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28 March, 23:26

The solubility of nitrogen gas at 25 degrees C and 1 atm is 6.8 x 10^ (-4) mol/L. If the partial pressure of nitrogen gas in air is 0.76 atm, what is the concentration (molarity) of dissolved nitrogen?

5.2 x 10^ (-4) M

1.1 x 10^ (-5) M

4.9 x 10^ (-4) M

3.8 x 10^ (-4) M

6.8 x 10^ (-4) M

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  1. 29 March, 00:25
    0
    5.2 x 10⁻⁴ M.

    Explanation:

    The relationship between gas pressure and the concentration of dissolved gas is given by Henry's law:

    P = kC

    where P is the partial pressure of the gaseous solute above the solution.

    k is a constant (Henry's constant).

    C is the concentration of the dissolved gas.

    At two different pressures, there is two different concentrations of dissolved gases and is expressed in a relation as:

    P₁C₂ = P₂C₁,

    P₁ = 1.0 atm, C₁ = 6.8 x 10⁻⁴ mol/L.

    P₂ = 0.76 atm, C₂ = ? mol/L.

    ∴ C₂ = (P₂C₁) / P₁ = (0.76 atm) (6.8 x 10⁻⁴ mol/L) / (1.0 atm) = 5.168 x 10⁻⁴ mol/L ≅ 5.2 x 10⁻⁴ M.
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