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)`.

Use (IE) and (EA) listed below to determine whether the following process is endothermic exothermic. Mg_((s)) + 2F_((g)) to Mg_((g))^(2+) + 2F_((g))^(-) (IE)_1 of Mg_((g))=737.7 "kJ mol"^(-1) (IE)_2 of Mg_((g))=1451 "kJ mol"^(-1) (EA) of F_((g))=-328 "kJ mol"^(-1)

Calculate the percentage of Mg_((g))^(o+) and Mg_((g))^(2+) if 2.4 g of Mg absorbs 120 kJ of energy. The IE_(1) and IE_(2) of Mg_((g)) are 740 and 1450 kJ mol^(-1) .

Calculate the percentage of Mg_((g))^(o+) and Mg_((g))^(2+) if 2.4 g of Mg absorbs 120 kJ of energy. The IE_(1) and IE_(2) of Mg_((g)) are 740 and 1450 kJ mol^(-1) .

DeltaH in terms of 'x' xx 10^(3) KJ is if M_((g)) + 2X_((g)) rarr M_((g))^(2+) + 2X_((g))^(-) Given : (I.E)_(1) of M (g) = 705.7 kJ mol^(-1), (I.E)_(2) " of" M(g) = 951 kJ mol^(-1) and (E.A)_(1) of X(g) = -328 kJ mol^(-1) 'x' is

DeltaH in terms of 'x' xx 10^(3) KJ is if M_((g)) + 2X_((g)) rarr M_((g))^(2+) + 2X_((g))^(-) Given : (I.E)_(1) of M (g) = 705.7 kJ mol^(-1), (I.E)_(2) " of" M(g) = 951 kJ mol^(-1) and (E.A)_(1) of X(g) = -328 kJ mol^(-1) 'x' is

IE_(1) and IE_(2) of Mg are 178 and 348 kcal mol^(-1) . The energy required for the reaction Mg rarr Mg^(2+)+2e^(-) is

IE_(1) and IE_(2) of Mg are 178 and 348 kcal mol^(-1) . The energy required for the reaction Mg rarr Mg^(2+)+2e^(-) is

IE_(1) and IE_(2) of Mg are 178 and 348 kcal mol^(-1) . The energy required for the reaction Mg rarr Mg^(2+)+2e^(-) is

Using ._(f)G^(Theta)(Hi) = 1.3 kJ mol^(-1) , calculate the standard free enegry change for the following reaction: H_(2)(g) +I_(2)(g) rarr 2HI(g)