The solubility of nitrogen in water is mol/L at when the pressure above water is atm. Calculate the Henry’s law constant for in units of for Henry’s law in the form , where is the gas concentration in mol/L. Calculate the solubility of in water when the partial pressure of nitrogen above water is atm at 0°C.

The solubility of nitrogen in water is 8.21 x 10 -4 mol/L at 0°C when the N2 pressure above water is 0.790 atm. Calculate the Henry’s law constant for N2 in units of mol/L • atm for Henry’s law in the form C = kP, where C is the gas concentration in mol/L. Calculate the solubility of N2 in water when the partial pressure of nitrogen above water is 1.10 atm at 0°C.

The answer to the question is

1.143 × 10⁻³ mol/L

Explanation:

Henry's law states that the concentration of a gas in a solution is directly proportional to the partial pressure of the same gas existing above the solution at constant temperature

or c ∝ P which gives c = k × P

where c = concentration

k = constant of proportionality

P = Partial pressure of the same gas above the solution

The solubility of nitrogen = 8.21×10⁻⁴ M/L

The pressure above water = 0.790 atm

Therefore from C = kP

8.21×10⁻⁴ M/L = k×0.790 atm

k = 1.03924×10⁻³mol/(L·atm)

Hence when partial pressure = 1.10 atm we have

C = k×P = 1.03924×10⁻³mol/(L·atm) × 1.10 atm = 1.143×10⁻³ mol/L

answer

fusion: the energy source of stars. the energy released from the collapse of the gas into a protostar causes the center of the protostar to become extremely hot. when the core is hot enough, nuclear fusion commences. fusion is the process where two hydrogen atoms combine to form a helium atom, releasing energy.

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