Question

The concentration of dissolved nitrogen in water exposed to gaseous nitrogen at a partial pressure of 101.3 kPa at 20.0∘C is 6.90×10−4molL. Use Henry's law to determine the solubility of nitrogen when its partial pressure is 32.4 kPa.

Answer 1

The solubility of nitrogen at a partial pressure of 32.4 kPa can be calculated using Henry's law by finding the Henry's law constant (k) from the given concentration at 101.3 kPa and then applying it to the new pressure condition.

Step-by-step explanation:

Using Henry's Law to Calculate Nitrogen Solubility

To determine the solubility of nitrogen when its partial pressure is 32.4 kPa, we use Henry's law, which states that the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid. The formula for Henry's law is:

C = kP

where C is the concentration of the gas, k is Henry's law constant for the gas, and P is the partial pressure of the gas.

Given the concentration of dissolved nitrogen at a partial pressure of 101.3 kPa is 6.90×10⁻⁴ mol L⁻¹, we can calculate the Henry's law constant (k) for nitrogen at 20.0°C:

k = C / P = 6.90×10⁻⁴ mol L⁻¹ / 101.3 kPa

Now, using this law constant and the new partial pressure, we can calculate the new concentration:

C_new = k × P_new

C_new = (6.90×10⁻⁴ mol L⁻¹ / 101.3 kPa) × 32.4 kPa

By solving the equation, we'll find the new solubility of nitrogen at a partial pressure of 32.4 kPa.