What is the `DeltaH` of the following affinity.
`Mg_(g)+2F_(g) rarr Mg_((g))^(2+)+2F_((g))^(-)`.
If the electron affinity of
`F_(g) = -328 kJ " mol"^(-1)` and first ionisation energy of `Mg = 737.7kJ " mol"^(-1)` and second ionisation energy of `Mg = 1451kJ " mol"^(-1)`

The electron gain enthalpy Delta e_(g)H is -349 kJ mol^(-1) . If the ground state energy of Cl(g) is x kJ mol^(-1) . The ground state energy (in kJ mol^(-1) ) of Cl^(-) (g) is

Calculate the lattice energy of formation of NaCl from the following data : Na_((s)) +1//2Cl_(2(g)) to NaCl_((s)) Delta H_(f) -411.3 KJ.mol^(-1) Heat of sublimation of Na_((s)) = 108 . 7 kJ mol ^(-1) Ionisation energy of Na_((g)) = 49.5.0 kJ mol^(-1) Dissociation energy of Cl_(2(g)) = 244 kJ mol^(-1) Electron affinity of Cl_((g)) = - 349 . 0 kJ mol^(-1)

Construct a Born-Haber cycle and use it to calculate the first electron affinity of chlorine. DeltaH_(atom(CI))= +122 kJ mol^(-1) " " DeltaH_(atom(Mg))=+148 kJ mol^(-1) DeltaH_("1st ionisation energy" (Mg))=+738 KJ mol^(-1) " " DeltaH_(2nd " ionisation cnergy"(MgCI_(2))= +1451 kJ mol^(-1) DeltaH _("lattice energy "(MgCI_(2))= -2526 kJ mol^(-1) " " DeltaH_(2nd " formation "(MgCI_(2)) =-641 kJ mol^(-1)

Using the data given below,predict the nature of heat changes for the reaction . Mg_(g) + 2F_(g) rarr Mg_(g)^(2+) +2F_(g)^- IE_1 and IE_2 of Mg_(g) are 737.7 and 451 kJ "mol"^(-1) . EA_1 for F_(g) is -328 kJ "mol"^(-1) .

The energy required for the following process is 1.96 xx 104" kJ mol"^(-1)rarr3e^(-)+Li^(3+)(g) If the first ionisation energy of lithium is "520 kJ mol"^(-1) what is the second ionisation energy?

Which ions are present in MgO(s) Calculate the enthalpy change for the reaction Mg(s) + 1//2O_(2)(g) rarr MgO(s) What kind of enthalpy change is this? Standard enthalpy of formation of MgO. DeltaH_(atom(O))= +249 kJ mol^(-1) " " DeltaH_(atom(Mg))=+148 kJ mol^(-1) DeltaH_("1st ionisation energy" (Mg))=+738 KJ mol^(-1) " " DeltaH_(2nd "electron energy "(Mg))= +145 1 kJ mol^(-1) DeltaH _("1st electron affinity "(O))= -141 kJ mol^(-1) " " DeltaH_(2nd " electron affinity "(O)) =+798 kJ mol^(-1) DeltaH_("lattice energy "(MgO))= - 3791 kJ mol^(-1)

Calculate the enthalpy change of the reaction Na(s) + 1//2Br_(2)(g)rarr NaBr(s) DeltaH atomisation (Na) = +107 kJ mol^(-1) DeltaH atomisation (Br) = +97 kJ mol^(-1) DeltaH first ionisation energy (Na) = +496 kJ mol^(-1) DeltaH first electron affinity (Br) = -325 kJ mol^(-1) DeltaH lattice energy (NaBr) = -742 kJ mol^(-1)

The energy required for the following process is 1.96 xx 10^4 kJ mol^(-1) Li_(g) to 3e^(-) + Li_((g))^(3+) If the first ionisation energy of lithium is 520 kJ mol^(-1) , what is the second ionisation energy?

When a mole of magnesium bromide is prepared from 1 mole of magnesium and 1 mole of liquid bromine, 524 kJ of energy is released. The heat of sublimation of Mg metal is 148 "kJ mol"^(-1) . The heat of dissociation of bromine gas into atoms is 193 "kJ mol"^(-1) . The heat of vaporization of liquid bromine is 31 kJ "mol"^(-1) . The ionisation energy of magnesium is 2187 kJ mol^(-1) and the electron affinity of bromine is - 662 "kJ mol"^(-1) . Calculate the lattice energy of magnesium bromide.