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 4.010-4 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 3.1102 mol/Latm at 25°C.

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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Please please answer super fast

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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