At a certain temperature, the equilibrium constant K for the following reaction is 7.8 × 108 NO₂(g) + NO(g) 2 NO₂(g) Use this information to complete the following table. Suppose a 11. L reaction vessel is filled with 1.4 mol of NO₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(9) L NO3(9) + NO (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2NO3(9)+2NO(9) 4 NO₂(9) L There will be very little NO3 and NO. O There will be very little NO₂. O Neither of the above is true. K = 0 K = 0
At a certain temperature, the equilibrium constant K for the following reaction is 7.8 × 108 NO₂(g) + NO(g) 2 NO₂(g) Use this information to complete the following table. Suppose a 11. L reaction vessel is filled with 1.4 mol of NO₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(9) L NO3(9) + NO (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2NO3(9)+2NO(9) 4 NO₂(9) L There will be very little NO3 and NO. O There will be very little NO₂. O Neither of the above is true. K = 0 K = 0
Chemistry
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Chapter1: Chemical Foundations
Section: Chapter Questions
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![**Kinetics and Equilibrium: Using the General Properties of Equilibrium Constants**
---
At a certain temperature, the equilibrium constant \( K \) for the following reaction is \( 7.8 \times 10^{-8} \):
\[
\text{NO}_3(g) + \text{NO}(g) \rightarrow 2\text{NO}_2(g)
\]
Use this information to complete the following table.
---
**Suppose a 1 L reaction vessel is filled with 1.4 mol of NO\(_2\). What can you say about the composition of the mixture in the vessel at equilibrium?**
- [ ] There will be very little NO\(_3\) and NO.
- [ ] There will be very little NO\(_2\).
- [ ] Neither of the above is true.
---
**What is the equilibrium constant for the following reaction?**
Round your answer to 2 significant digits.
\[
2\text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g)
\]
\[
K = \text{[ \_\_ ]}
\]
---
**What is the equilibrium constant for the following reaction?**
Round your answer to 2 significant digits.
\[
2\text{NO}_3(g) + 2\text{NO}(g) \rightarrow 4\text{NO}_2(g)
\]
\[
K = \text{[ \_\_ ]}
\]
---
*Note*: Use the principles of chemical equilibrium and the provided equilibrium constant to determine the answers.
Buttons: [Explanation] [Check]
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Transcribed Image Text:**Kinetics and Equilibrium: Using the General Properties of Equilibrium Constants**
---
At a certain temperature, the equilibrium constant \( K \) for the following reaction is \( 7.8 \times 10^{-8} \):
\[
\text{NO}_3(g) + \text{NO}(g) \rightarrow 2\text{NO}_2(g)
\]
Use this information to complete the following table.
---
**Suppose a 1 L reaction vessel is filled with 1.4 mol of NO\(_2\). What can you say about the composition of the mixture in the vessel at equilibrium?**
- [ ] There will be very little NO\(_3\) and NO.
- [ ] There will be very little NO\(_2\).
- [ ] Neither of the above is true.
---
**What is the equilibrium constant for the following reaction?**
Round your answer to 2 significant digits.
\[
2\text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g)
\]
\[
K = \text{[ \_\_ ]}
\]
---
**What is the equilibrium constant for the following reaction?**
Round your answer to 2 significant digits.
\[
2\text{NO}_3(g) + 2\text{NO}(g) \rightarrow 4\text{NO}_2(g)
\]
\[
K = \text{[ \_\_ ]}
\]
---
*Note*: Use the principles of chemical equilibrium and the provided equilibrium constant to determine the answers.
Buttons: [Explanation] [Check]
© 2022 McGraw Hill LLC. All Rights Reserved.
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