Internal energy, enthalpy and entropy are thermodynamics state functions.
What is enthalpy of a system?

Internal energy, enthalpy and entropy are thermodynamics state functions. Calculate enthalpy of combustion of methane, given that the standard enthalpies of formation of CH_4 , CO_2 and H_2O are -75.2, -394.0 and -285.6 kJ//mol respectively.

A thermodynamic state function is a quantity.

a) What is enthalpy of solution? b) What is enthalpy of dilution?

Internal energy U of a system may change when

The spontaneity of a process is expressed in terms of a change in Gibbs energy. a) What is meant by a change in Gibbs energy of a system? b) How is it related to the enthalpy and entropy of a system? c) How is it useful in predicting the feasibility of a process?

Some properties of a system are state functions. What is the difference in internal energy of a system, if 100 kJ of energy is radiated out without doing any work?

a) Give the relation between change in enthalpy and change in free energy. b) Name the above relation. c) What is the significance of the above relation?

The standard enthalpy change for the neutralisation of HCN with NaOH is -2460 cal at 298 K. Given that standard enthalpy change for the neutralisation HCl with NaOH is -13.7 kcal. What is enthalpy of ionisation of HCN in kcal ?

a) What is meant by enthalpy? b) Derive an equation for enthalpy change. c) What is enthalpy change?