The solubility of CO2 in water at 25 degree celsis and 1 atm is 0.034 mol/L . what is the solubility under atmospheric condition? Assume that CO obeys henry's law. ( the partial pressure of CO2 in air is 0.0003 ATM
Henry's Law :
c = k P
c = the solubility
P = the pressure
k = the constant of that particular gas
If c = k P
then
k = c / P
In this case:
c = 0.034 mol / L
P = 1 atm
k = c / P
k = 0.034 / 1
k = 0.034 mol / L ∙ atm
Now put this constant into Henry's law, but use the second pressure 0.0003 atm.
c = k P
c = ( 0.034 mol / L ∙ atm ) ∙ 0.0003 atm
c = 0.034 ∙ 0.0003 mol / L
c = 0.0000102 mol / L
c = 1.02 ∙ 10⁻⁵ mol / L
Well, if CO2 obeys Henry's Law, then we can use that to determine the solubility under atmospheric conditions. Henry's Law states that the solubility of a gas is directly proportional to its partial pressure. So, let's do some math!
We know that the solubility at 25 degrees Celsius and 1 atm is 0.034 mol/L. Now, we have the partial pressure of CO2 in air, which is 0.0003 atm.
According to Henry's Law, we can set up a proportion:
(solubility under atmospheric conditions) / 0.0003 atm = 0.034 mol/L / 1 atm
Now, we can cross multiply and solve for the solubility under atmospheric conditions:
(solubility under atmospheric conditions) = 0.0003 atm * (0.034 mol/L / 1 atm)
(solubility under atmospheric conditions) = 0.0000102 mol/L
So, the solubility of CO2 under atmospheric conditions is approximately 0.0000102 mol/L. Keep in mind, though, that this answer is not scientifically rigorous. It's just a rough estimate, so take it with a pinch of salt (or CO2, in this case)!
To find the solubility of CO2 under atmospheric conditions, we can use Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Let's denote the solubility of CO2 under atmospheric conditions as x (in mol/L). According to Henry's Law, we have the equation:
x = k * P
Where:
x is the solubility of CO2 under atmospheric conditions,
k is the Henry's Law constant (proportionality constant),
P is the partial pressure of CO2 in air.
From the given information, we know that the solubility of CO2 in water at 25 degrees Celsius and 1 atm is 0.034 mol/L. This gives us the data point:
0.034 mol/L = k * 1 atm
To find the value of k, we can rearrange the equation:
k = 0.034 mol/L / 1 atm
Now, we can substitute the given partial pressure of CO2 in air (0.0003 atm) into the equation to find the solubility under atmospheric conditions:
x = (0.034 mol/L / 1 atm) * 0.0003 atm
Simplifying the equation, we get:
x = 0.0000102 mol/L
Therefore, the solubility of CO2 under atmospheric conditions is approximately 0.0000102 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 in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Henry's Law equation is given as:
C = k * P
where C is the solubility of the gas, k is the Henry's Law constant, and P is the partial pressure of the gas.
Given:
Solubility of CO2 in water at 25 degrees Celsius and 1 atm = 0.034 mol/L
Partial pressure of CO2 in air = 0.0003 atm
Since we are looking to find the solubility under atmospheric conditions, we can substitute the given values into the Henry's Law equation:
C = k * P
0.034 mol/L = k * 1 atm (at 25 degrees Celsius)
0.034 mol/L = k
Now, we can substitute the value of k into the equation to find the solubility under atmospheric conditions:
C = k * P
C = 0.034 mol/L * 0.0003 atm
Simplifying the equation, we get:
C = 0.0000102 mol/L
Therefore, the solubility of CO2 under atmospheric conditions is approximately 0.0000102 mol/L.