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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: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.104QE
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https://ezto.mheducation.com/ext/map/index.html?_con%3Dcon&external_browser3D0&launchUrl%=Dhttps%253A%2 Chapter 6 HW #2 Saved 2 attempts left Check my work Be sure to answer all parts. 1 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: points References 4 Fe(s) + 3 O2(g)→2 Fe,O3(s) AH =-1.65 × 103 kJ (a) What is the AH 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
Transcribed Image Text:https://ezto.mheducation.com/ext/map/index.html?_con%3Dcon&external_browser3D0&launchUrl%=Dhttps%253A%2 Chapter 6 HW #2 Saved 2 attempts left Check my work Be sure to answer all parts. 1 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: points References 4 Fe(s) + 3 O2(g)→2 Fe,O3(s) AH =-1.65 × 103 kJ (a) What is the AH 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
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