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 standard enthalpy for the reaction at 298K: C_(2)H_(5)Cl(g)toC_(2)H_(4)(g)+HC l(g) . Given: DeltaH^(0)(C-H)=413kJ*mol^(-1),DeltaH^(0)(C-C)=346kJ*mol^(-1) , DeltaH^(0)(C=C)=611kJ*mol^(-1),DeltaH^(0)(C-Cl)=339kJ*mol^(-1) , DeltaH^(0)(H-Cl)=432kJ*mol^(-1) .

Calculate the value of standard reaction enthalpy for the following reaction : C_2H_5Cl (g) rarr C_2H_4 (g) + HCl (g) at 298 K temperature.Given that DeltaH^@ (C-H) = 413 KJ mol^-1, DeltaH^@ (C-C) = 346 KJ mol^-1 ,DeltaH^@ (C=H) =611 KJ mol^-1, DeltaH^@ (C-CI) = 339 KJ mol^-1 DeltaH^@ (H-Cl) = 432 KJ- mol^-1 .

Delta H- Delta U for the reaction C_3H_8(g) +SO_2 (g) = 3CO_2 (g) + 4H_2O (g) .

Calculate Delta H-DeltaU at 25^@C for the reaction: H_2(g)+( 1/2)O_2(g) = H_2O(l) .

for the reaction 2Cl(g)rarr Cl_2(g) What are the signs of Delta H and Delta S ?

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 .

Determine the standard enthalpy of formation of isoprene(g) at 298K temperature. Given: at 298K, DeltaH^(0)(C-H)=413kJ*mol^(-1) DeltaH^(0)(H-H)=436kJ*mol^(-1) DeltaH^(0)(C-C)=346kJ*mol^(-1) , DeltaH^(0)(C=C)=611kJ*mol^(-1) , C("graphite, s")toC("graphite, g"), DeltaH^(0)=717kJ*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 of combustion of ethylene . Given : C_(2) H_(6) (g) + (7)/(2) O_(2) (g) to 2 CO_(2) + 3 H_(2)O (l) , Delta H = = 1562 kJ* mol^(-1) H_(2) (g) + (1)/(2) O_(2) (g) to H_(2) O (l) , Delta H = -286 kJ * mol^(-1) C_(2) H_(4) (g) + H_(2) (g) to C_(2) H_(6) (g) , Delta H = -32 kJ * mol^(-1)