Enthalpy of reaction `DeltaH` is expressed as

Enthalpy of a reaction Delta H is expressed as

For an endothermic reaction, energy of activation is E_a and enthalpy of reaction is DeltaH (both of these in kJ/mol). Minimum value of E will be

For a reaction, C_((s))+O_(2(g))rarrCO_(2(g)) What is the relation between enthalpy of reaction (DeltaH_(r)), enthalpy of formation of CO_(2)(DeltaH_(f)) and enthalpy of combustion of carbon (DeltaH_("comb")) ?

For a reaction, C_((s))+O_(2(g))rarrCO_(2(g)) What is the relation between enthalpy of reaction (DeltaH_(r)), enthalpy of formation of CO_(2)(DeltaH_(f)) and enthalpy of combustion of carbon (DeltaH_("comb")) ?

For an endothermic reaction energy of activation is E_(a) and enthalpy of reaction is DeltaH (both in kJ "mol"^(-1) ) Minimum value of E_(a) will be

For the conversion of 1 mole of SO_(2)(g) into SO_(3)(g) the enthalpy of reaction at constant volume. DeltaU , at 298 K is -97.027kJ . Calculate the enthalpy of reaction, DeltaH , at constant pressure.

If the enthalpy change of a reaction is DeltaH how will you calculate entropy of surroundings?