The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10 –4 mol/L. What is the value of the Henry's Law constant in mol/L·atm?

6.8 × 10⁻⁴ mol/L.atm

Explanation:

Step 1: Given data

Solubility of nitrogen gas at 25°C (S): 4.7 × 10⁻⁴ mol/L

Partial pressure of nitrogen gas (P): 522 mmHg

Step 2: Convert the partial pressure of nitrogen to atm

We will use the relationship 1 atm = 760 mmHg.

Step 3: Calculate the value of the Henry's Law constant (k)

We will use Henry's law.

space exploration has led to the development and technological improvement of many everyday items. (if this answer is wrong i will find the right answer) : )