Itc. 8. The enthalpy changes for the followi processes are listed below: CI, (g) = 2C1(g), 242.3kJ moli 12(g)= 21(g), 151.0kJ mol-1 ICI(g) = I(g) + CI(g), 211.3kJ mol na 1,($) = 1,(g), 62.76kJ mol Given that the standard states for iodine and chlorine are 1, (s) and Cl2(g), the standard enthalpy of formation for ICI(g) is: 1)+16.8 kJ mol 2) +244.8kJ mol! 3)-14.6kJ mol-1 4)-16.8kJ moll

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 :

Calculate the bond enthalpy of H-CI given that the bond enthalpies of H_(2) and CI_(2) are 435.4 and 242.8 kJ "mol"^(-1) respectively and enthalpy of formation of HCI(g) is -92.2 kJ mol

Calculate the standard enthalpy of combustion of CH_(4) , it standard enthalpies of formation of CH_(4(g)),H_(2)O_((l)), and CO_(2(g)) are -74.81kJ mol^(-1), -285.83kJ mol^(-1) and -393.51kJ mol^(-1) respectively.

Calculate the standard enthalpy change for the reaction CH_4(g) +2O_2(g) rarr CO_2(g)+2H_2O(l) Given that the standard enthalpies of formation of CH_4(g),CO_2(g), and H_2O(l) are -74.8 kJ mol^-1, -393.5 kJ mol^-1 and -285.8 kJ mol^-1 respectively.