**Thermochemistry: Using the General Properties of Reaction Enthalpy**A chemist measures the enthalpy change (ΔH) during the following reaction:\[ \text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow 2\text{CO}_2(g) + 2\text{C}_2\text{H}_5\text{OH}(l) \]\[ \Delta H = -69. \text{kJ} \]Use this information to complete the table below. Round each of your answers to the nearest kJ/mol.| Reaction | ΔH ||------------------------------------------------------------------------------------------------------|------------|| \( 4\text{CO}_2(g) + 4\text{C}_2\text{H}_5\text{OH}(l) \rightarrow 2\text{C}_6\text{H}_{12}\text{O}_6(s) \) | □ kJ || \( 4\text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow 8\text{CO}_2(g) + 8\text{C}_2\text{H}_5\text{OH}(l) \) | □ kJ || \( 2\text{CO}_2(g) + 2\text{C}_2\text{H}_5\text{OH}(l) \rightarrow \text{C}_6\text{H}_{12}\text{O}_6(s) \) | 69 kJ |Buttons: Explanation, Check**Explanation:**- The first reaction is the reverse of the given reaction, multiplied by 2. Therefore, ΔH should be \( +69 \text{ kJ} \times 2 = +138 \text{ kJ} \).- The second reaction is the given reaction, multiplied by 4. Thus, ΔH should be \( -69 \text{ kJ} \times 4 = -276 \text{ kJ} \).- The third reaction is already provided with its enthalpy change, confirming the value.

Answered: Image /qna-images/answer/887ea6bf-6a29-414b-a9b7-24ea304f202b.jpg

Answered: reaction AH 4CO, (g) + 4C,H,OH(1) →…

reaction AH 4CO, (g) + 4C,H,OH(1) → 2C,H,,0,(s) 2C,H,.0 H120;(s) O kJ 4C,H,,0,(s) 8CO, (g) + 8C, H,OH(1) O kJ 6 12 2' 2C0, (g) + 2C, H,OH() → C,H,,0,(s) 69. kJ 12 6

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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Question

**Thermochemistry: Using the General Properties of Reaction Enthalpy**

A chemist measures the enthalpy change (ΔH) during the following reaction:

\[ \text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow 2\text{CO}_2(g) + 2\text{C}_2\text{H}_5\text{OH}(l) \]

\[ \Delta H = -69. \text{kJ} \]

Use this information to complete the table below. Round each of your answers to the nearest kJ/mol.

| Reaction | ΔH |
|------------------------------------------------------------------------------------------------------|------------|
| \( 4\text{CO}_2(g) + 4\text{C}_2\text{H}_5\text{OH}(l) \rightarrow 2\text{C}_6\text{H}_{12}\text{O}_6(s) \) | □ kJ |
| \( 4\text{C}_6\text{H}_{12}\text{O}_6(s) \rightarrow 8\text{CO}_2(g) + 8\text{C}_2\text{H}_5\text{OH}(l) \) | □ kJ |
| \( 2\text{CO}_2(g) + 2\text{C}_2\text{H}_5\text{OH}(l) \rightarrow \text{C}_6\text{H}_{12}\text{O}_6(s) \) | 69 kJ |

Buttons: Explanation, Check

**Explanation:**

- The first reaction is the reverse of the given reaction, multiplied by 2. Therefore, ΔH should be \( +69 \text{ kJ} \times 2 = +138 \text{ kJ} \).
- The second reaction is the given reaction, multiplied by 4. Thus, ΔH should be \( -69 \text{ kJ} \times 4 = -276 \text{ kJ} \).
- The third reaction is already provided with its enthalpy change, confirming the value.

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