[" 16.The enthalpy change for the following processes are "],[" listed below "],[Cl_(2)(g)=2Cl(g),,242.3kJmol^(-1)],[I_(2)(g)=2I(g),,151.0kJmol^(-1)],[ICl(g)=I(g)+Cl(g),,211.3kJmol^(-1)],[I_(2)(s)=I_(2)(g),,62.76kJmol^(-1)],[" Given that the standard states for iodine and chlorine "],[" are "I_(2)(s)" and "Cl_(2)(g)," the standard enthalpy of formation "]

The enthaplpy changes state for the following processes are listed below: Cl_(2)(g)=2Cl(g) : 242.3KJmol^(-1) I_(2)(g)=2I(g) , 151.0KJ mol^(-1) ICl(g)=I(g)+Cl(g) : 211.3KJ mol^(-1) I_(2)(s)=l_(2)(g) , 62.76KJ mol^(-1) Given that the standard states for iodine chlorine are I_(2)(s) and Cl_(2)(g) , the standard enthalpy of formation for ICl(g) is:

The enthaplpy changes state for the following processes are listed below: Cl_(2)(g)=2Cl(g) : 242.3KJmol^(-1) I_(2)(g)=2I(g) , 151.0KJ mol^(-1) ICl(g)=I(g)+Cl(g) : 211.3KJ mol^(-1) I_(2)(s)=l_(2)(g) , 62.76KJ mol^(-1) Given that the standard states for iodine chlorine are I_(2)(s) and Cl_(2)(g) , the standard enthalpy of formation for ICl(g) is:

The enthalpy changes for the following process are listed below : Cl_(2)(g)=2Cl(g)," "242.3" kJ"mol^(-1) I_(2)(g)=2I(g)," "151.0" kJ"mol^(-1) ICl(g)=2I(g)+Cl(g)," "211.3" kJ"mol^(-1) I_(2)(s)=I_(2)(g)," "62.76" kJ"mol^(-1) Given that standard states for iodine and chlorine are I_(2)(s) and Cl_(2)(g) , the standerd enthalpy of formation for ICl(g) is :

The enthalpy changes for the following processes are listed below: Cl_(2(g)) rarr 2Cl_((g)) , DeltaH = 242.3 kJ mol^(-1) I_(2(g)) rarrr 2I_((g)) , DeltaH = 151.0 kJ mol^(-1) ICl_((g)) rarr I_((g)) + Cl_((g)) , DeltaH = 211.3 kJ mol^(-1) I_(2(s)) rarr I_(2(g)) , DeltaH = 62.76 kJ mol^(-1) Given that the standard states for iodine and chlorine are I_(2(s)) and Cl_(2(g)) , the standard enthalpy of formation for ICT is:

The enthalpy change for the following process are listed below : (a) Cl_(2(g)) rarr 2Cl_((g)), DeltaH=242.3kJ mol^(-1) (b) I_(2(g))rarr 2I_((g)), DeltaH=151.0kJ mol^(-1) (c) ICl_((g)) rarr I_((g))+Cl_((g)), DeltaH=211.3kJ mol^(-1) (d) I_(2(s)) rarr I_(2(g)), DeltaH=62.76kJ mol^(-1) If standard state of iodine and chloride are I_(2(s)) and Cl_(2(g)) , the standard enthalpy of formation for ICl_((g)) is :

For the following process, H_(2)(g)rarr2H(g) . It absorbs 438kJmol^(-1) . Thus,

Match the correct bond dissociation in halogens {:("Halogens","Bond energy "),(F_(2),"158.8 Kj mol"^(-1)),(Cl_(2),"242.6KJmol"^(-1)),(Br_(2),"151.1KJmol"^(-1)),(I_(2),"192.8KJmol"^(-1)):}

Cl_2(g)rarr 2Cl(g) Delta H^@=242KJ mol^(-1) what is its enthalpy of atomization?