Calculate change in internal energy if `Delta H= - 92.2 kJ, P = 40` atm and `Delta V = - 11`.

One mole of a non-ideal gas undergoes a change of state ( 2.0 atm, 3.0L, 95 K) rarr (4.0 atm, 5.0L, 245 K) with a change in internal energy , Delta U= 30.0 L. atm . Calculate change in enthalpy of the process in L. atm .

One mole of a non-ideal gas undergoes a change of state ( 2.0 atm, 3.0L, 95 K) rarr (4.0 atm, 5.0L, 245 K) with a change in internal energy , Delta U= 30.0 L. atm . Calculate change in enthalpy of the process in L. atm .

One mole of a non-ideal gas undergoes a change of state (2.0 atm, 3.0 L, 90K) rarr (4.0 atm, 5.0 L, 245 K) with a change in internal energy, Delta U = 30.0 L atm . The change in enthalpy (Delta H) of the process in L atm is (Give your answer after dividing with 11)

Chemical reactions are invariably associated with the transfer of energy either in the form of hear or light. In the laboratory, heat changes in physical and chemical processes are measured with an instrument called calorimeter. Heat change in the process is calculated as: q= ms Delta T , s= Specific heat = c Delta T = Heat capacity. Heat of reaction at constant pressure is measured using simple or water calorimeter. Q_(v)= Delta U = Internal energy change, Q_(P) = DeltaH, Q_(P) = Q_(V) + P Delta V and DeltaH = Delta U+ Delta nRT . The amount of energy released during a chemical change depends on the physical state of reactants and products, the condition of pressure, temperature and volume at which the reaction is carried out. The variation of heat of reaction with temperature and pressure is given by Kirchoff's equation: (DeltaH_(2) - DeltaH_(1))/(T_(2)-T_(1))= Delta C_(P) (At constant pressure), (DeltaU_(2) - DeltaU_(1))/(T_(2)-T_(1)) = DeltaC_(V) (At constant volume) The enthalpy change (DeltaH) for the reaction N_(2) (g) + 3H_(2)(g) rarr 2NH_(3)(g) is -92.38kJ at 298 K. The internal energy change DeltaU at 298 K is

Chemical reactions are invariably associated with the transfer of energy either in the form of hear or light. In the laboratory, heat changes in physical and chemical processes are measured with an instrument called calorimeter. Heat change in the process is calculated as: q= ms Delta T , s= Specific heat = c Delta T = Heat capacity. Heat of reaction at constant pressure is measured using simple or water calorimeter. Q_(v)= Delta U = Internal energy change, Q_(P) = DeltaH, Q_(P) = Q_(V) + P Delta V and DeltaH = Delta U+ Delta nRT . The amount of energy released during a chemical change depends on the physical state of reactants and products, the condition of pressure, temperature and volume at which the reaction is carried out. The variation of heat of reaction with temperature and pressure is given by Kirchoff's equation: (DeltaH_(2) - DeltaH_(1))/(T_(2)-T_(1))= Delta C_(P) (At constant pressure), (DeltaU_(2) - DeltaU_(1))/(T_(2)-T_(1)) = DeltaC_(V) (At constant volume) The enthalpy change (DeltaH) for the reaction N_(2) (g) + 3H_(2)(g) rarr 2NH_(3)(g) is -92.38kJ at 298 K. The internal energy change DeltaU at 298 K is

For the reaction, N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g), Delta H = -95.2 kJ and Delta S = -198.1 JK^(-1) . Calculate the temperature at which Gibb's energy change of the reaction (Delta G) becomes equal to zero.

Let Delta U_(1) and Delta U_(2) be the changes in internal energy of an ideal gas in the processes A and B then

During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. The change in internal energy, Delta U (in kJ) is _________ .

During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. The change in internal energy, Delta U (in kJ) is _________ .