Calculate the electronegativity of carbon from the following data:
`E_(H-H)=104.2 kcal mol^(-1)` , `E_(C-C) =83.1kcal mol^(-1)` `E_(C-H)=98.8 kcal mol^(-1)` `X_H=2.1`

Calculate the electronegativity of fluorine from the following data E_H-H=104.2Kcal mol^(-1) , E_F-F=36.6 Kcal mol^(-1) , E_H-F=134.6 Kcal 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 enthalpy for the reaction at 27^0C . C_2 H_5 Cl (s) rarr C H_4 (g) +HCl (g) , Delta H^0(C -C) = 350 kjmol ^(-1) H^0(C-H) = 410 Kjmol^(-)1 , Delta H(C = C) =600 kjmol^(-1) -Delta H^0(C-Cl) = 340^0k jmol^(-1) , Delta H^0(H-Cl) = 430 kjmol^(-1) .

Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: (1) CH_(3)OH(l)+(3)/(2)O_(2)(g)toCO_(2)(g)+2H_(2)O(l),Delta_(r)H^(0)=-726kJ*mol^(-1) (2) C(s)+O_(2)(g) to CO_(2)(g),Delta_(c)H^(0)=-393kJ*mol^(-1) (3) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(l),Delta_(f)H^(0)=-286kJ*mol^(-1) .

Calculate the bond energy of O-H bond in H_(2)O(g) at the standard state from the following data: (1) H_(2)(g) to 2H(g),DeltaH^(0)=436kJ*mol^(-1) (2) (1)/(2)O_(2)(g)toO(g),DeltaH^(0)=249k*mol^(-1) (3) H_(2)(g)+(1)/(2)O_(2)(g)toH_(2)O(g),DeltaH_(f)^(0)[H_(2)O(g)]=-241.8kJ*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) )

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

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