One mole of an ideal diatomic gas `(C_(v) =5 cal)` was transformed from initial `25^(@)` and `1 L` to the state when temperature is `100^(@)` C and volume `10` L. Then for this process(R=`2 "calories" //"mol"//K"`)(take calories as unit of energy and kelvin for temp)

Options

A. `DeltaH=525`
B. `DeltaS=5 "In" 373/298 +2 "In" 10`
C. `DeltaE=525`
D. `DeltaG` of the process cannot be calculated using given information.

Answer

A,B,D

Explanation

`DeltaS=nC_v "In" (T_f/T_i)+nR "In" (V_f/V_i)=5 "In"373/298+2"In"10/1`
`DeltaH=nC_pDeltaT=7(75)=525` cal
`DeltaE=nC_vDeltaT=5(75)=375` cal
`DeltaG=DeltaH-Delta(TS)`