Suppose a 500. mL flask is filled with 0.50 mol of NO₂ and 1.5 mol of NO. This reaction becomes possible: 2NO₂(g) 2NO(g) + O₂(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 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 O₂. You can leave out the M symbol for molarity. 1 initial change equilibrium NO₂ 0 NO 0 0 0 0₂ 0 X 0 00 X
Suppose a 500. mL flask is filled with 0.50 mol of NO₂ and 1.5 mol of NO. This reaction becomes possible: 2NO₂(g) 2NO(g) + O₂(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 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 O₂. You can leave out the M symbol for molarity. 1 initial change equilibrium NO₂ 0 NO 0 0 0 0₂ 0 X 0 00 X
Chemistry
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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
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![## Title: Setting Up a Reaction Table
**Context: Kinetics and Equilibrium**
### Reaction and Initial Conditions
- A reaction takes place in a 500 mL flask containing 0.50 mol of NO₂ and 1.5 mol of NO.
- The reaction is as follows:
\[
2\text{NO}_2(g) \rightarrow 2\text{NO}(g) + \text{O}_2(g)
\]
### Objective
- Complete the table by determining:
- Initial molarity of each compound
- Change in molarity resulting from the reaction
- Equilibrium molarity of each compound
### Instructions
- Use \( x \) to represent the unknown change in the molarity of \(\text{O}_2\).
- The symbol \( M \) for molarity can be omitted.
### Reaction Table
\[
\begin{array}{|c|c|c|c|}
\hline
& \text{NO}_2 & \text{NO} & \text{O}_2 \\
\hline
\text{Initial} & 0.50 & 1.5 & 0 \\
\hline
\text{Change} & -2x & +2x & +x \\
\hline
\text{Equilibrium} & 0.50 - 2x & 1.5 + 2x & x \\
\hline
\end{array}
\]
### Explanation Box
Below the table, there is a section for entering explanations regarding the calculations and assumptions made.
- **Check**: A button to verify the accuracy of your input to ensure the values satisfy the equilibrium conditions.
---
This guide outlines the procedure for setting up and completing a reaction table as part of studying chemical kinetics and equilibrium. Follow the instructions carefully to determine how each reactant and product’s molar concentration changes over time until equilibrium is achieved.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9be9a090-f726-46c3-84a4-96616934014f%2Ffe4d8715-8268-40fe-a18c-32d0e002c13f%2Fe9mda4i_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Title: Setting Up a Reaction Table
**Context: Kinetics and Equilibrium**
### Reaction and Initial Conditions
- A reaction takes place in a 500 mL flask containing 0.50 mol of NO₂ and 1.5 mol of NO.
- The reaction is as follows:
\[
2\text{NO}_2(g) \rightarrow 2\text{NO}(g) + \text{O}_2(g)
\]
### Objective
- Complete the table by determining:
- Initial molarity of each compound
- Change in molarity resulting from the reaction
- Equilibrium molarity of each compound
### Instructions
- Use \( x \) to represent the unknown change in the molarity of \(\text{O}_2\).
- The symbol \( M \) for molarity can be omitted.
### Reaction Table
\[
\begin{array}{|c|c|c|c|}
\hline
& \text{NO}_2 & \text{NO} & \text{O}_2 \\
\hline
\text{Initial} & 0.50 & 1.5 & 0 \\
\hline
\text{Change} & -2x & +2x & +x \\
\hline
\text{Equilibrium} & 0.50 - 2x & 1.5 + 2x & x \\
\hline
\end{array}
\]
### Explanation Box
Below the table, there is a section for entering explanations regarding the calculations and assumptions made.
- **Check**: A button to verify the accuracy of your input to ensure the values satisfy the equilibrium conditions.
---
This guide outlines the procedure for setting up and completing a reaction table as part of studying chemical kinetics and equilibrium. Follow the instructions carefully to determine how each reactant and product’s molar concentration changes over time until equilibrium is achieved.
Expert Solution
Step 1
Answer:
In the given problem statement equilibrium of decomposition of NO2 in a 500mL flask is mentioned and we have to prepare ICE table for this equilibrium.
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