Calculate the enthalpy change on freezing of 1.0 mole of water at `10^@C` to ice at`-10^@C,triangle_(fus)H = 6.03 kJ mol^-1` at `0^@C`,
`C_p[H_2O(l)] = 75.3 J mol^-1 K^-1`
`C_p[H_2O(s)] = 36.8 J mol^-1 K^-1`

Calculate enthalpy change on freezing 1 mol water at 10^(@)C to ice at -10^(@)C. Delta_("fus")H= 6.03 " kJ mol"^(-1) " at " 0^(@)C . C_(p)[H_(2)O(l)]= 75.3 " J. mol"^(-1). K^(-1) , C_(p)[H_(2)O(s)]= 36.8 " J mol"^(-1). K^(-1) .

Calculate the entropy change in surroundings when 1.00 mole of H_2O(l) is formed under standard conditions. triangle_fH^@ = 286 kJ mol^-1 .

Calculate the enthalpy of sublimation of Na metal from the following data given Delta H_fus^@=2.6 KJ mol^(-1) Delta H_vap^@=98 KJ mol^(-1)

Calculate the entropy change in the surrounding when 1,00 mol of H_(2)O(l) is formed under standard conditions. Delta_(f)H^(0)=-286kJ*mol^(-1)

If the enthalpy change for the transition of liquid water to steam is 30kJ*mol^(-1) at 27^(@)C , the entropy change in J*mol^(-1)*K^(-1) for the process would be-

Calculate the enthaply change for the process : C Cl_4 (g) to C (g)+ 4Cl(g) and calculate the bond enthalpy of C-Cl in C Cl_4(g) triangle(vap))H^(@) (C Cl_4 )= 30.5 kJ mol^-1 trianglef H^(@)(C Cl_4) = -135.5 kJ mol^-1 triangle_a H^@(C) = 715.0 kJ mol^-1 triangle_a H^@(Cl_2)( atomisation ) = 242 kJ mol^-1

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

Calculate the entropy change, at 0^@C for the process H_2O(s) rarr H_2O(I) . Given : At 0^@C , H_2O(s) rarr H_2O(g) , Delta H=51885 J. mol^-1 and H_2O(I) rarr H_2O(g) , Delta H=45860 J. mol^-1 .

Calculate the molar entropy of vaporisation of water , (Given : H_(2)O (l) hArr H_(2)O (g) , Delta H = 40.8 kJ* mol^(-1) )

If water vapour is assumed to be a perfect gas and molar enthalpy change for vapourisation of 1 mole of water at 1 bar & 100^@C is 41 kJ mol^-1 , calculate the intenal energy change when 1 mol of water is vapourised at 1 bar pressure & 100^@C