Question
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 x 10-3 M/atm.
Answers
bobpursley
massO2=Hconstant*pressure*volume*molmass
= 1.3E-3*1.13*5L*32 grams=235mg\\check it.
= 1.3E-3*1.13*5L*32 grams=235mg\\check it.
This answer worked better for me
P = P°*X
=> C = P°*X*k = 1.13atm * 0.21 * 1.3*10^-3M/atm = 3.085*10^-4M
3.085*10^-4M * 5L = 1.54*10^-3mol = 1.54mmol
1.54*MM(O2) = 1.54mmol * 32mg/mmol = 49.4mg
P = P°*X
=> C = P°*X*k = 1.13atm * 0.21 * 1.3*10^-3M/atm = 3.085*10^-4M
3.085*10^-4M * 5L = 1.54*10^-3mol = 1.54mmol
1.54*MM(O2) = 1.54mmol * 32mg/mmol = 49.4mg
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