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HI is formed from the reaction of H, and I2, according to the following reaction. H2(g) + I(g) = 2HI(g) Part 1 out of 2 Use the following thermochemical data to calculate AG. for the formation of HI at 25 rin H2(g) I2g) HI(g) AH° (kJ/mol) 62.25 25.9 AS° (J/mol) 131 260.57 206.3 kJ AG rxn mol

HI is formed from the reaction of H, and I2, according to the following reaction. H2(g) + I(g) = 2HI(g) Part 1 out of 2 Use the following thermochemical data to calculate AG. for the formation of HI at 25 rin H2(g) I2g) HI(g) AH° (kJ/mol) 62.25 25.9 AS° (J/mol) 131 260.57 206.3 kJ AG rxn mol

Chemistry
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
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**Thermochemistry Calculation: Formation of HI** **Reaction Overview:** HI (hydrogen iodide) is formed from the reaction of H₂ (hydrogen gas) and I₂ (iodine gas) as shown in the equation: \[ \text{H}_2(g) + \text{I}_2(g) \rightarrow 2\text{HI}(g) \] **Part 1 out of 2:** Use the following thermochemical data to calculate \( \Delta G^\circ_{\text{rxn}} \) for the formation of HI at 25°C. **Thermochemical Data Table:** | | H₂(g) | I₂(g) | HI(g) | |----------------|-------|-------|--------| | \( \Delta H^\circ_f \) (kJ/mol) | 0 | 62.25 | 25.9 | | \( \Delta S^\circ_f \) (J/mol) | 131 | 260.57| 206.3 | **Calculation:** Calculate \( \Delta G^\circ_{\text{rxn}} \) using the formula: \[ \Delta G^\circ_{\text{rxn}} = \Delta H^\circ_{\text{rxn}} - T \Delta S^\circ_{\text{rxn}} \] *Note: Ensure to convert all values to consistent units before computing.* **Result:** \[ \Delta G^\circ_{\text{rxn}} = \text{[Insert calculated value]} \, \text{kJ/mol} \] Click "Next part" to proceed to the subsequent section. **Graph/Diagram Explanation:** There is no graph or diagram appearing with the given problem.
Transcribed Image Text:**Thermochemistry Calculation: Formation of HI** **Reaction Overview:** HI (hydrogen iodide) is formed from the reaction of H₂ (hydrogen gas) and I₂ (iodine gas) as shown in the equation: \[ \text{H}_2(g) + \text{I}_2(g) \rightarrow 2\text{HI}(g) \] **Part 1 out of 2:** Use the following thermochemical data to calculate \( \Delta G^\circ_{\text{rxn}} \) for the formation of HI at 25°C. **Thermochemical Data Table:** | | H₂(g) | I₂(g) | HI(g) | |----------------|-------|-------|--------| | \( \Delta H^\circ_f \) (kJ/mol) | 0 | 62.25 | 25.9 | | \( \Delta S^\circ_f \) (J/mol) | 131 | 260.57| 206.3 | **Calculation:** Calculate \( \Delta G^\circ_{\text{rxn}} \) using the formula: \[ \Delta G^\circ_{\text{rxn}} = \Delta H^\circ_{\text{rxn}} - T \Delta S^\circ_{\text{rxn}} \] *Note: Ensure to convert all values to consistent units before computing.* **Result:** \[ \Delta G^\circ_{\text{rxn}} = \text{[Insert calculated value]} \, \text{kJ/mol} \] Click "Next part" to proceed to the subsequent section. **Graph/Diagram Explanation:** There is no graph or diagram appearing with the given problem.
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