bWhat is the enthalpy change if 3.1 g of chromium is oxidized to Cr₂O3(s)? AfH for Cr₂O3 (s) is -1134.7 kJ/mol Enthalpy change Submit Submit Answer kJ Try Another Version 10 item attempts remaining

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Balancing Chemical Equations and Calculating Enthalpy Change

**Question a:**
Write a balanced chemical equation for the formation of 1 mol of \( \text{Cr}_2\text{O}_3(s) \) from Cr and \( \text{O}_2 \) in their standard states.

> **Instructions:** Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.

**Balanced Equation:**
\[
2\text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)}
\]

**Status:** Correct

The equation of the formation of \( \text{Cr}_2\text{O}_3(s) \) from the elements:
\[
2 \text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)}
\]

---

**Question b:**
What is the enthalpy change if 3.1 g of chromium is oxidized to \( \text{Cr}_2\text{O}_3(s) \)?

> \(\Delta_f H^\circ\) for \( \text{Cr}_2\text{O}_3 \text{(s)} = -1134.7 \, \text{kJ/mol} \)

**Enthalpy Change:**
\[
\text{Enthalpy change} = \_\_\_ \, \text{kJ}
\]

**Options:**
- **Submit**
- **Submit Answer**
- **Try Another Version**
- **10 item attempts remaining**

*Controls:*
- Previous
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- Email Instructor
- Save and Exit

--- 

This exercise involves balancing a chemical reaction and calculating the enthalpy change based on the given data. Ensure to input your calculations accurately to determine the enthalpy change.
Transcribed Image Text:Sure! Below is a transcription of the image content suitable for an educational website: --- ### Balancing Chemical Equations and Calculating Enthalpy Change **Question a:** Write a balanced chemical equation for the formation of 1 mol of \( \text{Cr}_2\text{O}_3(s) \) from Cr and \( \text{O}_2 \) in their standard states. > **Instructions:** Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit. **Balanced Equation:** \[ 2\text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)} \] **Status:** Correct The equation of the formation of \( \text{Cr}_2\text{O}_3(s) \) from the elements: \[ 2 \text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)} \] --- **Question b:** What is the enthalpy change if 3.1 g of chromium is oxidized to \( \text{Cr}_2\text{O}_3(s) \)? > \(\Delta_f H^\circ\) for \( \text{Cr}_2\text{O}_3 \text{(s)} = -1134.7 \, \text{kJ/mol} \) **Enthalpy Change:** \[ \text{Enthalpy change} = \_\_\_ \, \text{kJ} \] **Options:** - **Submit** - **Submit Answer** - **Try Another Version** - **10 item attempts remaining** *Controls:* - Previous - Next - Email Instructor - Save and Exit --- This exercise involves balancing a chemical reaction and calculating the enthalpy change based on the given data. Ensure to input your calculations accurately to determine the enthalpy change.
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