Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Using Standard Heats of Formation to Calculate Enthalpy Change**
To find the standard enthalpy change (\(\Delta H^\circ_{\text{rxn}}\)) for the reaction:
\[
2\text{CO}_2(g) + 5\text{H}_2(g) \rightarrow \text{C}_2\text{H}_2(g) + 4\text{H}_2\text{O}(g)
\]
we use the following standard heats of formation (\(\Delta H^\circ_f\)):
- \(\Delta H^\circ_f(\text{CO}_2(g)) = -393.5 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{H}_2(g)) = 0.0 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{C}_2\text{H}_2(g)) = 226.7 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{H}_2\text{O}(g)) = -241.8 \, \text{kJ/mol}\)
**Calculate the standard enthalpy of the reaction:**
\[
\Delta H^\circ_{\text{rxn}} = \left( \sum \Delta H^\circ_f \text{(products)} \right) - \left( \sum \Delta H^\circ_f \text{(reactants)} \right)
\]
Using the above formula, determine the total \(\Delta H^\circ_{\text{rxn}}\).](https://content.bartleby.com/qna-images/question/4295bf62-da14-49f1-b3bf-6e678bc68de3/ca1f3f75-95a5-4803-bca5-9902b6583e01/d6j2ue_processed.jpeg)
Transcribed Image Text:**Using Standard Heats of Formation to Calculate Enthalpy Change**
To find the standard enthalpy change (\(\Delta H^\circ_{\text{rxn}}\)) for the reaction:
\[
2\text{CO}_2(g) + 5\text{H}_2(g) \rightarrow \text{C}_2\text{H}_2(g) + 4\text{H}_2\text{O}(g)
\]
we use the following standard heats of formation (\(\Delta H^\circ_f\)):
- \(\Delta H^\circ_f(\text{CO}_2(g)) = -393.5 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{H}_2(g)) = 0.0 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{C}_2\text{H}_2(g)) = 226.7 \, \text{kJ/mol}\)
- \(\Delta H^\circ_f(\text{H}_2\text{O}(g)) = -241.8 \, \text{kJ/mol}\)
**Calculate the standard enthalpy of the reaction:**
\[
\Delta H^\circ_{\text{rxn}} = \left( \sum \Delta H^\circ_f \text{(products)} \right) - \left( \sum \Delta H^\circ_f \text{(reactants)} \right)
\]
Using the above formula, determine the total \(\Delta H^\circ_{\text{rxn}}\).
![A scientist measures the standard enthalpy change for the following reaction to be -1122.6 kJ:
\[ 2\text{H}_2\text{S}(g) + 3\text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) + 2\text{SO}_2(g) \]
Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of \(\text{H}_2\text{S}(g)\) is ____ kJ/mol.
| Species | \(\Delta H_f^\circ\) (kJ/mol) |
|---------|---------------------------|
| \(\text{H}_2\text{O}(l)\) | -285.8 |
| \(\text{SO}_2(g)\) | -296.8 |
| \(\text{O}_2(g)\) | 0.0 |](https://content.bartleby.com/qna-images/question/4295bf62-da14-49f1-b3bf-6e678bc68de3/ca1f3f75-95a5-4803-bca5-9902b6583e01/vpqhkm_processed.jpeg)
Transcribed Image Text:A scientist measures the standard enthalpy change for the following reaction to be -1122.6 kJ:
\[ 2\text{H}_2\text{S}(g) + 3\text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) + 2\text{SO}_2(g) \]
Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of \(\text{H}_2\text{S}(g)\) is ____ kJ/mol.
| Species | \(\Delta H_f^\circ\) (kJ/mol) |
|---------|---------------------------|
| \(\text{H}_2\text{O}(l)\) | -285.8 |
| \(\text{SO}_2(g)\) | -296.8 |
| \(\text{O}_2(g)\) | 0.0 |
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