In: Chemistry
Case Study :-Volume of Wet Air (V)=947 ft3,Temperature(T) =70 0F,Pressure(Ps) =29.2 in Hg
Air id dehydrated and remove 0.94 lbs of water .Find out Relative Humidity of the wet air ?
Answer:-
(a)Volume of Wet Air (V)=947ft3=947/(3.281x3.281x3.281) m3=26.81 m3 thus V=26.81 m3
(b)Temperature (T)=70 0F=0.555(70-32)0C=21.090C=(21.09+273.16)0K=294.25 0K Thus T=294.25 0K
(c) Pressure (P)=29.2inHg=29.2x25.40 mmHg=741.68 mmHg=(741.68/760)atm=0.9759atm=(0.9759x101.325)KPa=98.88KPa Thus Ps=98.88 Kpa
Now According to Ideal Gas Law PV=nRT n=PV/RT=(98.88X26.81)/(8.314X294.25) here we are consider value of universal gas constant (R)=8.314 m3Kpa/KmoloK
n=1.084 Kmol ,Here n=Kmol of wet air present in system=1.084 Kmol
we are also known as 21% of oxygen (O2) and 79 % of Nitrogen (N2) present in Air
Oxygen (O2)=1.084x0.21 Kmol=0.23 Kmol
As per chemical reaction between oxygen (O2) and Hydrogen (H2)
H2+(1/2)O2H2O so that (1/2) Kmol of O2 produce 1 Kmol of H2O
Kmol of H2O present =0.23x2=0.46 Kmol Water present in system=0.46x18=8.28 Kg
Now Water are removed 0.94 lbs=0.94/2.20 kg=0.427 kg
Water Balance in systen after dehydration process=8.28-0.427=7.857 kg
Kmol of water present after dehydration process=7.857/18=0.437 Kmol
O2 present=0.438/2=0.219 kmol So moles of air present =0.219/0.21=1.04 kmol
n2=Kmol of wet air present after dehydration process in system=1.04 Kmol
According to Idea gas law PV=n2 RT P=n2 RT / V=(1.04X8.314X294.25)/(26.81) =94.90 KPa
Partial Pressure of Vapour (p)=94.90 KPa & Vapour pressure(Ps)=98.88 Kpa
Now Relative humidity(Rh) is ratio between partial pressure and vapour pressure
Rh=(p/Ps)x100=(94.90/98.88)x100=95.97 %
Relative Humidity after dehydration process or water removal is 95.97 %