PLEASE HELP!!
On a clear day at sea level, with a temperature of 25 °C, the partial pressure of N2 in air is 79 kPa and the concentration of nitrogen in water is 5.3 x 10-4 M. When the partial pressure of N2 is ________ kPa, the concentration in water is 1.1 x 10-4 M.
Just set up a proportion.
To find the partial pressure of N2 when the concentration in water is 1.1 x 10-4 M, you need to understand the relationship between partial pressure and concentration.
The relationship between the partial pressure of a gas and its concentration in a solution is described by Henry's Law. Henry's Law states that the concentration of a gas dissolved in a liquid is directly proportional to its partial pressure above the liquid.
Mathematically, Henry's Law can be expressed as:
C = k * P
Where:
C is the concentration of the gas in the liquid solution
k is the Henry's Law constant
P is the partial pressure of the gas above the solution
Given that the concentration of nitrogen in water is 5.3 x 10-4 M at a partial pressure of 79 kPa, we can use this information to find the value of k.
Rearranging the formula, we get:
k = C / P
Substituting the given values:
k = (5.3 x 10-4 M) / (79 kPa)
Now that we have the value of k, we can calculate the partial pressure (P2) when the concentration (C2) is 1.1 x 10-4 M.
Using Henry's Law equation, we have:
C2 = k * P2
Rearranging for P2, we get:
P2 = C2 / k
Substituting the values:
P2 = (1.1 x 10-4 M) / k
Now, plug in the calculated value of k into the equation to find the partial pressure (P2).