Suppose a 500. mL flask is filled with 0.10 mol of SO₂ and 1.1 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g)2SO₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. SO so
Suppose a 500. mL flask is filled with 0.10 mol of SO₂ and 1.1 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g)2SO₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. SO so
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![# Setting up a Reaction Table: Kinetics and Equilibrium
## Reaction Scenario
Suppose a 500. mL flask is filled with 0.10 mol of SO₂ and 1.1 mol of SO₃. This reaction becomes possible:
\[ 2\text{SO}_3(g) \rightleftharpoons 2\text{SO}_2(g) + \text{O}_2(g) \]
## Objective
Complete the table below, so that it lists:
- The initial molarity of each compound
- The change in molarity of each compound due to the reaction
- The equilibrium molarity of each compound after the reaction has come to equilibrium
Use \( x \) to stand for the unknown change in the molarity of \(\text{O}_2\). You can leave out the \( M \) symbol for molarity.
### Reaction Table
| | SO₂ | SO₃ | O₂ |
|--------------|-----|-----|-----|
| **Initial** | | | |
| **Change** | | | x |
| **Equilibrium** | | | |
[Explanation] [Check]
## Instructions
- Fill in the initial concentrations based on the moles given and calculate the changes using the stoichiometry of the reaction.
- Determine the equilibrium concentrations using the initial and change values.
This activity will help you understand how to apply the concepts of chemical equilibrium and stoichiometry in reaction tables.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9be9a090-f726-46c3-84a4-96616934014f%2F4a9e356b-e3e0-4adc-ad01-dc13d5504e54%2F9b5fsew_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# Setting up a Reaction Table: Kinetics and Equilibrium
## Reaction Scenario
Suppose a 500. mL flask is filled with 0.10 mol of SO₂ and 1.1 mol of SO₃. This reaction becomes possible:
\[ 2\text{SO}_3(g) \rightleftharpoons 2\text{SO}_2(g) + \text{O}_2(g) \]
## Objective
Complete the table below, so that it lists:
- The initial molarity of each compound
- The change in molarity of each compound due to the reaction
- The equilibrium molarity of each compound after the reaction has come to equilibrium
Use \( x \) to stand for the unknown change in the molarity of \(\text{O}_2\). You can leave out the \( M \) symbol for molarity.
### Reaction Table
| | SO₂ | SO₃ | O₂ |
|--------------|-----|-----|-----|
| **Initial** | | | |
| **Change** | | | x |
| **Equilibrium** | | | |
[Explanation] [Check]
## Instructions
- Fill in the initial concentrations based on the moles given and calculate the changes using the stoichiometry of the reaction.
- Determine the equilibrium concentrations using the initial and change values.
This activity will help you understand how to apply the concepts of chemical equilibrium and stoichiometry in reaction tables.
Expert Solution
Step 1
Given moles of SO2 = 0.10 mol
Gicen moles of SO3 = 1.1 mol
Initial moles of oxygen = 0
We are given reaction at equilibrium and we have to complete ICE table
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