The equilibrium constant, K., for the following reaction is 6.50×10-3 at 298 K. 2NOBr(g) |2NO(g) + Br2(g) Assuming that you start with only NOBr, describe the relative abundance of each species present at equilibrium. Clear All [Br2] Higher [NO] Lower [NOB1] Can't tell
The equilibrium constant, K., for the following reaction is 6.50×10-3 at 298 K. 2NOBr(g) |2NO(g) + Br2(g) Assuming that you start with only NOBr, describe the relative abundance of each species present at equilibrium. Clear All [Br2] Higher [NO] Lower [NOB1] Can't tell
Chemistry
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ISBN:9781305957404
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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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![### Equilibrium Constants and Reaction Abundance
The equilibrium constant, \( K_c \), for the following reaction is \( 6.50 \times 10^{-3} \) at 298 K.
\[ 2NOBr(g) \leftrightharpoons 2NO(g) + Br_2(g) \]
Assuming that you start with only NOBr, describe the relative abundance of each species present at equilibrium.
#### Abundance Options Box
This interactive element allows users to classify the relative abundance (Higher, Lower, Can't tell) of the chemical species at equilibrium:
- **[Br\(_2\)]**
- **Higher**
- **Lower**
- **Can't tell**
- **[NO]**
- **Higher**
- **Lower**
- **Can't tell**
- **[NOBr]**
- **Higher**
- **Lower**
- **Can't tell**
There is also a "Clear All" button which resets the selections.
### Explanation:
Given that the equilibrium constant \( K_c \) is small (\( 6.50 \times 10^{-3} \)), it suggests that at equilibrium, the concentration of reactants (\( NOBr \)) will be higher than the concentration of products (\( NO \) and \( Br_2 \)). Therefore:
- **[Br\(_2\)]**: Lower
- **[NO]**: Lower
- **[NOBr]**: Higher](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9cce6311-c94c-4650-90f7-705d2febbb40%2F6a9426d8-3848-438b-b077-3499b71c3d91%2Fg86jamr_processed.png&w=3840&q=75)
Transcribed Image Text:### Equilibrium Constants and Reaction Abundance
The equilibrium constant, \( K_c \), for the following reaction is \( 6.50 \times 10^{-3} \) at 298 K.
\[ 2NOBr(g) \leftrightharpoons 2NO(g) + Br_2(g) \]
Assuming that you start with only NOBr, describe the relative abundance of each species present at equilibrium.
#### Abundance Options Box
This interactive element allows users to classify the relative abundance (Higher, Lower, Can't tell) of the chemical species at equilibrium:
- **[Br\(_2\)]**
- **Higher**
- **Lower**
- **Can't tell**
- **[NO]**
- **Higher**
- **Lower**
- **Can't tell**
- **[NOBr]**
- **Higher**
- **Lower**
- **Can't tell**
There is also a "Clear All" button which resets the selections.
### Explanation:
Given that the equilibrium constant \( K_c \) is small (\( 6.50 \times 10^{-3} \)), it suggests that at equilibrium, the concentration of reactants (\( NOBr \)) will be higher than the concentration of products (\( NO \) and \( Br_2 \)). Therefore:
- **[Br\(_2\)]**: Lower
- **[NO]**: Lower
- **[NOBr]**: Higher
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