Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe,O3) is: 4 Fe(s) + 3 02(g) → 2 Fe,O3(s) AH =-1.65 × 10³ kJ (a) What is the AHxn when 0.250 kg of iron rusts? x 10 kJ (b) How much rust forms when 9.40 x 10 kJ of heat is released? x 10 g Fe,O3
Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe,O3) is: 4 Fe(s) + 3 02(g) → 2 Fe,O3(s) AH =-1.65 × 10³ kJ (a) What is the AHxn when 0.250 kg of iron rusts? x 10 kJ (b) How much rust forms when 9.40 x 10 kJ of heat is released? x 10 g Fe,O3
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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![**Chapter 6 HW #2**
**Points: 1**
---
**Be sure to answer all parts.**
**Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe₂O₃) is:**
\[ 4 \text{Fe(s)} + 3 \text{O}_2\text{(g)} \rightarrow 2 \text{Fe}_2\text{O}_3\text{(s)} \]
\(\Delta H_{\text{rxn}} = -1.65 \times 10^3 \text{kJ}\)
**(a) What is the \(\Delta H_{\text{rxn}}\) when 0.250 kg of iron rusts?**
\[\boxed{\,} \times 10^{\,} \text{kJ}\]
**(b) How much rust forms when 9.40 × 10³ kJ of heat is released?**
\[\boxed{\,} \times 10^{\,} \text{g Fe}_2\text{O}_3\]
---
This exercise involves calculating the change in enthalpy (\(\Delta H\)) for a given amount of reactants and products in the chemical reaction provided, showing the transformation of iron and oxygen into rust.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F728e70e5-602c-40ad-8198-449db4e3e647%2F3d79edcf-9ff5-4296-8fa1-1796b279eb79%2Fu3fdyrr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chapter 6 HW #2**
**Points: 1**
---
**Be sure to answer all parts.**
**Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe₂O₃) is:**
\[ 4 \text{Fe(s)} + 3 \text{O}_2\text{(g)} \rightarrow 2 \text{Fe}_2\text{O}_3\text{(s)} \]
\(\Delta H_{\text{rxn}} = -1.65 \times 10^3 \text{kJ}\)
**(a) What is the \(\Delta H_{\text{rxn}}\) when 0.250 kg of iron rusts?**
\[\boxed{\,} \times 10^{\,} \text{kJ}\]
**(b) How much rust forms when 9.40 × 10³ kJ of heat is released?**
\[\boxed{\,} \times 10^{\,} \text{g Fe}_2\text{O}_3\]
---
This exercise involves calculating the change in enthalpy (\(\Delta H\)) for a given amount of reactants and products in the chemical reaction provided, showing the transformation of iron and oxygen into rust.
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