A chemist measures the energy change ΔH during the following reaction:\[ \text{C}_3\text{H}_8(g) + 5\text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 4\text{H}_2\text{O}(l) \quad \Delta H = -2220 \, \text{kJ} \]Use the information to answer the following questions.| This reaction is... ||------------------------------------------------------------------------|| ☐ endothermic. || ☐ exothermic. || Suppose 95.4 g of $\text{C}_3\text{H}_8$ 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. ||------------------------------------------------------------------------|| Be sure your answer has the correct number of significant digits. || [_____ kJ] developed by the users.|Additionally, there is a checkbox interface for selecting options.Explanation of Graphs/Diagrams:- The image includes interactive elements, with checkboxes that users can select to indicate their answers regarding the nature of the reaction (endothermic or exothermic) and whether heat is absorbed or released.- A text box is provided for users to input their calculated answer regarding the amount of heat released or absorbed.

Answered: A chemist measures the energy change AH…

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 ΔH during the following reaction:

\[ \text{C}_3\text{H}_8(g) + 5\text{O}_2(g) \rightarrow 3\text{CO}_2(g) + 4\text{H}_2\text{O}(l) \quad \Delta H = -2220 \, \text{kJ} \]

Use the information to answer the following questions.

| This reaction is... |
|------------------------------------------------------------------------|
| ☐ endothermic. |
| ☐ exothermic. |

| Suppose 95.4 g of $\text{C}_3\text{H}_8$ 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. |
|------------------------------------------------------------------------|
| Be sure your answer has the correct number of significant digits. |
| [_____ kJ] developed by the users.|

Additionally, there is a checkbox interface for selecting options.

Explanation of Graphs/Diagrams:
- The image includes interactive elements, with checkboxes that users can select to indicate their answers regarding the nature of the reaction (endothermic or exothermic) and whether heat is absorbed or released.
- A text box is provided for users to input their calculated answer regarding the amount of heat released or absorbed.

Expert Solution

Step 1: Determine the enthalpy change for the reaction using given data:

$G i v e n comma T h e space b a l a n c e d space r e a c t i o n colon C subscript 3 H subscript 8 space left parenthesis g right parenthesis end subscript space plus space 5 space O subscript 2 space left parenthesis g right parenthesis end subscript space rightwards arrow space 3 space C O subscript 2 space left parenthesis g right parenthesis end subscript space plus space 4 space H subscript 2 O subscript left parenthesis l right parenthesis end subscript space space space increment H space equals space minus 2220. space k J$

mass of C₃H₈ = 95.4 g

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