The solubility of N2 in blood at 37 °C and at a partial pressure of 0.80 atm is 5.6×10−4mol L−1. The Henry’s law constant for this system is

The solubility of N2 in blood at 37 °C and at a partial pressure of 0.80 atm is 5.6×104mol L1. The Henry's law constant for this system is

  1. A

    1.43×103 atm L mol1

  2. B

    1.62×103atm L mol1

  3. C

    5.6×104 atm L mol1

  4. D

    2.86×102atm L mol1

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    Solution:

    Henry's law in terms of concentration of dissolved gas is p=kHc. Hence,

    kH=pc=0.80atm5.6×104mol L1=1.43×103atm L mol1

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