2(g) \rightarrow 2HCl(g)} \)** - Initially, we have two moles of gas (one mole of \( \mathrm{H_2} \) and one mole of \( \mathrm{Cl_2} \)). - The products are two moles of \( \mathrm{HCl} \) gas. - This suggests a similar level of disorder, but with new molecular interactions. -
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Transcribed Image Text:**Determining the Change in Entropy (ΔS) for Chemical Reactions** In thermodynamics, entropy (S) is a measure of the randomness or disorder of a system. The change in entropy (ΔS) of a reaction can be described as: - **ΔS > 0**: Indicates an increase in disorder. - **ΔS < 0**: Indicates a decrease in disorder. - **Too close to zero to decide**: Indicates that the change in disorder is negligible or not easily discernible. Below are several reactions for which we'll predict whether the entropy change (ΔS) will be greater than zero, less than zero, or too close to zero to decide. ### Reactions 1. **\( \mathrm{H_2(g) + Cl_2(g) \rightarrow 2HCl(g)} \)** 2. **\( \mathrm{PCl_5(g) \rightarrow PCl_3(g) + Cl_2(g)} \)** 3. **\( \mathrm{2HBr(g) + Cl_2(g) \rightarrow 2HCl(g) + Br_2(g)} \)** 4. **\( \mathrm{2H_2S(g) + 3O_2(g) \rightarrow 2H_2O(g) + 2SO_2(g)} \)** 5. **\( \mathrm{2H_2O_2(l) \rightarrow 2H_2O(l) + O_2(g)} \)** ### Categories for Entropy Change (ΔS) - **\( \Delta S > 0 \)**: The reaction leads to an increase in disorder. - **\( \Delta S < 0 \)**: The reaction leads to a decrease in disorder. - **Too close to zero to decide**: The change in disorder is minimal or uncertain. ### Analysis of Reactions 1. **\( \mathrm{H_2(g) + Cl_2(g) \rightarrow 2HCl(g)} \)** - Initially, we have two moles of gas (one mole of \( \mathrm{H_2} \) and one mole of \( \mathrm{Cl_2} \)). - The products are two moles of \( \mathrm{HCl} \) gas. - This suggests a similar level of disorder, but with new molecular interactions. -
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