Question

The Henry's law constant for nitrogen in water at 25oC is 6.10 x 10-4 M/atm. What is the concentration (molarity) of nitrogen in water at a pressure of 23.6 atm?

Answer 1

The concentration of nitrogen in water at a pressure of 23.6 atm, given a Henry's Law constant of 6.10 x 10^-4 M/atm, is 0.0144 M.

Step-by-step explanation:

To calculate the molarity of nitrogen in water at a given pressure using Henry's Law, we use the formula:

Concentration (C) = Henry's Law constant (k) × Pressure (P)

Given the Henry's Law constant for nitrogen in water at 25°C is 6.10 × 10-4 M/atm and the pressure is 23.6 atm, we can plug these values into the formula:

C = 6.10 × 10-4 M/atm × 23.6 atm

This results in:

C = 0.0144 M, which is the concentration of nitrogen in water at 23.6 atm pressure.

To get to this result, you multiply the Henry's Law constant by the pressure. It is important to note that units of pressure and the constant must match to cancel each other out correctly, leaving the concentration in molarity.

Answer 2

Answer: The concentration of nitrogen gas is 0.0144 M

Step-by-step explanation:

To calculate the molar solubility, we use the equation given by Henry's law, which is:

`C_(N_2)=K_H* p_(N_2)`

where,

`K_H` = Henry's constant =
`6.10* 10^(-4)mol/L.atm`

`C_(N_2)` = molar solubility of nitrogen gas

`p_(N_2)` = partial pressure of nitrogen gas = 23.6 atm

Putting values in above equation, we get:

`C_(N_2)=6.10* 10^(-4)mol/L.atm* 23.6atm\\\\C_(N_2)=0.0144mol/L`

Hence, the concentration of nitrogen gas is 0.0144 M