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 entropy change at 0^(@) C for the process- H_(2)O(s) to H_(2)O(l) . Given: At 0^(2)C" "C_(2)O(s)toH_(2)O(g),DeltaH=51885J*mol^(-1) and H_(2)O(l)toH_(2)O(g),DeltaH=45860J*mol^(-1) .

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

Predict the sign of entropy change is the following reactions 2H_2(g)+O_2(g)rarr 2H_2O(g)

Using the datas given calculate the heat of formation of ethylene. C(s)+O_2(g)rarrCO_2(g) ,Delta H=-97300 cal H_2(g)+1/2O_2(g)rarr H_2O(l), Delta H=-68400 cal , C_2H_4(g)+3O_2(g)rarr 2CO_2(g)+2H_2O(l), Delta H=-333000 cal

H_2O(l)rarr H_2O(g) ,DeltaH=+43.7 KJ H_2O(s) rarr H_2O(l) ,Delta h=+6.05KJ the value of Delta H_(vaporisation) of ice is

Using the data provided calculate the multiple bond energy (KJ mol^(-)) of a C-=C bond in c_2H_2 consider the bond energy of a C-H bond is 350 KJ mol^(-1) 2C(s)+H_2(g)rarr C_2H_2(g), Delta H=225KJ mol^(-1) 2C(s)rarr2 C(g), Delta H=1410 KJ mol^(-1) H_2(g)rarr 2H(g), Delta H=330KJ mol^(-1)

For the reaction H_2O(s) iff H_2O(l) at 0^@C and normal pressure

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 DeltaH at 85^@ for the reaction : Fe_2O_3(s) + 3H_2 to 2Fe (s) + 3H_2O(l) The data are : Delta (298)^@ = -33.29 kJ/mol and