Calculate the solubility of in water at a partial pressure of of 140. torr at 25°C. The Henry's law constant for is for Henry's law in the form C = kP, where C is the gas concentration (mol/L).
To calculate the solubility of a gas in water using Henry's law, we can use the equation C = kP, where C is the gas concentration (mol/L), k is the Henry's law constant, and P is the partial pressure of the gas.
Given information:
Partial pressure of
Partial pressure (P) = 140 torr
Henry's law constant (k) =
We need to find the solubility of (C).
Using the Henry's law equation C = kP, we can rearrange it to solve for C:
C = (k)(P)
Substituting the values:
C = ( )(140 torr)
To calculate solubility, we need to convert the pressure from torr to atm:
1 atm = 760 torr
P (in atm) = 140 torr / 760 torr/atm
Substituting back into the equation:
C = ( ) * (140 torr / 760 torr/atm)
Calculating the value inside the brackets:
C = (140 torr / 760 torr/atm)
Now, calculate the solubility:
C =
The solubility of in water at a partial pressure of 140 torr at 25°C using Henry's law is mol/L.
To calculate the solubility of a gas in water at a given partial pressure using Henry's Law, we can use the equation C = kP, where C is the concentration of the gas in solution, k is the Henry's Law constant, and P is the partial pressure of the gas.
In this case, you are given the partial pressure of carbon dioxide (P = 140. torr) and the Henry's Law constant for carbon dioxide (k = ). You need to find the solubility of carbon dioxide (C) in water.
The first step is to rearrange the Henry's Law equation to solve for C:
C = kP
Now, substitute the given values into the equation:
C = × (140. torr)
Next, convert the partial pressure from torr to atm (since the Henry's Law constant is given in atm):
1 atm = 760 torr
Therefore, the partial pressure of carbon dioxide (P) in atm is:
P = 140. torr / 760 torr/atm
Now, substitute the value of P into the equation:
C = ×
Finally, evaluate the expression to calculate the solubility of carbon dioxide in water at the given conditions.