`G^(0)` and `H^(0)` for a reaction at 300K is `-66.9kJmol^(-1)` and `-41.8kJmol^(-1)` respectively. `S^(0)` for the same reaction at 300K is

(A) `-25.1kJmol^(-1)`
(B) `+25.1kJmol^(-1)`
`(C)18.7kJmol^(-1)`
(D) `0.08367kJmol^(-1)`

For a reaction A to B , Delta H_R=-10 kJ mol^-1 and E_a=50kJmol^-1 then E_a for the backward reaction B to A will be :

If EA_1 and EA_2 for oxygen atom -142kJmol"^(-1) and +844kJmol^(-1) . The energy released form 2O+2e^(-)rarr2O^(-) will be

Given that Bond energy of H_(2) and N_(2) are 400KJmol^(-1) and 240KJmol^(-1) respectively and DeltaH_(f) of NH_(3) is -120KJmol^(-1) calculate the bond energy of N-H bond :-

For the equilibrium: CO_((g))+H_(2)O_((g))hArrCO_(2(g))+H_(2(g)) the standard enthalpy and entropy changes at 300 K and 1200 K for the forward reaction are as follows: {:(DeltaH_(300 K)^(@)=-41.16kJmol^(-1),), (DeltaS_(300 K)^(@)=-0.0424kJmol^(-1)), (DeltaH_(1200 K)^(@)=-32.93kJmol^(-1),), (DeltaS_(1200K)^(@)=-0.0296kJmol^(-1)):} In which direction will the reaction be spontaneous? ( a ) At 300 K , ( b ) At 1200 K , when at equilibrium P_(CO)=P_(CO_(2))=P_(H_(2))=P_(H_(2)O)=1atm Also calculate K_(p) for the reaction at each temperature.

For an exothermic reaction ArarrB , the activation energy is 65kJmol^(-1) and enthalpy of reaction is 42kJmol^(-1) . The activation energy for the reaction BrarrA will be:

The bond energies of H--H , Br--Br and H--Br are 433,, 192 and 364KJmol^(-1) respectively. The DeltaH^(@) for the reaction H_(2)(g)+Br_(2)(g)rarr2HBr(g) is

Calculate the bond enthalpy of HCl. Given that the bond enthalpies of H_(2) and Cl_(2) are 430KJmol^(-1) and 242KJmol^(-1) respectively and Delta_(f)H^(0)HCl is -91KJmol^(-1) )