At a total atmospheric pressure of 1.00 atm, the partial pressure of CO2 in air is approximately 4.0×10−4 atm.
If at 20 ∘C and a partial pressure of 760 mmHg, the solubility of CO2 in water is 0.169 g/100mL, what is the solubility of CO2 in an open bottle of seltzer water at 20 ∘C?
6.8×10−5 g/100mL
wrong
To find the solubility of CO2 in an open bottle of seltzer water at 20 ∘C, we first need to determine the partial pressure of CO2 in the bottle.
Since we know the partial pressure of CO2 in air is approximately 4.0×10−4 atm at a total atmospheric pressure of 1.00 atm, we can calculate the partial pressure of CO2 in the bottle of seltzer water as follows:
Partial Pressure of CO2 = Total Atmospheric Pressure × Partial Pressure of CO2 in Air
Partial Pressure of CO2 = 1.00 atm × 4.0×10−4 atm
Partial Pressure of CO2 = 4.0×10−4 atm
Now, let's convert the given partial pressure of CO2 from mmHg to atm.
1 atm = 760 mmHg
Partial Pressure of CO2 = 760 mmHg × (1 atm / 760 mmHg)
Partial Pressure of CO2 = 1 atm
Therefore, the partial pressure of CO2 in the bottle of seltzer water is 1 atm.
Now, we can use the solubility of CO2 in water at 20 ∘C and a partial pressure of 1 atm to find the solubility of CO2 in the open bottle of seltzer water.
Solubility of CO2 = Solubility in Water × (Partial Pressure of CO2 / 1 atm)
Using the given solubility of CO2 in water at 20 ∘C (0.169 g/100mL) and the partial pressure of CO2 in the bottle (1 atm), we can calculate the solubility of CO2 in the open bottle of seltzer water as follows:
Solubility of CO2 = 0.169 g/100mL × (1 atm / 1 atm)
Solubility of CO2 = 0.169 g/100mL
Therefore, the solubility of CO2 in an open bottle of seltzer water at 20 ∘C is 0.169 g/100mL.