Given a gas under 600*"mm Hg" pressure, and at 303.15*K temperature, that occupies a volume of 2.02*L, what volume will it occupy at 273.15*K temperature, under 750*"mm Hg" pressure?

1 Answer
Aug 2, 2017

Well, the current definition of "STP" is.... a temperature of 273.15*K and a pressure of exactly 10^5*Pa (100*kPa, 1*"bar").

Explanation:

And 1*"bar"-=(1*"bar")/(1.01325*atm*"bar"^-1)=0.987*atm

I do all this rigmarole BECAUSE I know that 1*atm will support a column of mercury that is 760*mm high...........

And hence in terms of the length of a mercury column, 1*"bar"-=760*mm*Hg*atm^-1xx0.987*atm=750.0*mm*Hg

(P_1V_1)/T_1=(P_2V_2)/T_2

We want V_2=(P_1V_1)/T_1xxT_2/P_2

(600.0*mm*Hgxx2.02*L)/(303.15*K)xx(273.15*K)/(750*mm*Hg)

~=1.5*L