A gaseous system is initially characterised by 500 mL volume and 1 atm pressure at 298 K. This system is allowed to do work as In isobaric conditions it expands to 800 mL resulting a decrease in pressure and temperature to 0.6 atm and 273 K respectively. (ii) In adiabatic conditions it is allowed to expand upto 800 mL and results a decrease in pressure and temperature to 0.6 atm and 273 K respectively. If Gibbs energy change in (i) is DeltaG_(a) and in (ii) is DeltaG_(b), then what will be the ration of (DeltaG_(a))/(DeltaG_(b))?

A gaseous system is initially characterised by 500 mL volume and 1 atm

1.	A gaseous system is initially characterised by 500 mL volume and 1 atm pressure at 298 K. This system is allowed to do work as In isobaric conditions it expands to 800 mL resulting a decrease in pressure and temperature to 0.6 atm and 273 K respectively. (ii) In adiabatic conditions it is allowed to expand upto 800 mL and results a decrease in pressure and temperature to 0.6 atm and 273 K respectively. If Gibbs energy change in (i) is DeltaG_(a) and in (ii) is DeltaG_(b), then what will be the ration of (DeltaG_(a))/(DeltaG_(b))?
Answer» 0 1 between 0 -1 gt 1 Solution :`(DeltaG_(a))/(DeltaG_(b))=1`, as Gibbs ENERGY is a state FUNCTION and INTIAL and final states are same in (i) and (ii).