hi, i think this prob has to do what you did the last time
but how does pressure play appart in this chapter??
What pressure would have to be applied to steam at 325°C to condense the steam to liquid water (ÄH vap = 40.7 kJ/mol)?
3 answers
http://www.lsbu.ac.uk/water/phase.html
Use the Clausius-Clapeyron Equation to calculate the vapor pressure at 325°C. That is the pressure that must be applied to condense the steam at 325°C.
Ln(P2/P1) = (∆H/R)[(T2-T1)/T2T1]
P1 = 1 atm
∆H = 40700J
R = 8.3145 J/°K.mol
T2 = (325+273) = 598°K
T1 = (100+273) = 373°K
P2 = (unknown)
[NOTE: The pressure needed is quite high]
Ln(P2/P1) = (∆H/R)[(T2-T1)/T2T1]
P1 = 1 atm
∆H = 40700J
R = 8.3145 J/°K.mol
T2 = (325+273) = 598°K
T1 = (100+273) = 373°K
P2 = (unknown)
[NOTE: The pressure needed is quite high]
i solved for lnx=4,852,725
whats next? and i relaly cant put it into the calc. it says (overflow)
whats next? and i relaly cant put it into the calc. it says (overflow)
0 answers