Henry's law constant of oxygen is `1.4 xx 10^(-3)` mol `"lit"^(-1) "atm"^(-1)` at 298 K. How much of oxygen is dissolved in 100 mL at 298 K when the partial pressure of oxygen is 0.5 atm?

Options

A. 1.4g
B. 3.2g
C. 22.4mg
D. 2.24mg

Answer

D

Explanation

` p = (1)/(k) xx ` Solubility .
solubility =k.p
` = 0.5 xx 1.4 xx 10^(-3) mol//L`
` = 0.5 xx 1.4 xx 10^(-3) xx 32 g//L`
` = 22.4 xx 10^(-3) g//L`
Amount dissolved in 100 ml
` = (22.4 xx 10^(-3))/(10)`
` = 2..24 xx 10^(-3) g = 2.24 mg` .