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:**
How much heat is absorbed in the process of making 0.793 mol of CF₄ from the following reaction?
\( \text{C (s) + 2 F}_2 \text{(g)} \rightarrow \text{CF}_4 \text{(g)} \quad \Delta H^\circ = 141.3 \, \text{kJ/mol} \)
**Explanation:**
This equation describes the formation of carbon tetrafluoride (CF₄) from carbon (C) and fluorine gas (F₂). The enthalpy change (ΔH°) for this reaction is 141.3 kJ per mole of CF₄ formed. To find out how much heat is absorbed for 0.793 moles, you multiply the enthalpy change by the number of moles:
\[
\text{Heat absorbed} = 0.793 \, \text{mol} \times 141.3 \, \text{kJ/mol} = 112.0599 \, \text{kJ}
\]
Thus, 112.06 kJ of heat is absorbed in the process.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F68e3e7e7-0be3-454d-bc7f-70ceaacfbf3f%2Fbdcc5ddb-7c88-4a2f-9a2e-fc393b0e6bfb%2Fvcej0s5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
How much heat is absorbed in the process of making 0.793 mol of CF₄ from the following reaction?
\( \text{C (s) + 2 F}_2 \text{(g)} \rightarrow \text{CF}_4 \text{(g)} \quad \Delta H^\circ = 141.3 \, \text{kJ/mol} \)
**Explanation:**
This equation describes the formation of carbon tetrafluoride (CF₄) from carbon (C) and fluorine gas (F₂). The enthalpy change (ΔH°) for this reaction is 141.3 kJ per mole of CF₄ formed. To find out how much heat is absorbed for 0.793 moles, you multiply the enthalpy change by the number of moles:
\[
\text{Heat absorbed} = 0.793 \, \text{mol} \times 141.3 \, \text{kJ/mol} = 112.0599 \, \text{kJ}
\]
Thus, 112.06 kJ of heat is absorbed in the process.
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