Predict the standard reaction enthalpy of `2NO_(2)(g)rarrN_(2)O_(4)(g)` at `100^(@)C`. `Delta H^(@)` at `25^(@)C` is `-57.2 kj.mol^(-1)C_(p)(NO_(2))=37.2j.mol^(-1)K^(-1)C_(p)(N_(2)O_(4))=77.28 J. mol^(-1)k^(-1)`

Calculate the change in enthalpy for the following process at 1 atm H_(2)O(1, 50^(@)C) rarr H_(2)O (g, 150^(@)C) given that Delta H_(v) at 100^(@)C is 40.7 kJ mol^(-1) C_(p)(H_(2)O, l) = 75.0 J mol^(-1)K^(-1) C_(p)(H_(2)O, g) = 33.3 J mol^(-1)K^(-1)

Calculate the enthalpy change on freezing of 1.0 mol of water at 10.0^(@)C to ice at -10.0^(@)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)

The enthalpy change on freezing of 1.0 mol of water at 10^(@)C to ice at -10^(@)C is : 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 enthalpy change of freezing of 1.0 mol of 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)

The enthalpy change on freezing of 1 mol of water at 5^(@)C to ice at -5^(@) C is (Given Delta_("fus") H = 6 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 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 equilibrium constant for the reaction : NO(g) + 1/2 O_(2)(g) iff NO_(2)(g) Given, Delta_(f)H^(@) at 298K : NO(g) = 90.4 kJ "mol"^(-1), NO_(2)(g) = 33.8 kJ "mol"^(-1) and DeltaS^(@) at 298 K = -70.8 J K^(-1) "mol"^(-1) , R = 8.31 J K^(-1) "mol"^(-1) .