Concept explainers
Interpretation: It should be determined that what mass of dissolved CO2 which is released to the atmosphere in order to reach equilibrium.
Concept introduction:
- Henry’s law: The solubility of a gas in liquid is directly proportional to the gas pressure.
Sg= kHPg,where, Sg is the gas solubility (in mol/kg) kH is Henry's constant Pg is the partial pressure of the gaseous solute.
- Density = MassVolume
Answer to Problem 2.4ACP
6.0 g CO2 will be released to the atmosphere in order to reach equilibrium.
Explanation of Solution
Given,partial pressure of CO2 = 4 barHenry's constant = 0.034 mol/kg.barAccording to Henry's law, Sg = kHPgsolubility of CO2 before opening = 0.034 mol/kg.bar × 4 bar = 0.136 mol /kg
Assume that, the density of the solution is 1.0 g/cm3. Therefore 1.0 L corresponds to 1 kg. The amount of CO2 dissolved is 0.136 mol.
Solubility of CO2 after opening can be calculated as follows:
partial pressure of CO2 = 3.7×10-4 barHenry's constant = 0.034 mol/kg.bar
According to Henry’s law:
Sg = kHPg
Substituting the given values in the above equation, the solubility can be calculated.
Sg = 0.034mol/kg.bar ×3.7×10-4 bar = 1.26 ×10-5 mol/kg Solubility of CO2 after opening = 1.26 × 10-5 mol/Kg.The amount of CO2 in 1.0 kg is 1.26 × 10-5 mol.
Mass of CO2 released = (Amount of CO2 present before opening soda - Amount of CO2 present after opening soda) × Molar mass of CO2 = (0.136 mol CO2 - 1.26 × 10-5 mol CO2 ) × 44.01 g/mol CO2 = 6.0 g CO2
6.0 g CO2 would be released to the atmosphere in order to reach equilibrium.
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Chapter 13 Solutions
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