The solubility of nitrogen in water is 8.21 E-4 mol/L at 0°C when the nitrogen pressure above water is 0.790 atm. Calculate the solubility of nitrogen in water when the partial pressure of nitrogen above water is 9.55 atm at 0°C?

pN2 = KcC

0.790 = Kc(8.21E-4)
Solve for Kc. Then
pN2 = KcC, substitute new P and solve for new C(in mols/L)

To calculate the solubility of nitrogen in water when the partial pressure is 9.55 atm at 0°C, we can use Henry's Law.

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, we can express this as:

C = k * P

Where C is the solubility of the gas, k is the Henry's law constant, and P is the partial pressure of the gas.

First, we need to find the value of k. We can use the given data to solve for k:

C1 = k * P1

Rearranging the equation:

k = C1 / P1

Using the given data:
C1 = 8.21 E-4 mol/L
P1 = 0.790 atm

k = (8.21 E-4 mol/L) / (0.790 atm)
k ≈ 0.00104 mol/L·atm

Now that we have the value of k, we can use it to calculate the solubility of nitrogen in water when the partial pressure is 9.55 atm:

C2 = k * P2

Using the given data:
P2 = 9.55 atm

C2 = (0.00104 mol/L·atm) * (9.55 atm)
C2 ≈ 0.00994 mol/L

Therefore, the solubility of nitrogen in water when the partial pressure of nitrogen above water is 9.55 atm at 0°C is approximately 0.00994 mol/L.

To calculate the solubility of nitrogen in water, we can use Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

Henry's law can be expressed as follows:
C = k * P

Where:
C = solubility of the gas in the liquid (in this case, nitrogen in water)
k = Henry's law constant
P = partial pressure of the gas above the liquid

The given information provides the values for the solubility of nitrogen in water and the nitrogen pressure at 0°C. We can use these values to determine the Henry's law constant (k).

C1 = 8.21 E-4 mol/L (when P1 = 0.790 atm)
C2 = ? (when P2 = 9.55 atm)

To find the Henry's law constant (k), we can rearrange the formula:
k = C / P

Substituting the values into the formula:
k = (8.21 E-4 mol/L) / (0.790 atm)

Now we can calculate the value of k.

k = 1.03924 E-3 mol/L*atm

Finally, we can use this value of k to calculate the solubility of nitrogen in water when the partial pressure of nitrogen is 9.55 atm at 0°C.

C2 = k * P2

Substituting the values into the formula:
C2 = (1.03924 E-3 mol/L*atm) * (9.55 atm)

Now we can calculate the solubility of nitrogen in water.

C2 = 9.91962 E-3 mol/L

Therefore, the solubility of nitrogen in water when the partial pressure of nitrogen above water is 9.55 atm at 0°C is approximately 9.92 E-3 mol/L.