Calculate the standard enthalpy of formation of FeS2 (s) at 700. °C from the following data at 298.15 K. Assume that the heat capacities are independent of temperature. Fe(s) FeS2(s) Fe2O3 (s) S(rhombic) SO2(g) Substance AH: (kJ - mol-1) CP,m/R -824.2 - 296.81 3.02 7.48 2.72 You are also given that for the reaction 2FES2(s) + 02(g) Fe2 O3 (s) + 4SO2 (g), AH; -1655 kJ · mol-1.
Calculate the standard enthalpy of formation of FeS2 (s) at 700. °C from the following data at 298.15 K. Assume that the heat capacities are independent of temperature. Fe(s) FeS2(s) Fe2O3 (s) S(rhombic) SO2(g) Substance AH: (kJ - mol-1) CP,m/R -824.2 - 296.81 3.02 7.48 2.72 You are also given that for the reaction 2FES2(s) + 02(g) Fe2 O3 (s) + 4SO2 (g), AH; -1655 kJ · mol-1.
Chemistry
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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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Calculate the standard enthalpy of formation of FeS2(s)FeS2(s) at 700. ∘C from the following data at 298.15 KK. Assume that the heat capacities are independent of temperature.
![### Part A
**Objective:**
Calculate the standard enthalpy of formation of FeS₂ (s) at 700°C from the given data at 298.15 K. Assume that the heat capacities are independent of temperature.
**Data Table:**
| Substance | \( \Delta H_f^{\circ} \) (kJ·mol⁻¹) | \( \frac{C_{p,m}}{R} \) |
|-------------|-------------------------------------|-------------------------|
| Fe(s) | — | 3.02 |
| FeS₂(s) | -824.2 | 7.48 |
| Fe₂O₃(s) | — | — |
| S(rhombic) | — | 2.72 |
| SO₂(g) | -296.81 | — |
**Additional Information:**
For the reaction:
\[ 2 \text{FeS}_2(s) + \frac{11}{2} \text{O}_2(g) \rightarrow \text{Fe}_2\text{O}_3(s) + 4\text{SO}_2(g) \]
\(\Delta H_r^{\circ} = -1655 \text{ kJ·mol}^{-1}\)
**Instructions:**
Express your answer to four significant figures and include the appropriate units.
**Solution Box:**
\[ \Delta H_f^{\circ} = -181.34 \text{ kJ/mol} \]
**Feedback:**
❌ Incorrect; Try Again; 5 attempts remaining.
---
This problem involves the calculation of the enthalpy using given thermodynamic data and encourages accuracy by requiring four significant figures in the answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9269888f-6fb9-4d4f-8484-919fffe14161%2Fa4fbeb33-dc9a-42a5-83ae-ce2241bad75d%2F4bej5xc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Part A
**Objective:**
Calculate the standard enthalpy of formation of FeS₂ (s) at 700°C from the given data at 298.15 K. Assume that the heat capacities are independent of temperature.
**Data Table:**
| Substance | \( \Delta H_f^{\circ} \) (kJ·mol⁻¹) | \( \frac{C_{p,m}}{R} \) |
|-------------|-------------------------------------|-------------------------|
| Fe(s) | — | 3.02 |
| FeS₂(s) | -824.2 | 7.48 |
| Fe₂O₃(s) | — | — |
| S(rhombic) | — | 2.72 |
| SO₂(g) | -296.81 | — |
**Additional Information:**
For the reaction:
\[ 2 \text{FeS}_2(s) + \frac{11}{2} \text{O}_2(g) \rightarrow \text{Fe}_2\text{O}_3(s) + 4\text{SO}_2(g) \]
\(\Delta H_r^{\circ} = -1655 \text{ kJ·mol}^{-1}\)
**Instructions:**
Express your answer to four significant figures and include the appropriate units.
**Solution Box:**
\[ \Delta H_f^{\circ} = -181.34 \text{ kJ/mol} \]
**Feedback:**
❌ Incorrect; Try Again; 5 attempts remaining.
---
This problem involves the calculation of the enthalpy using given thermodynamic data and encourages accuracy by requiring four significant figures in the answer.
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