Calculate the enthalpy change, A, H, for the formation of 1.00 mol of magnesium carbonate (also used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste) from its elements. Mg(s) + C(graphite) + 3/2 O₂(g) → MgCO₂ (s) The experimental information available is Mg(s) + 1/2O₂(g) → MgO(s) AH = -601 kJ/mol-rxn MgO(s) + CO₂(g) → MgCO₂ (s) A,H=-117 kJ/mol-rxn C(graphite) + O₂(g) → CO₂(g) AH* = -394 kJ/mol-rxn
Calculate the enthalpy change, A, H, for the formation of 1.00 mol of magnesium carbonate (also used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste) from its elements. Mg(s) + C(graphite) + 3/2 O₂(g) → MgCO₂ (s) The experimental information available is Mg(s) + 1/2O₂(g) → MgO(s) AH = -601 kJ/mol-rxn MgO(s) + CO₂(g) → MgCO₂ (s) A,H=-117 kJ/mol-rxn C(graphite) + O₂(g) → CO₂(g) AH* = -394 kJ/mol-rxn
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...
Related questions
Question
Calculate the enthalpy change, , for the formation of 1.00 mol of magnesium carbonate (also used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste) from its elements.
![This exercise involves calculating the enthalpy change, \(\Delta_{\text{r}}H^\circ\), for the formation of 1.00 mol of magnesium carbonate from its elements. Magnesium carbonate is commonly used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste.
The chemical reaction is:
\[ \text{Mg(s)} + \text{C(graphite)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{MgCO}_3 \text{(s)} \]
The experimental information provided includes:
1. \(\text{Mg(s)} + \frac{1}{2} \text{O}_2 \text{(g)} \rightarrow \text{MgO(s)}\)
\(\Delta_{\text{f}}H^\circ = -601 \text{ kJ/mol-rxn}\)
2. \(\text{MgO(s)} + \text{CO}_2 \text{(g)} \rightarrow \text{MgCO}_3 \text{(s)}\)
\(\Delta_{\text{r}}H^\circ = -117 \text{ kJ/mol-rxn}\)
3. \(\text{C(graphite)} + \text{O}_2 \text{(g)} \rightarrow \text{CO}_2 \text{(g)}\)
\(\Delta_{\text{f}}H^\circ = -394 \text{ kJ/mol-rxn}\)
Using these reactions, determine \(\Delta_{\text{r}}H^\circ\) for the target reaction and enter your answer in the provided field as \(\Delta_{\text{r}}H^\circ = \, \_ \_ \_\text{kJ/mol-rxn}\).
Click "Submit" when you have calculated the enthalpy change.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf41f395-6e79-4d96-8a7b-e72dcc99d382%2F5f2f82d0-c650-44b9-9356-f7082a26a1ff%2F5jxh598_processed.png&w=3840&q=75)
Transcribed Image Text:This exercise involves calculating the enthalpy change, \(\Delta_{\text{r}}H^\circ\), for the formation of 1.00 mol of magnesium carbonate from its elements. Magnesium carbonate is commonly used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste.
The chemical reaction is:
\[ \text{Mg(s)} + \text{C(graphite)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{MgCO}_3 \text{(s)} \]
The experimental information provided includes:
1. \(\text{Mg(s)} + \frac{1}{2} \text{O}_2 \text{(g)} \rightarrow \text{MgO(s)}\)
\(\Delta_{\text{f}}H^\circ = -601 \text{ kJ/mol-rxn}\)
2. \(\text{MgO(s)} + \text{CO}_2 \text{(g)} \rightarrow \text{MgCO}_3 \text{(s)}\)
\(\Delta_{\text{r}}H^\circ = -117 \text{ kJ/mol-rxn}\)
3. \(\text{C(graphite)} + \text{O}_2 \text{(g)} \rightarrow \text{CO}_2 \text{(g)}\)
\(\Delta_{\text{f}}H^\circ = -394 \text{ kJ/mol-rxn}\)
Using these reactions, determine \(\Delta_{\text{r}}H^\circ\) for the target reaction and enter your answer in the provided field as \(\Delta_{\text{r}}H^\circ = \, \_ \_ \_\text{kJ/mol-rxn}\).
Click "Submit" when you have calculated the enthalpy change.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 1 images
Knowledge Booster
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
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY