How many grams of CO2 gas is dissolved in a 1 lt bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at 25oC?(KH of CO2 water=29.76atm/mole/l at 25oC)
How many grams of CO2 gas is dissolved in a 1 lt bottle of carbonated water if the manufacturer uses a pressure of 2.4 atmosphere in the bottling process at 25oC?(KH of CO2 water=29.76atm/mole/l at 25oC)
The correct option is C 3.52
When a gas is dissolved in a liquid, the concentrations will eventually reach equilibrium between the source of the gas and the solution. Henry's law shows that the concentration of a solute gas in a solution is directly proportional to the partial pressure of the gas over the solution.
P = KHC where:
P is the partial pressure of the gas above the solution.
KH is Henry's law constant for the solution.
C is the concentration of the dissolved gas in solution.
C = P/KH
C = 2.4 atm/29.76 atm/(mol/L)
C = 0.08 mol/L
Since we have only 1 L of water, we have 0.08 mol of CO.
Convert moles to grams:
Mass of 1 mol of CO2 = 12+(16x2) = 12+32 = 44 g
g of CO2 = mol CO2 x (44 g/mol)
g of CO2 = 8.06 x 10-2 mol x 44 g/mol
g of CO2 = 3.52 g
When a gas is dissolved in a liquid, the concentrations will eventually reach equilibrium between the source of the gas and the solution. Henry's law shows that the concentration of a solute gas in a solution is directly proportional to the partial pressure of the gas over the solution.
P = KHC where:
P is the partial pressure of the gas above the solution.
KH is Henry's law constant for the solution.
C is the concentration of the dissolved gas in solution.
C = P/KH
C = 2.4 atm/29.76 atm/(mol/L)
C = 0.08 mol/L
Since we have only 1 L of water, we have 0.08 mol of CO.
Convert moles to grams:
Mass of 1 mol of CO2 = 12+(16x2) = 12+32 = 44 g
g of CO2 = mol CO2 x (44 g/mol)
g of CO2 = 8.06 x 10-2 mol x 44 g/mol
g of CO2 = 3.52 g
