A sealed flask containing water and N2 gas in equilibrium is at a temperature of 25°C. If the concentration of N2 gas in the solution is 1.4 x 10-3 M, what is the partial pressure of N2 gas in the container? (kH for N2 gas in water is 6.1 x 10-4 M/atm at 25°C.)
C= kp
You know C and k, solve for p which is the partial pressure of N2 above the gas in the container.
To find the partial pressure of N2 gas in the container, you can use Henry's Law, which states that the partial pressure of a gas in a liquid is directly proportional to its concentration in the solution.
The equation for Henry's Law is:
P = kH * C
Where:
P = partial pressure of gas
kH = Henry's Law constant
C = concentration of gas in solution
In this case, you are given the concentration of N2 gas (C) as 1.4 x 10^-3 M and the Henry's Law constant (kH) as 6.1 x 10^-4 M/atm.
Using these values in the equation, you can calculate the partial pressure (P):
P = (6.1 x 10^-4 M/atm) * (1.4 x 10^-3 M)
P = 8.54 x 10^-7 atm
Therefore, the partial pressure of N2 gas in the container is 8.54 x 10^-7 atm.
To calculate the partial pressure of N2 gas in the container, we need to use Henry's law. Henry's law states that the partial pressure of a gas above a liquid is proportional to the concentration of the gas in the solution.
The equation we can use is:
P = kH * C
where P is the partial pressure of the gas, kH is the Henry's law constant, and C is the concentration of the gas in the solution.
Given data:
Temperature (T) = 25°C = 298 K
Concentration (C) = 1.4 x 10^-3 M
Henry's law constant (kH) = 6.1 x 10^-4 M/atm
Plug in the values into the equation:
P = (6.1 x 10^-4 M/atm) * (1.4 x 10^-3 M)
P = 8.54 x 10^-7 atm
Therefore, the partial pressure of N2 gas in the container is 8.54 x 10^-7 atm.