The latent heat of evaporation of Bromine at `59^@C` at 1 atm is 29.2 KJ/mol what are `Delta H` and `Delta U` of this process?

The temperature of 1 mol of an ideal monoatomic gas at constant pressure of 1 atm changes from 25^(@)C and 50^(@)C . Calculate Delta U and Delta H in this process, (C_(V)=(3)/(2)R) .

Heat required to vaporise 1 g of water at 100^(@)C and 1 atm is 2.26 kJ. What is the enthalpy of vaporisation of water at this temperature and pressure?

Calculate the value of enthalpy of combustion of cyclopropane at 25^(@)C and 1 atm pressure. Given: Standard enthalpy of formation of CO_(2)(g),H_(2)O(l) & propene (g) at 25^(@)C are -393.5kJ*mol^(_1),-285.8kJ*mol^(-1)& 20.4kJ*mol^(-1) respectively. also standard enthalpy change for isomerisation reaction: Cyclopropane (g) hArr Propene (g) is -33.0kJ*mol^(-1) .

How are Delta H and Delta U are related? What is the difference between Delta Hand Delta U in a fusion process?

Two moles of a perfect gas undergoes the following process : (i) a reversible isobaric expansion from (1.0 atm, 20.0 L) to (1.0 atm, 40.0 L). (ii) a reversible isochoric change of state from (1.0 atm, 40.0 L ) to (0.5 atm, 40.0 L). (iii) a reversible isothermal expansion from (0.5 atm, 40.0 L )to (1.0 atm, 20.0 L) (i) Sketch with labels each procsses on the same P- V diagram. (ii) Calculate the total work (w) and the total heat (Q) involved in the above process. (iii) What will be values of Delta U, Delta H and Delta S for overall process ?

Latent heat in fusion of ice at 0^(@)C is 6025.24 J*mol^(-1) . Calculate molar entropy of the process at 0^(@)C .

At 25^(@)C the standard heat of formation of liquid benzene is +49.0 kJ*mol^(-1) -what does it mean?

The standard enthalpy of formation of H_2O(g) at 298 K is -241.82 kJ mol^-1 , Calculate DeltaH^@ at 373 K. Assume that C_p , is independent of temperature C "_p^o of H_2O(g) = 33.58 JK^-1 mol^-1 C "_p^o of H_2(g) = 28.84 JK^-1 mol^-1 C "_p^o of O_2(g) = 29.37 JK^-1 mol^-1

Standard enthalpy of vaporisation, Delta_(vap)H^theta for water at 100^@C Is 40.66 kJ mol^-1 . The internal energy of vaporisation of water at 100^@C (in kJ mol^-1 )is (Assume water vapour to behave like an ideal gas).