Enthalpy and internal energy

A reversible cyclic process for an ideal gas is shown below. Here, P, V, and T are pressure, volume and temperature, respectively. The thermodynamic parameters q, w, H and U are heat, work, enthalpy and internal energy, respectively. The correct option (s) is (are)

Which of the following are intensive properties? Boiling point Melting point Heat capacity Volume Enthalpy Mass Internal energy Molar volume

Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemical equation . The amount of energy released during a chemical change depends upon the state of reactants and products, the conditions of pressure and volume at which reaction is carried out, and temperature. The variation of heat of reaction (DeltaH_(1) or DeltaE) with temperature is given as DeltaH_(2)-DeltaH_(1)=DeltaC_(P)[T_(2)-T_(1)] or DeltaE_(2)-DeltaE_(1)=DeltaC_(v)(T_(2)-T_(1). Standard heat enthalpy of elements in their most stable state is assumed to be zero whereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atm pressure and 25^(@)C . Oxidation of N_(2) to N_(2)O,NO,NO_(2) shows absorption of energy whereas heat of combustion of N_(2) is exothermic like other heat of combustion. Standard heat enthalpy has been assumed to be zero for :

Heat of reaction at constant pressure is equal to .............change. Write the expression between enthalpy change and internal energy

Write the expression showing relation between enthalpy change and internal energy change for gaseous phase reaction

The relationship between enthalpy change (DeltaH) and internal energy change (DeltaE) for a system is given by

For the reaction PCl_(5)(g)toPCl_(3)(g)+Cl_(2)(g) where ΔH and ΔE represents enthalpy change and internal energy change respectively.