Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Calculating Standard Enthalpy of Reaction (ΔH°_rxn)
#### Part A
**Problem Statement:**
What is \( \Delta H^\circ_\text{rxn} \) for the following chemical reaction?
\[ \text{H}_2\text{O}(l) + \text{CCl}_4(l) \rightarrow \text{COCl}_2(g) + 2\text{HCl}(g) \]
You can use the following table of standard heats of formation (\( \Delta H_f^\circ \)) to calculate the enthalpy of the given reaction.
#### Standard Heats of Formation Table
| Element/ Compound | Standard Heat of Formation (kJ/mol) | Element/ Compound | Standard Heat of Formation (kJ/mol) |
|-------------------|--------------------------------------|-------------------|--------------------------------------|
| H(g) | 218 | N(g) | 473 |
| H2(g) | 0 | O2(g) | 0 |
| CCl4(l) | -139.5 | O(g) | 249 |
| H2O(l) | -285.8 | HCl(g) | -92.30 |
| C(g) | 71 | COCl2(g) | -218.8 |
| C(s) | 0 | HNO3(aq) | -206.6 |
**Instructions:**
Express the standard enthalpy of reaction to three significant figures and include the appropriate units.
**Disclaimer:**
- The image above shows an interface where students can input their answers.
- Copyright © 2021 Pearson Education Inc. All rights reserved
**Hint:**
To calculate \( \Delta H^\circ_\text{rxn} \), use the formula:
\[ \Delta H^\circ_\text{rxn} = \sum \Delta H_f^\circ (\text{products}) - \sum \Delta H_f^\circ (\text{reactants}) \]
Use the provided standard heats of formation from the table to find the values for the reactants and products.](https://content.bartleby.com/qna-images/question/24ca723d-2dd5-46d5-9d14-7e20868efa99/ad001d80-ec55-43f8-86a1-4ee00ef629df/qs3kxmw_processed.jpeg)
Transcribed Image Text:### Calculating Standard Enthalpy of Reaction (ΔH°_rxn)
#### Part A
**Problem Statement:**
What is \( \Delta H^\circ_\text{rxn} \) for the following chemical reaction?
\[ \text{H}_2\text{O}(l) + \text{CCl}_4(l) \rightarrow \text{COCl}_2(g) + 2\text{HCl}(g) \]
You can use the following table of standard heats of formation (\( \Delta H_f^\circ \)) to calculate the enthalpy of the given reaction.
#### Standard Heats of Formation Table
| Element/ Compound | Standard Heat of Formation (kJ/mol) | Element/ Compound | Standard Heat of Formation (kJ/mol) |
|-------------------|--------------------------------------|-------------------|--------------------------------------|
| H(g) | 218 | N(g) | 473 |
| H2(g) | 0 | O2(g) | 0 |
| CCl4(l) | -139.5 | O(g) | 249 |
| H2O(l) | -285.8 | HCl(g) | -92.30 |
| C(g) | 71 | COCl2(g) | -218.8 |
| C(s) | 0 | HNO3(aq) | -206.6 |
**Instructions:**
Express the standard enthalpy of reaction to three significant figures and include the appropriate units.
**Disclaimer:**
- The image above shows an interface where students can input their answers.
- Copyright © 2021 Pearson Education Inc. All rights reserved
**Hint:**
To calculate \( \Delta H^\circ_\text{rxn} \), use the formula:
\[ \Delta H^\circ_\text{rxn} = \sum \Delta H_f^\circ (\text{products}) - \sum \Delta H_f^\circ (\text{reactants}) \]
Use the provided standard heats of formation from the table to find the values for the reactants and products.
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