The overall reaction in a commercial heat pack can be represented as:\[ 4 \text{Fe}(s) + 3 \text{O}_2(g) \rightarrow 2 \text{Fe}_2\text{O}_3(s) \quad \Delta H = -1652 \text{ kJ} \]**Questions:**a. How much heat is released when 4.80 moles of iron are reacted with excess \( \text{O}_2 \)? Heat = \[\underline{\hspace{2cm}}\] kJb. How much heat is released when 1.00 mole of \( \text{Fe}_2\text{O}_3 \) is produced? Heat = \[\underline{\hspace{2cm}}\] kJc. How much heat is released when 1.10 g of iron is reacted with excess \( \text{O}_2 \)? Heat = \[\underline{\hspace{2cm}}\] kJd. How much heat is released when 11.2 g \( \text{Fe} \) and 1.40 g \( \text{O}_2 \) are reacted? Heat = \[\underline{\hspace{2cm}}\] kJ**Instructions:**- Click "Submit Answer" to check your calculations.- Click "Try Another Version" for different values to practice with.- You have 3 item attempts remaining.

• Given, 4fe(s)+3O2(g)→2 fe2O3(s), ∆H=-1652 kJ• from the above equation we conclude Heat:-…

The overall reaction in a commercial heat pack can be represented as 4 Fe(s) + 302(g) → 2 Fe,O3 (s) AH=-1652 kJ a. How much heat is released when 4.80 moles of iron are reacted with excess O2? Heat = kJ b. How much heat is released when 1.00 mole of Fe2O3 is produced? Heat = kJ c. How much heat is released when 1.10 g iron is reacted with excess O2? Heat = kJ

The overall reaction in a commercial heat pack can be represented as 4 Fe(s) + 302(g) → 2 Fe,O3 (s) AH=-1652 kJ a. How much heat is released when 4.80 moles of iron are reacted with excess O2? Heat = kJ b. How much heat is released when 1.00 mole of Fe2O3 is produced? Heat = kJ c. How much heat is released when 1.10 g iron is reacted with excess O2? Heat = kJ

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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