A chemist measures the energy change AH during the following reaction: 2 H₂O(1)→ 2 H₂(g) + O₂(g) Use the information to answer the following questions. This reaction is... Suppose 89.7 g of H₂O react. Will any heat be released or absorbed? ΔΗ=572. kJ 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. Be sure your answer has the correct number of significant digits. endothermic. exothermic. O Yes, absorbed. O Yes, released. O No. X
A chemist measures the energy change AH during the following reaction: 2 H₂O(1)→ 2 H₂(g) + O₂(g) Use the information to answer the following questions. This reaction is... Suppose 89.7 g of H₂O react. Will any heat be released or absorbed? ΔΗ=572. kJ 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. Be sure your answer has the correct number of significant digits. endothermic. exothermic. O Yes, absorbed. O Yes, released. O No. X
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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![A chemist measures the energy change \( \Delta H \) during the following reaction:
\[ 2 \text{H}_2\text{O}(l) \rightarrow 2 \text{H}_2(g) + \text{O}_2(g) \quad \Delta H = 572. \text{ kJ} \]
Use the information to answer the following questions.
<table>
<tr>
<td>This reaction is...</td>
<td>
<input type="radio" name="reaction" value="endothermic"> endothermic.<br>
<input type="radio" name="reaction" value="exothermic"> exothermic.
</td>
</tr>
<tr>
<td>Suppose 89.7 g of \(\text{H}_2\text{O}\) react.</td>
</tr>
<tr>
<td>Will any heat be released or absorbed?</td>
<td>
<input type="radio" name="heat" value="absorbed"> Yes, absorbed.<br>
<input type="radio" name="heat" value="released"> Yes, released.<br>
<input type="radio" name="heat" value="no"> No.
</td>
</tr>
<tr>
<td colspan="2">
If you said heat <b>will</b> be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed.
</td>
</tr>
<tr>
<td colspan="2">Be sure your answer has the correct number of significant digits.</td>
</tr>
<tr>
<td colspan="2">
<input type="text" placeholder="kJ" style="width: 50px;">
</td>
</tr>
</table>
### Explanation:
- \(\Delta H = 572. \text{ kJ}\) indicates the enthalpy change for the reaction.
- The reaction involves liquid water (\(\text{H}_2\text{O}(l)\)) converting to gaseous hydrogen (\(\text{H}_2(g)\)) and oxygen (\(\text{O}_2(g)\)).
- The choices provided help determine if the reaction is endothermic (absorbing heat) or ex](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd11077d3-f0b7-424b-830f-d72f05e11bec%2F6d77f0da-ad95-43d5-8b97-17328bfb59a9%2Fethxlpe_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A chemist measures the energy change \( \Delta H \) during the following reaction:
\[ 2 \text{H}_2\text{O}(l) \rightarrow 2 \text{H}_2(g) + \text{O}_2(g) \quad \Delta H = 572. \text{ kJ} \]
Use the information to answer the following questions.
<table>
<tr>
<td>This reaction is...</td>
<td>
<input type="radio" name="reaction" value="endothermic"> endothermic.<br>
<input type="radio" name="reaction" value="exothermic"> exothermic.
</td>
</tr>
<tr>
<td>Suppose 89.7 g of \(\text{H}_2\text{O}\) react.</td>
</tr>
<tr>
<td>Will any heat be released or absorbed?</td>
<td>
<input type="radio" name="heat" value="absorbed"> Yes, absorbed.<br>
<input type="radio" name="heat" value="released"> Yes, released.<br>
<input type="radio" name="heat" value="no"> No.
</td>
</tr>
<tr>
<td colspan="2">
If you said heat <b>will</b> be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed.
</td>
</tr>
<tr>
<td colspan="2">Be sure your answer has the correct number of significant digits.</td>
</tr>
<tr>
<td colspan="2">
<input type="text" placeholder="kJ" style="width: 50px;">
</td>
</tr>
</table>
### Explanation:
- \(\Delta H = 572. \text{ kJ}\) indicates the enthalpy change for the reaction.
- The reaction involves liquid water (\(\text{H}_2\text{O}(l)\)) converting to gaseous hydrogen (\(\text{H}_2(g)\)) and oxygen (\(\text{O}_2(g)\)).
- The choices provided help determine if the reaction is endothermic (absorbing heat) or ex
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