A chemical engineer is studying the two reactions shown in the table below.In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 56.0 °C and constant total pressure. Then, she measures the reaction enthalpy ΔH and reaction entropy ΔS of the first reaction, and the reaction enthalpy ΔH and reaction free energy ΔG of the second reaction. The results of her measurements are shown in the table.Complete the table. That is, calculate ΔG for the first reaction and ΔS 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.---**Table:**- Reaction: \( 2\text{H}_2\text{O}(g) \rightarrow 2\text{H}_2(g) + \text{O}_2(g) \)- \(\Delta H = 484. \text{ kJ}\)- \(\Delta S = 1446. \frac{\text{J}}{\text{K}}\)- \(\Delta G = \underline{\hspace{10mm}} \text{ kJ}\)***Which is spontaneous?***- [ ] this reaction- [ ] the reverse reaction- [ ] neither ### Chemical Reaction Representation and Thermodynamic Properties**Chemical Equation:**\[ 2\text{Al}(s) + 3\text{H}_2\text{O}(g) \rightarrow \text{Al}_2\text{O}_3(s) + 3\text{H}_2(g) \]This equation shows the reaction of aluminum in solid form with water vapor to produce aluminum oxide and hydrogen gas.**Thermodynamic Properties:**- **Enthalpy Change (\(\Delta H\))**: \[ \Delta H = -951. \, \text{kJ} \] This negative value indicates an exothermic reaction, meaning it releases heat.- **Entropy Change (\(\Delta S\))**: \[ \Delta S = \Box \, \frac{\text{J}}{\text{K}} \] The entropy change value is missing in the box and typically represents the degree of disorder or randomness in the system.- **Gibbs Free Energy Change (\(\Delta G\))**: \[ \Delta G = -28. \, \text{kJ} \] A negative Gibbs Free Energy value indicates that the reaction is spontaneous under standard conditions.**Spontaneity Question:**- The options given are: - O this reaction - O the reverse reaction - O neitherThe negative \(\Delta G\) suggests that "this reaction" is spontaneous.

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A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 56.0 °C and constant total pressure. Then, she 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 her 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. 2H₂O(g) → 2H₂(g) + O₂(g) ΔΗ = 484. kJ AS = 1446. AG = kJ J K Which is spontaneous? Othis reaction the reverse reaction neither X 6 ol E

A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 56.0 °C and constant total pressure. Then, she 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 her 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. 2H₂O(g) → 2H₂(g) + O₂(g) ΔΗ = 484. kJ AS = 1446. AG = kJ J K Which is spontaneous? Othis reaction the reverse reaction neither X 6 ol E

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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