In this exercise, a reaction vessel is prepared with a mix of reactants and products under controlled conditions of 121.0 °C and constant pressure. The engineer measures the reaction enthalpy (ΔH) and reaction entropy (ΔS) for the first reaction, and the reaction enthalpy (ΔH) and reaction free energy (ΔG) for the second. The objective is to complete the table by calculating ΔG for the first reaction and ΔS for the second.**Reaction 1:**\[ \text{Sn(s) + 2CO}_2\text{(g) → SnO}_2\text{(s) + 2CO(g)} \]- ΔH = -12. kJ- ΔS = 32. J/K- ΔG = [blank] kJ **Spontaneity:**- This reaction- The reverse reaction- NeitherCalculate the Gibbs free energy change (ΔG) for the first reaction.**Reaction 2:**\[ \text{CH}_4\text{(g) + 2O}_2\text{(g) → CO}_2\text{(g) + 2H}_2\text{O(g)} \]- ΔH = -803. kJ- ΔS = [blank] J/K- ΔG = 0. kJ**Spontaneity:**- This reaction- The reverse reaction- NeitherCalculate the change in entropy (ΔS) for the second reaction.**Analysis Method:**- Use the Gibbs free energy equation: \[ ΔG = ΔH - TΔS \]- Temperature (T) must be converted to Kelvin. The calculations will help determine which reactions are spontaneous, considering the system may be at equilibrium.

Answered: Image /qna-images/answer/19eab36b-8a33-44de-9243-6e424445f26f.jpg

In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 121.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. Sn(s) + 2CO₂(g) SnO₂ (s) + 2CO (g) CH₂ (g) + 20₂ (g) → CO₂(g) + 2H₂O (8) AH = -12. kJ AS = 32. J K AG = kJ Which is spontaneous? Othis reaction AS = the reverse reaction Oneither AH-803. kJ J K AG= 0. kJ Which is spontaneous? Othis reaction the reverse reaction. neither X S

In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 121.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. Sn(s) + 2CO₂(g) SnO₂ (s) + 2CO (g) CH₂ (g) + 20₂ (g) → CO₂(g) + 2H₂O (8) AH = -12. kJ AS = 32. J K AG = kJ Which is spontaneous? Othis reaction AS = the reverse reaction Oneither AH-803. kJ J K AG= 0. kJ Which is spontaneous? Othis reaction the reverse reaction. neither X S

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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