How much oxygen is dissolved in 100 mL water at
298 K if partial pressure of oxygen is 0.5 atm and
Ky = 1.4 x 10 mol/L/atm?
(a) 22.4 mg
(b) 22,4 g
(c) 2.24 g
(d) 2.24 mg
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according to Henry's law,
where S is concentration of O2 is dissolved , is Henry's constant and partial pressure of O2
here, = 1.4 × 10^-3 mol/L/atm and = 0.5atm
so, S = 1.4 × 10^-3 × 0.5 = 0.7 × 10^-3 M
now, molarity = number of mole of solute /volume of solution
or, 0.7 × 10^-3 = mass of O2/molecular weight of O2 × volume of solution in L
or, 0.7 × 10^-3 = mass of O2/(32g/mol × 100/1000 L)
or 0.7 × 10^-3 × 3.2 = mass of O2
or, mass of O2 = 2.24 × 10^-3 g = 2.24mg
hence, option (d) is correct choice.
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