The Henry's law constant at 25 °C for CO2 in water is 0.035 M/ atm. What is the solubility of CO2, in molarity units, in 1.0 L of water when the partial pressure of CO2 is 1.1 atm?
The Henry's law constant at 25 °C for CO2 in water is 0.035 M/ atm. What is the solubility of CO2, in molarity units, in 1.0 L of water when the partial pressure of CO2 is 1.1 atm?
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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![**Henry's Law and Solubility of CO₂ in Water**
The Henry's law constant at 25 °C for carbon dioxide (CO₂) in water is 0.035 M/atm. To find the solubility of CO₂, expressed in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 1.1 atm, you can use Henry's law.
**Henry's Law Formula:**
\[ C = k_{\text{H}} \times P \]
Where:
- \( C \) is the solubility of the gas (in molarity, M)
- \( k_{\text{H}} \) is Henry's law constant (0.035 M/atm)
- \( P \) is the partial pressure of the gas (1.1 atm)
**Calculation:**
\[ C = 0.035 \, \text{M/atm} \times 1.1 \, \text{atm} = 0.0385 \, \text{M} \]
Thus, the solubility of CO₂ in 1.0 L of water, under a partial pressure of 1.1 atm, is 0.0385 M.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4e3da8d7-5e45-4b35-92f7-ecdb5bd91ee7%2Fc57a778c-8465-479c-913f-b3cdff10943b%2Fm6njus_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Henry's Law and Solubility of CO₂ in Water**
The Henry's law constant at 25 °C for carbon dioxide (CO₂) in water is 0.035 M/atm. To find the solubility of CO₂, expressed in molarity units, in 1.0 L of water when the partial pressure of CO₂ is 1.1 atm, you can use Henry's law.
**Henry's Law Formula:**
\[ C = k_{\text{H}} \times P \]
Where:
- \( C \) is the solubility of the gas (in molarity, M)
- \( k_{\text{H}} \) is Henry's law constant (0.035 M/atm)
- \( P \) is the partial pressure of the gas (1.1 atm)
**Calculation:**
\[ C = 0.035 \, \text{M/atm} \times 1.1 \, \text{atm} = 0.0385 \, \text{M} \]
Thus, the solubility of CO₂ in 1.0 L of water, under a partial pressure of 1.1 atm, is 0.0385 M.
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