Explain the following sequence of IE's in group IIIA. B(801), Al(577), Ga(579), In(558), TI(589) kJ `"mol"^(-1)1` .

Calculate the enthalpy of formation of ammonia from the following bond energy data: (N-H) bond = 389 kJ mol^(-1), (H-H) bond = 435 kJ mol^(-1) , and (N-=N)bond = 945.36kJ mol^(-1) .

Calculate the value of equilibrium constant, K for the following reaction at 400 K. 2NOCl(g) hArr 2NO (g) + Cl_2(g) DeltaH^@ = 80.0 kJ mol^(-1), DeltaS^@ = 120 KJ^(-1) mol^(-1) at 400 K, R = 8.31 JK^(-1) mol^(-1) .

Answer the following question (Based on EA, Delta_(eg)H^(ɵ) and IE ). IE_(1) of Li is 5.4 eV "atom"^(-1) and the EA of Cl is 3.6 eV "atom"^(-1) . Calculate Delta_( r)H^(ɵ) in "kcal mol"^(-1) and kJ mol^(-1) for the reaction Li_((g))+Cl_((g)) rarr Li_((g))^(o+)+Cl_((g))^(ɵ) formed at such a low pressure that resulting ions do not combine with each other.

What is the enthalpy change for the given reaction, if enthalpies of formation of Al_(2)O_(3) and Fe_(2)O_(3) are -"1670 kJ mol"^(-1) and -"834 kJ mol"^(-1) respectively? Fe_(2)O_(3) +2Al rarr Al_(2)O_(3)+2Fe

Calculate the EA of O atom to O^(2-) ion from the following data: i. Delta_(f)H^(ɵ)[MgO(s)] = -600 kJ mol^(-1) ii. Delta_(u)H^(ɵ) [MgO(s)] = -3860 kJ mol^(-1) iii. IE_(1) + IE_(2) of Mg(g) = 2170 kJ mol^(-1) iv. Delta_("diss")H^(ɵ) of Mg(s) = + 494 kJ mol^(-1) v. Delta_("sub")H^(ɵ) of Mg(s) = +150 kJ mol^(-1)

The enthalpy of formation of ammonia when calculated from the following bond energy data is (B.E. of N-H, H-H, N-=N is "389 kJ mol"^(-1), "435 kJ mol"^(-1),"945.36 kJ mol"^(-1) respectively)

Calculate the lattice energy of the reaction Li^(o+)(g) +CI^(Theta) (g) rarr LiCI(s) from the following data: Delta_("sub")H^(Theta)(Li) = 160.67 kJ mol^(-1), (1)/(2)D(CI_(2)) = 122.17 kJ mol^(-1) IP(Li) = 520.07 kJ mol^(-1),E_(A)(CI) = - 365.26 kJ mol^(-1) and Delta_(f)H^(Theta)(LiCI) =- 401.66 kJ mol^(-1)

In a hypothetical reaction X to Y , the activation energy for the forward backward reactions are 15 and 9 kJ mol^(-1) respectively. The potential energy of X is 10 kJ mol^(-1) . Which of the following statement is/are correct? (i) The threshold energy of the reaction is 25 kJ mol^(-1) (ii) The potential energy of Y is 16 kJ mol^(-1) (iii) Heat of reaction is 6 kJ mol^(-1) The reaction is endothermic.

The following data is known for melting of KCI: DeltaS^(Theta) = 0.007 kJ K^(-1) mol^(-1), DeltaH^(Theta) = 7.25 kJ mol^(-1) Calculate the melting point of KCI .

Find the enthalpy of formation of hydrogen flouride on the basis of following data: Bond energy of H-H bond =434 kJ mol^(-1) Bond energy of F-F bond =158 kJ mol^(-1) Bond enegry of H -F bond =565 kJ mol^(-1)