One mole of Cl_(2(g)) which may be assumed to obey the ideal gas law, initially at 300 K and 1.01325 xx 10^(7) Pa, is expanded against a constant exteranl pressure of 1.01325 xx 10^(5) Pa to a final pressure of 1.01325 xx 10^(6) Pa . As a result of the expansion , the gas cooled to a temperature of 239 K (which is the normal boiling point of Cl_(2)) and 0.100 mol of Cl_(2) condensed. The enthalpy of vaporization of Cl_(2(l)) is 20.42 KJ "mol"^(-1) at the normal volume is C_(v)=28.66 JK^(-1) "mol"^(-1) and the density of Cl_(2(l)) is 1.56 g cm^(-1)(at 239 K) . Assume that the molar heat capacity at constant pressure for Cl_(2(g)) is C_(p)=C_(v)+R. (1 atm = 101325 xx 10^(5) Pa , R=8.314510 Jk^(-1) "mol"^(-1) = 0.0820584 L atm K^(-1)"mol"^(-1)) (i) Either draw a complete molecular orbital energy diagram or write the complete electronic configuration of Cl_(2) Predict the bond order of Cl_(2) and thus whether this molecules will be diamagnetic , ferromagnetic ,or paramagnetic. (ii) For the changes decribed above, calculate the change in the internal energy (DeltaE) and the change in the entropy (DeltaS_("sys")) of the system.