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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 80QRT

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Question

The henry constant for the dissolution of CO2 in water is 3.4 x 10^-2 atm/M at 25°C. Assuming ideal behavior, calculate the pressure of CO2 gas required to reach 0.0018 mole fraction of CO2 in the prepared carbonated water. density of carbonated water=1gcm^-3

Expert Solution

Step 1

Given data set:

Henry constant = Kh = 3.4*10^-2 atm/M

Temperature = T = 25 C

Mole fraction of CO2(solute) = Xsolute= 0.0018

Mole fraction of water(solvent) = Xsolvent = 0.9982

Density = 1 g/cm^3 = Dsolution = 1 g/ml = 1000 g/L

Molar mass of CO2 = M.Wsolute = 44 g/mol

Molar mass of H2O = M.Wsolvent = 18 g/mol.

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