Entropy is a state function and its depends on two or three variable temperature (T), pressure(P) and volume (V). Entropy change for an ideal gas having number of moles (n) can be determined by the following equation:
`DeltaS=2.303nC_(v)" "log((T_(2))/(T_(1)))+2.303 nR" "log ((V_(2))/(V_(1)))`
`DeltaS=2.303nC_(p)" "log((T_(2))/(T_(1)))+2.303 nR" "log ((P_(2))/(P_(1)))`
Since free energy change for a process or a chemical equation is a deciding factor of spontaneity, which can be obtained by using entropy change (`DeltaS)` according to the expression, `Delta G=DeltaH-TDeltaS` at a temperature T.
What would be the entropy change involved in thermodynamic expansion of 2 moles of a gas from a volume of 5 Lts to a volume of 50 Lts at `25^(@)C`? [Given R=8.3 J/mole-K]
A. 38.23J/K
B. 26.76J/K
C. 20J/K
D. 28.23J/K
