**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.### Reactions1. **\( \mathrm{H_2(g) + Cl_2(g) \rightarrow 2HCl(g)} \)**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 Reactions1. **\( \mathrm{H_2(g) + Cl_2(g) \rightarrow 2HCl(g)} \)** - 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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Predict whether AS for each reaction would be greater than zero, less than zero, or too close to zero to decide. Clear All H,(g) + C2(g)–→2HCI(g) PCI3(g)→PCl3g) + C2(2) AS>0 2HBr(g) + Ch(g) 2HCI(g) + Br2(g) AS<0 2H,S(g) + 30,(g)- 2H,0(g) + 2SO,(g) too close to decide 2H,021) 2H,0(1) + 02(g)

Predict whether AS for each reaction would be greater than zero, less than zero, or too close to zero to decide. Clear All H,(g) + C2(g)–→2HCI(g) PCI3(g)→PCl3g) + C2(2) AS>0 2HBr(g) + Ch(g) 2HCI(g) + Br2(g) AS<0 2H,S(g) + 30,(g)- 2H,0(g) + 2SO,(g) too close to decide 2H,021) 2H,0(1) + 02(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Predict whether AS for each reaction would be greater than zero, less than zero, or too close to zero to decide. I₂ (g) + Cl₂ (g) → 2IC1(g) COC1₂ (g) → CO(g) + Cl₂ (g) CH₂(g) +202 (g) → CO2(g) + 2H₂O(g) 4HC1(g) + O₂(g) → 2H₂O(g) + 2Cl₂ (9) 2H₂O2(1)→ 2H₂O(l) + O₂(g) Clear All AS >0 AS < 0 too close to decide
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4) Consider the reaction between liquid bromine and fluorine to produce BrF3 gas: Br2 (1) + 3 F2 (g) → 2 BrF3 (g) At 298.15 K, AGP of BrF3 (g) is -229.41 kJ/mol. a) Develop the direction predictor equation for the reaction: b) A flask contains liquid bromine, F2 gas with a partial pressure of Prz= 0.0060 bar and BFF3 gas with a partial pressure of PBIF3 = 1.996 bar. Which way will this reaction go? c) Describe what is happening here- in other words, explain how the two terms in dG either dx favor or go against spontaneity at this point in the reaction. What does the answer to this question say about how heavily favored reactants or products are in this reaction? d) Make a rough sketch of G vs x. Label the relevant features and indicate where the conditions of this problem are on the graph. e) What is the sign of AS? How do you know? What is the sign of AH? How do you know? f) A flask containing this reaction at equilibrium at 298 K has a partial pressure of BrF3 of 2.50 bar. What is…
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2 For the synthesis of ammonia where AG = -33.3 kJ/mole, determine whether the reaction is spontaneous at 25 C with the following pressures: PN, = 1.0 atm, PH, = 3.0 atm, PNH, = 0.020 atm N2(8) + 3H2(g) = 2NH3(g)
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Calculate the AS°rxn of the following reaction at 223°C and standard pressure. 1st attempt O See Hint C,H,(8) + 30,(g) . 200,(g) + 2H,0(g) AH°f, kJ/mol S°, J/mol K AG°F, kJ/mol C2H4(g) 52.3 219.5 68.1 O2(g) 205.0 CO2(g) -393.5 213.6 -394.4 H20(g) -241.8 188.7 -228.6 J/mol K
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