Henry’s law constant (mol/L · atm) for oxygen dissolving in blood is 3.74 x 10–2 mol/(L...

Henry’s law constant (mol/L · atm) for oxygen dissolving in blood is 3.74 x 10–2 mol/(L atm) at body temperature, 37°C. Calculate the molar concentration of oxygen in blood for a scuba diver where the air pressure is 2.0 atm. The mole fraction of oxygen in air is 0.209.

0.11 M

2.7 x 10–3 M

1.3 x 10–2 M

1.6 x 10–2 M

7.8 x 10–3 M

Solutions

Expert Solution

C = k Pgas

partial pressure of oxygen in that air is = molefraction * Air pressure

= 0.209*2.0 atm

= 0.418 atm

C = 3.74*10^-2*0.418

= 1.6*10^-2 M

queen_honey_blossom answered 1 year ago

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