E Question Completion Status: What is AH° (in kilojoules) for the reaction below? rxn CH 4(g) + 4 Cl 2(g) → CCI 4(1) + 4 HCI(g) CH 4(g) AH f° = -74.86 kJ/mol. CCI 4(1) AH f = -135.4 kJ/mol. HCI(g) AH f° = -92.31 kJ/mol. %3D

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...
icon
Related questions
icon
Concept explainers
Question
### Calculating the Standard Enthalpy Change of Reaction (ΔH°rxn)

The problem requires you to find the standard enthalpy change of reaction (ΔH°rxn) for the following chemical equation:

\[ \text{CH}_4(g) + 4 \text{Cl}_2(g) \rightleftharpoons \text{CCl}_4(l) + 4 \text{HCl}(g) \]

Below are the standard enthalpies of formation (\(ΔH_f°\)) for each substance involved:

- \(\text{CH}_4(g)\), \(ΔH_f° = -74.86 \, \text{kJ/mol}\)
- \(\text{CCl}_4(l)\), \(ΔH_f° = -135.4 \, \text{kJ/mol}\)
- \(\text{HCl}(g)\), \(ΔH_f° = -92.31 \, \text{kJ/mol}\)

### Explanation:
To calculate the \(ΔH°_{rxn}\), use the formula:

\[ ΔH°_{rxn} = \sum ΔH_f°(\text{products}) - \sum ΔH_f°(\text{reactants}) \]

This involves subtracting the total standard enthalpy of formation of the reactants from that of the products. Apply the formula to find the \(ΔH°_{rxn}\).
Transcribed Image Text:### Calculating the Standard Enthalpy Change of Reaction (ΔH°rxn) The problem requires you to find the standard enthalpy change of reaction (ΔH°rxn) for the following chemical equation: \[ \text{CH}_4(g) + 4 \text{Cl}_2(g) \rightleftharpoons \text{CCl}_4(l) + 4 \text{HCl}(g) \] Below are the standard enthalpies of formation (\(ΔH_f°\)) for each substance involved: - \(\text{CH}_4(g)\), \(ΔH_f° = -74.86 \, \text{kJ/mol}\) - \(\text{CCl}_4(l)\), \(ΔH_f° = -135.4 \, \text{kJ/mol}\) - \(\text{HCl}(g)\), \(ΔH_f° = -92.31 \, \text{kJ/mol}\) ### Explanation: To calculate the \(ΔH°_{rxn}\), use the formula: \[ ΔH°_{rxn} = \sum ΔH_f°(\text{products}) - \sum ΔH_f°(\text{reactants}) \] This involves subtracting the total standard enthalpy of formation of the reactants from that of the products. Apply the formula to find the \(ΔH°_{rxn}\).
Expert Solution
steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Knowledge Booster
Thermochemistry
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.
Similar questions
  • SEE MORE QUESTIONS
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