A app.101edu.co E Apps M Gmail O YouTube A Maps 1 VitalSource Books. Question 1 of 24 Submit Balance the following chemical equation (if necessary): Li:Se(s) + SO:(g) → SSe:(g) + Li:O(s) D2+ 04+ 1 2 3 4 6. 7 8. D4 Os Os Do (s) (1) (g) (aq) SO2 LizSe SSe2 Li2O Reset • x H2O Delete a fishes lab.pdf a Early Chrodates La..pdf Show all (0)
A app.101edu.co E Apps M Gmail O YouTube A Maps 1 VitalSource Books. Question 1 of 24 Submit Balance the following chemical equation (if necessary): Li:Se(s) + SO:(g) → SSe:(g) + Li:O(s) D2+ 04+ 1 2 3 4 6. 7 8. D4 Os Os Do (s) (1) (g) (aq) SO2 LizSe SSe2 Li2O Reset • x H2O Delete a fishes lab.pdf a Early Chrodates La..pdf Show all (0)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Concept explainers
Reactions of Ethers
Ethers (R-O-R’) are compounds formed by replacing hydrogen atoms of an alcohol (R-OH compound) or a phenol (C6H5OH) by an aryl/ acyl group (functional group after removing single hydrogen from an aromatic ring). In this section, reaction, preparation and behavior of ethers are discussed in the context of organic chemistry.
Epoxides
Epoxides are a special class of cyclic ethers which are an important functional group in organic chemistry and generate reactive centers due to their unusual high reactivity. Due to their high reactivity, epoxides are considered to be toxic and mutagenic.
Williamson Ether Synthesis
An organic reaction in which an organohalide and a deprotonated alcohol forms ether is known as Williamson ether synthesis. Alexander Williamson developed the Williamson ether synthesis in 1850. The formation of ether in this synthesis is an SN2 reaction.
Question
![**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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1a6ab37d-5853-4f5d-a5a4-203e58403879%2F1244c29d-ad26-468d-a0f9-579c3f40072d%2F8es2p94_processed.png&w=3840&q=75)
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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