The solubility of CO2 in water at 25 degrees Celsius and P CO2= 1 atm is 0.034 mol/L. What is its water solubility under normal atmospheric conditions (in air, carbon dioxide is about 380 ppmv assuming that CO2 obeys Henry's Law?
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To determine the water solubility of carbon dioxide (CO2) under normal atmospheric conditions assuming it obeys Henry's Law, we need to calculate the Henry's Law constant (K) and use the given partial pressure of CO2 in air (P).
Henry's Law states that the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid. Mathematically, it can be expressed as:
C = K * P
Where:
C = Concentration of the gas in the liquid (mol/L)
K = Henry's Law constant (mol/L/atm)
P = Partial pressure of the gas above the liquid (atm)
Now, we can calculate K using the solubility of CO2 in water at 25 degrees Celsius and P CO2 = 1 atm, which is given as 0.034 mol/L.
K = C / P = 0.034 mol/L / 1 atm = 0.034 mol/L
Since we know the partial pressure of CO2 in air is about 380 ppmv (parts per million by volume), we need to convert it to atm by dividing it by 1,000,000.
P = 380 ppmv / 1,000,000 = 0.000380 atm
Using the calculated value of K and the given P, we can now determine the water solubility (C) under normal atmospheric conditions:
C = K * P = 0.034 mol/L * 0.000380 atm ≈ 0.00001292 mol/L
Therefore, the water solubility of CO2 under normal atmospheric conditions is approximately 0.00001292 mol/L.
To find the water solubility of CO2 under normal atmospheric conditions, we 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.
In this case, we need to find the solubility of CO2 in water when the partial pressure of CO2 is 380 ppmv. The partial pressure of CO2 in air is usually given in units of pressure, such as atm or Pa, so we first need to convert ppmv to atm.
Since 1 ppmv represents one part per million by volume, we can assume that one ppmv is equal to one molecule of CO2 per million molecules of air.
To convert ppmv to atm, we can use the ideal gas law equation:
P = nRT/V
Where:
P = Pressure in atm
n = Number of moles of CO2
R = Ideal gas constant (0.0821 L·atm/mol·K)
T = Temperature in Kelvin
V = Volume of the gas in liters
However, we only need to find the partial pressure, so we can rearrange the equation to solve for P:
P = (n/V)RT
Given that the partial pressure of CO2 is 1 atm at 25 degrees Celsius, we can rearrange the equation and solve for n/V:
1 atm = (n/V) * (0.0821 L·atm/mol·K) * (273 + 25 K)
n/V = 1 atm / [(0.0821 L·atm/mol·K) * (273 + 25 K)]
n/V ≈ 0.0427 mol/L
Now, we can use Henry's Law to find the water solubility of CO2:
Solubility = k * P
Where:
Solubility = Concentration of CO2 in water (mol/L)
k = Henry's Law constant for CO2 in water at the given temperature (mol/L/atm)
P = Partial pressure of CO2 (atm)
Given that the solubility of CO2 in water at 25 degrees Celsius and P CO2 = 1 atm is 0.034 mol/L, we can rearrange the equation and solve for k:
0.034 mol/L = k * 1 atm
k ≈ 0.034 mol/L
Finally, we can calculate the water solubility of CO2 under normal atmospheric conditions:
Solubility = k * P
Solubility = (0.034 mol/L) * (0.0427 mol/L)
Solubility ≈ 0.00145 mol/L
Therefore, the water solubility of CO2 under normal atmospheric conditions (assuming CO2 obeys Henry's Law) is approximately 0.00145 mol/L.
solubility is directly proporional to partial pressure.
Partial pressue of CO2: 1atm(380/1E6)
solubiliy: .034mol/L * 380*1E-6
= 1.25E-5 mol/liter
= .0000125 mol/liter