Homework Help is Here – Start Your Trial Now!
Science
Chemistry
How much heat is absorbed in the process of making 0.793 mol of CF from the following reaction? C(s) + 2 F₂ (g) → CF4 (g) AH° = 141.3 kJ/mol

How much heat is absorbed in the process of making 0.793 mol of CF from the following reaction? C(s) + 2 F₂ (g) → CF4 (g) AH° = 141.3 kJ/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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question

Give detailed Solution..don't give Handwritten answer 

**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.
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.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermodynamics
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS