The enthalpy change for the conversion of `(1)/(2)Cl_(2)(g)` to `Cl^(-)` (aq) is `(-)`_____
`KJmol^(-1)` (Nearest integer)
Given : `Delta_(dis) H_(Cl_(2)(g))=240kJmol^(-1),Delta_(eg)HCl_((g))=-350kJmol^(-1)` `Delta_(h)dH^(-)(g_((g)))=-380kJmol^(-1)`

Oxidising power of chlorine in aqueous solution can be determined by the parameters indicated below (1)/(2)CL_(2)(g)overset((1)/(2)Delta_(diss)H^(Theta))(rarr)Cl(g)overset(DeltaH_(Eg)^(Theta))(rarr) Cl^(-)(g)overset(Delta_(hyd)H^(Theta))(rarr)Cl^(-)(aq) The energy involved in the conversion of (1)/(2)Cl_(2)(g) to Cl^(-)(aq) (Using the data Delta_(diss)H_(Cl_(2))^(Theta)=240KJ mol^(-1) ) Delta_(Eg)H_(Cl)^(Theta)=-349KJmol^(-1) , Delta_(Eg)H_(Cl)^(Theta)=-381KJmol^(-1) ) will be

Enthalpy change for reaction 1//2H_(2)(g)+1//2Cl_(2)(g)toHCl(g) is called :-

oxidising power of chlorine in aqueous solution can be determined by the parameters indicated below: Calculate the energy involved in the conversion of (1)/(2)Cl_(2)(g)"to"Cl^(-)(aq) Using the data , DeltaH_("disso"(Cl_(2)))^(@)=240KJmol^(-1), DeltaH_("eg"(Cl_(2)))^(@)=-349KJmol^(-1), DeltaH_("hydroation"(Cl_(2)))^(@)=-381KJmol^(-1),

Calculate the enthalpy change for the process C Cl_(4)(g) rarr C(g)+4Cl(g) and calculate bond enthalpy of C-Cl in C Cl_(4)(g) . Delta_(vap)H^(Θ)(C Cl_(4))=30.5 kJ mol^(-1) Delta_(f)H^(Θ)(C Cl_(4))=-135.5 kJ mol^(-1) Delta_(a)H^(Θ)(C )=715.0 kJ mol^(-1) , where Delta_(a)H^(Θ) is enthalpy of atomisation Delta_(a)H^(Θ)(Cl_(2))=242 kJ mol^(-1)