presented by Macmillan Learning The Henry's law constant for CO,(g) in water at 25 °C is 29.4 bar-M-. Estimate the concentration of dissolved CO, (g) in a carbonated soft drink pressurized with 1.80 bar of CO,(g). M Mco, 0.6122 %3D Incorrect
presented by Macmillan Learning The Henry's law constant for CO,(g) in water at 25 °C is 29.4 bar-M-. Estimate the concentration of dissolved CO, (g) in a carbonated soft drink pressurized with 1.80 bar of CO,(g). M Mco, 0.6122 %3D Incorrect
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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![**Title: Solubility of Carbon Dioxide in Water**
**Henry's Law and CO₂ Solubility**
*Context: General Chemistry, 4th Edition by McQuarrie, Rock, Gallogly. Published by University Science Books, presented by Macmillan Learning.*
**Problem Statement:**
The Henry's law constant for CO₂(g) in water at 25 °C is 29.4 bar·M⁻¹. Estimate the concentration of dissolved CO₂(g) in a carbonated soft drink pressurized with 1.80 bar of CO₂(g).
**Solution:**
Let the concentration of dissolved CO₂ be represented as \( M_{\text{CO}_2} \).
\[ M_{\text{CO}_2} = 0.6122 \, \text{M} \]
**Note:**
The provided answer is marked as "Incorrect."
**Explanation:**
This exercise involves applying Henry’s Law to determine the concentration of a dissolved gas in a liquid under a given pressure. Henry’s Law states that the concentration of a gas in a liquid is proportional to the partial pressure of the gas above the liquid. The constant \( k_H \) represents this proportionality.
**Summary:**
To find the correct concentration of CO₂ in the soft drink, the formula used is:
\[ C = k_H \times P \]
Where:
- \( C \) is the concentration of the dissolved gas (Molarity, M).
- \( k_H \) is Henry's law constant (29.4 bar·M⁻¹).
- \( P \) is the partial pressure of the gas (1.80 bar).
Please ensure calculations are verified for accuracy.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F95728312-9199-46db-b527-95cb7d377f2b%2Fbef96a6f-04c1-4e1f-999e-e12852c99e97%2F1obhvxn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Solubility of Carbon Dioxide in Water**
**Henry's Law and CO₂ Solubility**
*Context: General Chemistry, 4th Edition by McQuarrie, Rock, Gallogly. Published by University Science Books, presented by Macmillan Learning.*
**Problem Statement:**
The Henry's law constant for CO₂(g) in water at 25 °C is 29.4 bar·M⁻¹. Estimate the concentration of dissolved CO₂(g) in a carbonated soft drink pressurized with 1.80 bar of CO₂(g).
**Solution:**
Let the concentration of dissolved CO₂ be represented as \( M_{\text{CO}_2} \).
\[ M_{\text{CO}_2} = 0.6122 \, \text{M} \]
**Note:**
The provided answer is marked as "Incorrect."
**Explanation:**
This exercise involves applying Henry’s Law to determine the concentration of a dissolved gas in a liquid under a given pressure. Henry’s Law states that the concentration of a gas in a liquid is proportional to the partial pressure of the gas above the liquid. The constant \( k_H \) represents this proportionality.
**Summary:**
To find the correct concentration of CO₂ in the soft drink, the formula used is:
\[ C = k_H \times P \]
Where:
- \( C \) is the concentration of the dissolved gas (Molarity, M).
- \( k_H \) is Henry's law constant (29.4 bar·M⁻¹).
- \( P \) is the partial pressure of the gas (1.80 bar).
Please ensure calculations are verified for accuracy.
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