ulfur dioxide content of the outlet of a combustion reaction is monitored by passing it

through a SO $2$ analyzer. The SO$2$ analyzer reading was $1000$ ppm $($parts per million parts by

mole$).$ The sample gas leaves the analyzer at $1\mathrm{.}50$ L$/$min at $30\mathrm{.}0\backslash$deg C and $10\mathrm{.}0$ mmHg gauge and is

bubble through a tank that contains $140.$ L of initially pure water. In the bubbler, SO$2$ is absorbed

and some of the water evaporates. The gas leaving the bubbler is assumed to be in equilibrium

with the liquid in the bubbler at $30\mathrm{.}0\backslash$deg C and $1\mathrm{.}00$ atm absolute$.$ The SO$2$ content in the outlet gas

is monitored and when it hits $100$ ppm$,$ the water is replaced in the bubbler with fresh water.

A$)$ Why is this problem interesting to analyze? What principles apply to this problem?

B$)$ Use the following table to estimate the Henry$$s law coefficient for SO $2$ at $30\mathrm{.}0\backslash$deg C$.$

g SO$2$ dissolved$/100$ g

H$2$ O $($l$)$

$0\mathrm{.}00\mathrm{.}51\mathrm{.}01\mathrm{.}52\mathrm{.}0$

pSO$2($mmHg$)0\mathrm{.}04285129176$

C$)$ Estimate the SO$2$ concentration in the bubbler solution $($mol SO$2/$L$)$ when the bubbler

solution is to be changed. Determine the molar composition of the outlet gas stream for

air, SO$2$ and water $($v$).$ Assume: The inlet and outlet gas stream obey ideal gas law. The

inlet gas stream is dry air and SO$2.$ The water volume in the tank remains constant at $140$

L since the amount of water evaporated is low. The tank is well mixed and the amount of

SO$2$ in the tank at any time is given by Henry$$s law.

#$3$ A