Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Chemical Equation Balancing Exercise**
**Objective:** Balance the following chemical equation, if necessary.
**Equation:**
\[ \text{Li}_2\text{Se(s)} + \text{SO}_2\text{(g)} \rightarrow \text{SSe}_2\text{(g)} + \text{Li}_2\text{O(s)} \]
**Instructions:**
- Use the provided numerical keypad below the equation to input coefficients to balance the equation.
- Ensure that the same number of each type of atom appears on both sides of the reaction.
**Keypad:**
- The keypad includes numbers (0-9) and pre-set notations like SO₂, Li₂Se, SSe₂, and Li₂O for easy entry.
- Use the buttons to adjust coefficients, reset to start over, or delete to remove entries.
**Explanation and Analysis:**
- **Left Side:**
- Lithium Selenide (\(\text{Li}_2\text{Se}\)) is a solid.
- Sulfur Dioxide (\(\text{SO}_2\)) is in a gaseous state.
- **Right Side:**
- Selenium Disulfide (\(\text{SSe}_2\)) is produced as a gas.
- Lithium Oxide (\(\text{Li}_2\text{O}\)) appears as a solid.
**Tips for Balancing:**
1. Identify the number of atoms for each element on both sides.
2. Use coefficients to multiply the number of atoms as needed.
3. Balance one element at a time, starting with the most complex molecule.
4. Check that all elements are balanced with equal atoms on both sides.
**Example:**
If you start with 1 mole of \(\text{Li}_2\text{Se}\) and 1 mole of \(\text{SO}_2\), ensure that their product \(\text{SSe}_2\) and \(\text{Li}_2\text{O}\) reflect the same total number of atoms by applying the correct coefficients. Adjust as necessary.
Begin the balancing process using the online platform’s tools, and practice to enhance your understanding of chemical reactions and stoichiometry.](https://content.bartleby.com/qna-images/question/1a6ab37d-5853-4f5d-a5a4-203e58403879/1244c29d-ad26-468d-a0f9-579c3f40072d/8es2p94_processed.png)
Transcribed Image Text:**Chemical Equation Balancing Exercise**
**Objective:** Balance the following chemical equation, if necessary.
**Equation:**
\[ \text{Li}_2\text{Se(s)} + \text{SO}_2\text{(g)} \rightarrow \text{SSe}_2\text{(g)} + \text{Li}_2\text{O(s)} \]
**Instructions:**
- Use the provided numerical keypad below the equation to input coefficients to balance the equation.
- Ensure that the same number of each type of atom appears on both sides of the reaction.
**Keypad:**
- The keypad includes numbers (0-9) and pre-set notations like SO₂, Li₂Se, SSe₂, and Li₂O for easy entry.
- Use the buttons to adjust coefficients, reset to start over, or delete to remove entries.
**Explanation and Analysis:**
- **Left Side:**
- Lithium Selenide (\(\text{Li}_2\text{Se}\)) is a solid.
- Sulfur Dioxide (\(\text{SO}_2\)) is in a gaseous state.
- **Right Side:**
- Selenium Disulfide (\(\text{SSe}_2\)) is produced as a gas.
- Lithium Oxide (\(\text{Li}_2\text{O}\)) appears as a solid.
**Tips for Balancing:**
1. Identify the number of atoms for each element on both sides.
2. Use coefficients to multiply the number of atoms as needed.
3. Balance one element at a time, starting with the most complex molecule.
4. Check that all elements are balanced with equal atoms on both sides.
**Example:**
If you start with 1 mole of \(\text{Li}_2\text{Se}\) and 1 mole of \(\text{SO}_2\), ensure that their product \(\text{SSe}_2\) and \(\text{Li}_2\text{O}\) reflect the same total number of atoms by applying the correct coefficients. Adjust as necessary.
Begin the balancing process using the online platform’s tools, and practice to enhance your understanding of chemical reactions and stoichiometry.
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