calculate the Henry's law proportionality constant for N2?
partial pressure at 1 atm=0.78 atm
solubility at 1 atm= 5.3 x 10^-3 mol/L
constant=Partial pressure / solubility
What's the temperature? 0.78/0.0053 doesn't give a number that agrees with the literature.
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. Mathematically, it can be expressed as:
C = k * P
Where C is the solubility of the gas, P is the partial pressure of the gas, and k is the Henry's law constant (also known as the proportionality constant).
To calculate the Henry's law constant for N2, you can rearrange the equation as:
k = C / P
Given that the partial pressure of N2 (P) is 0.78 atm and the solubility (C) is 5.3 x 10^-3 mol/L, you can substitute these values into the equation to find the Henry's law constant for N2:
k = (5.3 x 10^-3 mol/L) / (0.78 atm)
k ≈ 0.0068 mol/(L·atm)
Therefore, the Henry's law proportionality constant for N2 is approximately 0.0068 mol/(L·atm).
To calculate the Henry's law proportionality constant (also known as Henry's law constant) for N2, we can use the equation:
C = k * P
Where C is the concentration of the gas in moles per liter (mol/L), k is the Henry's law constant, and P is the partial pressure of the gas in atmospheres (atm).
In this case, we have the following information:
Partial pressure at 1 atm (P) = 0.78 atm
Solubility at 1 atm (C) = 5.3 x 10^-3 mol/L
We want to find the Henry's law constant (k).
Rearranging the equation, we have:
k = C / P
Substituting the given values, we get:
k = (5.3 x 10^-3 mol/L) / (0.78 atm)
Now, we'll calculate the value using a calculator.
k ≈ 0.0068 mol/(L·atm)
Therefore, the Henry's law constant for N2 is approximately 0.0068 mol/(L·atm).