The solubility of CO2 in water at 25 degrees C and 1 atm is 0.034 mol/L. What is its solubility under atmospheric conditions? (The partial pressure of CO2 in air is 0.0003 atm.) Assume that CO2 obeys Henry's law.
My Answer:
1.02 x 10^-5 mol/L
. Henry's law states that the solubility of a gas in a liquid is proportional to the partial pressure of the gas. Therefore, the solubility of CO2 in water at atmospheric conditions (0.0003 atm) is 0.034 mol/L x (0.0003 atm/1 atm) = 1.02 x 10^-5 mol/L.
To calculate the solubility of CO2 under atmospheric conditions, you can use Henry's law. Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
First, you need to determine the Henry's law constant (K) for CO2 in water at 25 degrees Celsius and 1 atm. The formula for Henry's law is given by:
C = K * P
Where C is the concentration of the gas in the liquid, K is the Henry's law constant, and P is the partial pressure of the gas.
Given that the solubility of CO2 in water is 0.034 mol/L at 25 degrees Celsius and 1 atm, you can rearrange the equation to solve for K:
0.034 mol/L = K * 1 atm
Therefore, K = 0.034 mol/L / 1 atm = 0.034 mol/(L * atm).
Now, using the partial pressure of CO2 in air (0.0003 atm), you can calculate the solubility of CO2 under atmospheric conditions:
C = K * P
C = 0.034 mol/(L * atm) * 0.0003 atm
C = 1.02 x 10^-5 mol/L
Therefore, the solubility of CO2 under atmospheric conditions is approximately 1.02 x 10^-5 mol/L.
To find the solubility of CO2 under atmospheric conditions, we can use Henry's law, which states that the solubility of a gas is directly proportional to its partial pressure.
First, we need to calculate the solubility constant (K) using the given solubility at 25 degrees Celsius and 1 atm. We can use the formula K = solubility/partial pressure.
K = 0.034 mol/L / 1 atm
Now, we can use this solubility constant to find the solubility under atmospheric conditions, where the partial pressure of CO2 in air is 0.0003 atm.
solubility = K x partial pressure
solubility = (0.034 mol/L)(0.0003 atm)
solubility = 1.02 x 10^-5 mol/L
Therefore, the solubility of CO2 under atmospheric conditions is 1.02 x 10^-5 mol/L.