Chemistry & Chemical Reactivity
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ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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![### Calculating the Enthalpy of Reaction
**a. Calculate the enthalpy of reaction for:**
\[ 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \]
**b. If 18.5 grams of carbon dioxide are produced, what is the change in energy in kJ?**
---
**Explanation:**
To solve part (a), you will need the standard enthalpies of formation for the reactants and products involved in the reaction. The enthalpy change for the reaction \(\Delta H_{reaction}\) can be calculated using Hess's Law:
\[ \Delta H_{reaction} = \Sigma \Delta H_f \text{(products)} - \Sigma \Delta H_f \text{(reactants)} \]
For part (b), use the enthalpy change per mole from part (a) to calculate the energy change for 18.5 grams of \(\text{CO}_2\). First, convert the mass of \(\text{CO}_2\) to moles:
\[ \text{Molar Mass of } \text{CO}_2 = 44.01 \text{ g/mol} \]
\[ \text{Moles of } \text{CO}_2 = \frac{18.5 \text{ g}}{44.01 \text{ g/mol}} \]
Then, multiply the moles by the enthalpy change per mole obtained in part (a) to find the total energy change in kJ.](https://content.bartleby.com/qna-images/question/26d9d132-de79-44b4-9982-9bb4e4e01868/b9995966-cc41-4f6b-ac5d-39854826bc04/l1jtd78.jpeg)
Transcribed Image Text:### Calculating the Enthalpy of Reaction
**a. Calculate the enthalpy of reaction for:**
\[ 2 \text{CO}(g) + \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) \]
**b. If 18.5 grams of carbon dioxide are produced, what is the change in energy in kJ?**
---
**Explanation:**
To solve part (a), you will need the standard enthalpies of formation for the reactants and products involved in the reaction. The enthalpy change for the reaction \(\Delta H_{reaction}\) can be calculated using Hess's Law:
\[ \Delta H_{reaction} = \Sigma \Delta H_f \text{(products)} - \Sigma \Delta H_f \text{(reactants)} \]
For part (b), use the enthalpy change per mole from part (a) to calculate the energy change for 18.5 grams of \(\text{CO}_2\). First, convert the mass of \(\text{CO}_2\) to moles:
\[ \text{Molar Mass of } \text{CO}_2 = 44.01 \text{ g/mol} \]
\[ \text{Moles of } \text{CO}_2 = \frac{18.5 \text{ g}}{44.01 \text{ g/mol}} \]
Then, multiply the moles by the enthalpy change per mole obtained in part (a) to find the total energy change in kJ.
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