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3. A bottled soft drink at 25°C contains carbon dioxide at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of the carbon dioxide gas is 4.0*10-4 atm, calculate the equilibrium concentrations of carbon dioxide in the soda both before and after the bottle is opened. The Henry's Law constant for carbon dioxide in aqueous solution is 3.1*102 mol/Latm at 25°C.

3. A bottled soft drink at 25°C contains carbon dioxide at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of the carbon dioxide gas is 4.0*10-4 atm, calculate the equilibrium concentrations of carbon dioxide in the soda both before and after the bottle is opened. The Henry's Law constant for carbon dioxide in aqueous solution is 3.1*102 mol/Latm at 25°C.

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Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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3. A bottled soft drink at 25°C contains carbon dioxide at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of the carbon dioxide gas is 4.0*10-4 atm, calculate the equilibrium concentrations of carbon dioxide in the soda both before and after the bottle is opened. The Henry's Law constant for carbon dioxide in aqueous solution is 3.1*10² mol/Latm at 25°C. 4. Calculate the expected vapor pressure at 25°C for a solution prepared by dissolving 158.0 g of sugar (molar mass=342.3 g/mol) in 643.5 cm³ water. At 25°C, the density of water is 0.9971 g/cm³ and the vapor pressure is 23.76 torr.
Transcribed Image Text:3. A bottled soft drink at 25°C contains carbon dioxide at a pressure of 5.0 atm over the liquid. Assuming that the partial pressure of the carbon dioxide gas is 4.0*10-4 atm, calculate the equilibrium concentrations of carbon dioxide in the soda both before and after the bottle is opened. The Henry's Law constant for carbon dioxide in aqueous solution is 3.1*10² mol/Latm at 25°C. 4. Calculate the expected vapor pressure at 25°C for a solution prepared by dissolving 158.0 g of sugar (molar mass=342.3 g/mol) in 643.5 cm³ water. At 25°C, the density of water is 0.9971 g/cm³ and the vapor pressure is 23.76 torr.
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