Calculate the maximum work done when pressure on `10 g` of hydrogen is reduces from `20 atm` to `1 atm` at a constant temperature of `273 K`. The gas behaves ideally. Will there be any change in internal energy? Also, calculate `'q'`.

Explanation

we have, `W= -2.303 nRT"log"(P_(1))/(P_(2))`
`n= "number of moles of hydrogen"=("Wt.in grams")/("mol.wt.")=(10)/(2)=5"moles"`
Thus, `W = -2.303xx5xx2xx273xx"log"(20)/(1) = -8180 "calories"`.
Further, the change in state of system at constant temperature will not change internal energy i.e., `Delta U =0`.
Again, `q=DeltaU-W=0-(-8180)=8180"calories"`.