A chemist measures the energy change AH during the following reaction: 2 Fe, O3(s) 4 FeO(s)+O,(9) AH=560. kJ Use the information to answer the following questions. endothermic. This reaction is... exothermic. x10 Suppose 12.7 g of Fe, O, react. O Yes, absorbed. Yes, released. Will any heat be released or absorbed? O No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits.

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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**Transcription for Educational Website:**

---

A chemist measures the energy change \( \Delta H \) during the following reaction:

\[ 2 \text{Fe}_2\text{O}_3(s) \rightarrow 4 \text{FeO}(s) + \text{O}_2(g) \]

\[ \Delta H = 560. \text{ kJ} \]

Use the information to answer the following questions.

---

**This reaction is...**

- ◯ endothermic.
- ◯ exothermic.

---

**Suppose 12.7 g of Fe\(_2\)O\(_3\) react.**

**Will any heat be released or absorbed?**

- ◯ Yes, absorbed.
- ◯ Yes, released.
- ◯ No.

---

**If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed.**

Round your answer to **3 significant digits**.

\[\boxed{ \ \ \ }\] kJ

---

**Additional Explanation:**

- This text outlines a chemistry problem focused on determining the energy change during a reaction.
- The reaction involves iron(III) oxide (Fe\(_2\)O\(_3\)) and produces iron(II) oxide (FeO) and oxygen gas (O\(_2\)).
- The enthalpy change (\( \Delta H \)) is given as 560 kJ, indicating whether the reaction is endothermic or exothermic.
- Users are prompted to calculate the heat change based on the amount of Fe\(_2\)O\(_3\) that reacts (12.7 g) and determine the heat's direction (absorbed or released).
Transcribed Image Text:**Transcription for Educational Website:** --- A chemist measures the energy change \( \Delta H \) during the following reaction: \[ 2 \text{Fe}_2\text{O}_3(s) \rightarrow 4 \text{FeO}(s) + \text{O}_2(g) \] \[ \Delta H = 560. \text{ kJ} \] Use the information to answer the following questions. --- **This reaction is...** - ◯ endothermic. - ◯ exothermic. --- **Suppose 12.7 g of Fe\(_2\)O\(_3\) react.** **Will any heat be released or absorbed?** - ◯ Yes, absorbed. - ◯ Yes, released. - ◯ No. --- **If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed.** Round your answer to **3 significant digits**. \[\boxed{ \ \ \ }\] kJ --- **Additional Explanation:** - This text outlines a chemistry problem focused on determining the energy change during a reaction. - The reaction involves iron(III) oxide (Fe\(_2\)O\(_3\)) and produces iron(II) oxide (FeO) and oxygen gas (O\(_2\)). - The enthalpy change (\( \Delta H \)) is given as 560 kJ, indicating whether the reaction is endothermic or exothermic. - Users are prompted to calculate the heat change based on the amount of Fe\(_2\)O\(_3\) that reacts (12.7 g) and determine the heat's direction (absorbed or released).
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