The free energy for a reaction having `DeltaH=31400` cal, `DeltaS=32" cal "K^(-1)mol^(-1)` at `1000^(@)C` is:

The change in Gibbs free energy of the system along provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a sytem at constant temperature and pressure will be: DeltaG_("system") = DeltaH_("system") - T DeltaS_("system") The free energy for a reaction having Delta H= 31400 cal, DeltaS= 32 cal K^(-1) mol^(-1) at 1000^(@)C is

The change in Gibbs free energy of the system along provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a sytem at constant temperature and pressure will be: DeltaG_("system") = DeltaH_("system") - T DeltaS_("system") The free energy for a reaction having Delta H= 31400 cal, DeltaS= 32 cal K^(-1) mol^(-1) at 1000^(@)C is

The change in Gibbs free energy of the system alone provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a system at constant temperature and pressure will be : DeltaG_("system")=DeltaH_("system")-T DeltaS_(system") The free energy for a reaction having DeltaH=31400 cal, DeltaS=32 cal L^(-1) mol^(-1) at 1000^(@)C

A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) The free enegry for a reaction having DeltaH = 31400 cal, DeltaS = 32 cal K^(-1) mol^(-1) at 1000^(@)C is

A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) The free enegry for a reaction having DeltaH = 31400 cal, DeltaS = 32 cal K^(-1) mol^(-1) at 1000^(@)C is

Solve : DeltaH=10k " cal mol"^(-1),DeltaS=20 " cal deg"^(-1)mol^(-1) and T = 300k. " Then " DeltaG= ?

The half-life period for first order reaction having activation energy 39.3 k cal mol^(-1) at 300^@ C and frequency constant 1.11xx10^(11) s^-1 will be

The equilibrium constant K_(p) for a homogeneous gaseous reaction is 10^(-8) . The standard Gibbs free energy change DeltaG^(ɵ) for the reaction ("using" R=2 cal K^(-1) mol^(-1)) is

The equilibrium constant K_(p) for a homogeneous gaseous reaction is 10^(-8) . The standard Gibbs free energy change DeltaG^(ɵ) for the reaction ("using" R=2 cal K^(-1) mol^(-1)) is