Homework Help is Here – Start Your Trial Now!
Science
Chemistry
73./ Given, the following data (oo 30,(g) AH = -427 kJ 203(g) 0,(g) NO(g) + 0;(g) mi →20(g) AH = 495 kJ %3D NO,(g) + O,(g)(3) aH = -199 kJ / calculate AH for the reaction NO(g) + O(g) → NO,(g)

73./ Given, the following data (oo 30,(g) AH = -427 kJ 203(g) 0,(g) NO(g) + 0;(g) mi →20(g) AH = 495 kJ %3D NO,(g) + O,(g)(3) aH = -199 kJ / calculate AH for the reaction NO(g) + O(g) → NO,(g)

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

Can you help me on number 73. I don't like using fractions and I simply added equation 3 with equation 2

tgen I combine it with 1

and wanted to finish by then adding equation 3, but this leaves me with one extra  03. 

**Enthalpy Change Calculations** **72. Reaction Enthalpies** *Given Data:* 1. \(2 \text{ClF(g)} + \text{O}_2\text{(g)} \rightarrow \text{Cl}_2\text{O(g)} + \text{F}_2\text{O(g)}\) \(\Delta H = 167.4 \text{ kJ}\) 2. \(2 \text{ClF}_3\text{(g)} + 2\text{O}_2\text{(g)} \rightarrow \text{Cl}_2\text{O(g)} + 3\text{F}_2\text{O(g)}\) \(\Delta H = 341.4 \text{ kJ}\) 3. \(2 \text{F}_2\text{(g)} + \text{O}_2\text{(g)} \rightarrow 2\text{F}_2\text{O(g)}\) \(\Delta H = -43.4 \text{ kJ}\) **Calculate \(\Delta H\) for the reaction:** \(\text{ClF(g)} + \text{F}_2\text{O(g)} \rightarrow \text{ClF}_3\text{(g)}\) --- **73. Reaction Enthalpies** *Given Data:* 1. \(2\text{O}_3\text{(g)} \rightarrow 3\text{O}_2\text{(g)}\) \(\Delta H = -427 \text{ kJ}\) 2. \(\text{O}_2\text{(g)} \rightarrow 2\text{O(g)}\) \(\Delta H = 495 \text{ kJ}\) 3. \(\text{NO(g)} + \text{O}_3\text{(g)} \rightarrow \text{NO}_2\text{(g)} + \text{O}_2\text{(g)}\) \(\Delta H = -199 \text{ kJ}\) **Calculate \(\Delta H\) for the reaction:** \(\text{NO(g)} + \text{O(g)} \rightarrow \text{NO}_2\text
Transcribed Image Text:**Enthalpy Change Calculations** **72. Reaction Enthalpies** *Given Data:* 1. \(2 \text{ClF(g)} + \text{O}_2\text{(g)} \rightarrow \text{Cl}_2\text{O(g)} + \text{F}_2\text{O(g)}\) \(\Delta H = 167.4 \text{ kJ}\) 2. \(2 \text{ClF}_3\text{(g)} + 2\text{O}_2\text{(g)} \rightarrow \text{Cl}_2\text{O(g)} + 3\text{F}_2\text{O(g)}\) \(\Delta H = 341.4 \text{ kJ}\) 3. \(2 \text{F}_2\text{(g)} + \text{O}_2\text{(g)} \rightarrow 2\text{F}_2\text{O(g)}\) \(\Delta H = -43.4 \text{ kJ}\) **Calculate \(\Delta H\) for the reaction:** \(\text{ClF(g)} + \text{F}_2\text{O(g)} \rightarrow \text{ClF}_3\text{(g)}\) --- **73. Reaction Enthalpies** *Given Data:* 1. \(2\text{O}_3\text{(g)} \rightarrow 3\text{O}_2\text{(g)}\) \(\Delta H = -427 \text{ kJ}\) 2. \(\text{O}_2\text{(g)} \rightarrow 2\text{O(g)}\) \(\Delta H = 495 \text{ kJ}\) 3. \(\text{NO(g)} + \text{O}_3\text{(g)} \rightarrow \text{NO}_2\text{(g)} + \text{O}_2\text{(g)}\) \(\Delta H = -199 \text{ kJ}\) **Calculate \(\Delta H\) for the reaction:** \(\text{NO(g)} + \text{O(g)} \rightarrow \text{NO}_2\text
The image contains handwritten notes with chemical equations and steps for a reaction mechanism. Here's a transcription of the content: --- **Equation #77:** 1. NO(g) + O3(g) → NO2(g) + O2 - ΔH = -99 kJ/mol 2. 2 O → O2 - ΔH = -495 kJ/mol 3. (NO + O3 + 2 O) → (NO2 + 2 O3) - ΔH = -694 kJ/mol Combining these steps results in the overall reaction: \[ 3 NO + 3 O3 + 6 O → 3 NO2 + 6 O2 \] This leads to the production of: 4 O3 --- The notes demonstrate the step-by-step mechanism and enthalpy changes (ΔH) involved in the reaction between nitric oxide (NO) and ozone (O3). Each step involves intermediate species and energy changes, culminating in the overall balanced chemical equation.
Transcribed Image Text:The image contains handwritten notes with chemical equations and steps for a reaction mechanism. Here's a transcription of the content: --- **Equation #77:** 1. NO(g) + O3(g) → NO2(g) + O2 - ΔH = -99 kJ/mol 2. 2 O → O2 - ΔH = -495 kJ/mol 3. (NO + O3 + 2 O) → (NO2 + 2 O3) - ΔH = -694 kJ/mol Combining these steps results in the overall reaction: \[ 3 NO + 3 O3 + 6 O → 3 NO2 + 6 O2 \] This leads to the production of: 4 O3 --- The notes demonstrate the step-by-step mechanism and enthalpy changes (ΔH) involved in the reaction between nitric oxide (NO) and ozone (O3). Each step involves intermediate species and energy changes, culminating in the overall balanced chemical equation.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Concentration Terms
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
SEE MORE TEXTBOOKS