We have a gas stream containing nitrogen vapor H$2$S$,$ in which the partial pressure of H$2$S is $47$ mm Hg$.$ The temperature of the gas mixture is $25$ degrees Celsius, its flow rate is $0\mathrm{.}38$ m$/$s$,$ and its pressure is atmospheric. We want to reduce the concentration of H$2$S in the gas mixture to $0\mathrm{.}51\%$ in an absorption tower by a liquid solvent that is initially free of H$2$S$.$ The solvent has a molecular weight of $195,$ a viscosity of $2\mathrm{.}1$ centipoise and a density of $0\mathrm{.}811$ at the same temperature. The vapor pressure of H$2$S at the above temperature is equal to $323$ mm Hg$.$ The tower works in isotherm conditions. The solubility of H$2$S gas in the solvent follows Raoult's law. a$)$ What is the minimum ratio of solvent to gas?

b$)$ The above absorption tower is filled with $45$ mm ceramic rushing rings. If we want to use $1\mathrm{.}5$ times the minimum required solvent so that the pressure drop does not exceed $31$ newtons per square meter per meter.

Calculate the diameter of the tower?

C is desirable Nta and Ntos

It is desirable to calculate Hts

It is desirable to calculate the height of the tower bed

Volumetric coefficients of mass transfer in terms of gram moles per cubic meter per second in the molar part in the problem conditions are:

Kya $=81,$ Kxa $=36$