The solubility of nitrogen, N2, in water is 4.52 ✕ 10−4 mol/L at 0°C when the nitrogen pressure above water is 0.741 atm. Calculate the solubility of nitrogen in water when the partial pressure of nitrogen above water is 1.086 atm at 0°C?

The concentration of nitrogen gas when the partial pressure is 1.086 atm above water is

Explanation:

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

where,

= Henry's constant = ?

= molar solubility of nitrogen gas =

= partial pressure of nitrogen gas = 0.741 atm

Putting values in above equation, we get:

Now, calculating the concentration when pressure is changed by using above equation:

= 1.086 atm

Putting values in above equation, we get:

Hence, the concentration of nitrogen gas when the partial pressure is 1.086 atm above water is

- "the choice that is not an indicator of a chemical change is "state of matter changes". more common than not, chemical reactions produce energy in the form of light or heat. along with energy, they also produce a new substance called the product that could be in any state of matter (solid, gas, or liquid)."

your parents i think this could be it