Using standard heats of formation, calculate the standard enthalpy change for the following reaction. ΔΗ° rxn 2CO2 (g) + 5H2(g) → C₂H₂(g) + 4H₂O(g) AH (CO₂(g)) = -393.5 kJ/mol AH (H₂(g)) = 0.0 kJ/mol AH (C₂H₂ (9)) = 226.7 kJ/mol AH (H₂O(g)) kJ = - 241.8 kJ/mol

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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 \(\Delta H^\circ_{\text{rxn}}\).
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                       |
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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