of students made 5 standard solutions and measured their corresponding absorbance values at group a wavelength of 525.0 nm to generate the graph below. Absorbance of Standard Solutions to Find Concentration of Unknown X Solution 0.50 y = 75.9x + 0.0045 R? = 0.9946 0.40 0.30 0.20 0.10 0.00 0.001 0.002 0.003 0.004 0.005 0.006 Concentration of X (mole/L) The colorless reactants V and W form unknown X from the reaction: 2V + W S X A solution is prepared by mixing together the following: Volume 0.0150 M V (mL) Volume 0.0150 M W (mL) 6.00 4.00 This solution reaches equilibrium, and then is placed in a 1.00 cm wide cuvet and inserted into the spectrometer, producing an absorbance reading of 0.275 at a wavelength of 525.0 nm. Calculate Keg for the above reaction, including units. Absorbance
of students made 5 standard solutions and measured their corresponding absorbance values at group a wavelength of 525.0 nm to generate the graph below. Absorbance of Standard Solutions to Find Concentration of Unknown X Solution 0.50 y = 75.9x + 0.0045 R? = 0.9946 0.40 0.30 0.20 0.10 0.00 0.001 0.002 0.003 0.004 0.005 0.006 Concentration of X (mole/L) The colorless reactants V and W form unknown X from the reaction: 2V + W S X A solution is prepared by mixing together the following: Volume 0.0150 M V (mL) Volume 0.0150 M W (mL) 6.00 4.00 This solution reaches equilibrium, and then is placed in a 1.00 cm wide cuvet and inserted into the spectrometer, producing an absorbance reading of 0.275 at a wavelength of 525.0 nm. Calculate Keg for the above reaction, including units. Absorbance
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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 <!-- Note: Replace with real image link -->
**Description:**
- **X-axis:** Concentration of X (mole/L)
- **Y-axis:** Absorbance
- **Best Fit Line Equation:** \( y = 75.9x + 0.0045 \)
- **R-squared Value:** \( R^2 = 0.9946 \)
The graph shows a linear relationship between the concentration of X (mole/L) and the absorbance, with the line equation given above.
#### Reaction
The colorless reactants V and W form unknown X from the reaction:
\[ 2V + W \rightleftharpoons X \]
#### Preparation of Solution
A solution was prepared by mixing the following volumes:
| Volume 0.0150 M V (mL) | Volume 0.0150 M W (mL) |
|------------------------|------------------------|
| 6.00 | 4.00 |
#### Experimental Data
This solution reached equilibrium and was then placed in a 1.00 cm wide cuvet for measurement. The spectrometer provided an absorbance reading of 0.275 at a wavelength of 525.0 nm.
#### Calculation of \( K_{eq} \)
1. **Calculate the concentration of X using the calibration curve:**
Given:
\[ \text{Absorbance (A)} = 0.275 \]
Using the best fit line equation:
\[ A = 75.9 \cdot [X] + 0.0045 \]
Solving for \([X]\):
\[ 0.275 = 75.9 \cdot [X] + 0.0045 \]
\[ 75.9 \cdot [X] = 0.275 - 0.0045 \]
\[ 75.9 \cdot [X] = 0.2705 \]
\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fda7693ac-42ba-43da-875a-8ee9e0eebed9%2F50832a4f-4ba3-486b-af1e-a51a04cb7889%2Feoimx4e_processed.png&w=3840&q=75)
Transcribed Image Text:### Determination of Equilibrium Constant \( K_{eq} \)
#### Experimental Background
A group of students prepared 5 standard solutions and measured their corresponding absorbance values at a wavelength of 525.0 nm. These values were then used to generate the calibration graph illustrated below.
#### Calibration Graph
**Title:** Absorbance of Standard Solutions to Find Concentration of Unknown X Solution
 <!-- Note: Replace with real image link -->
**Description:**
- **X-axis:** Concentration of X (mole/L)
- **Y-axis:** Absorbance
- **Best Fit Line Equation:** \( y = 75.9x + 0.0045 \)
- **R-squared Value:** \( R^2 = 0.9946 \)
The graph shows a linear relationship between the concentration of X (mole/L) and the absorbance, with the line equation given above.
#### Reaction
The colorless reactants V and W form unknown X from the reaction:
\[ 2V + W \rightleftharpoons X \]
#### Preparation of Solution
A solution was prepared by mixing the following volumes:
| Volume 0.0150 M V (mL) | Volume 0.0150 M W (mL) |
|------------------------|------------------------|
| 6.00 | 4.00 |
#### Experimental Data
This solution reached equilibrium and was then placed in a 1.00 cm wide cuvet for measurement. The spectrometer provided an absorbance reading of 0.275 at a wavelength of 525.0 nm.
#### Calculation of \( K_{eq} \)
1. **Calculate the concentration of X using the calibration curve:**
Given:
\[ \text{Absorbance (A)} = 0.275 \]
Using the best fit line equation:
\[ A = 75.9 \cdot [X] + 0.0045 \]
Solving for \([X]\):
\[ 0.275 = 75.9 \cdot [X] + 0.0045 \]
\[ 75.9 \cdot [X] = 0.275 - 0.0045 \]
\[ 75.9 \cdot [X] = 0.2705 \]
\
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