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 :

Charge in enthalpy and change in internal energy are equal at room temperature for

Why are we usually concerned with changes in enthalpy than changes in internal energy?

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