Anhydrous `AlCl_(3)` is covalent from the data given below, perdict whether it would remain covalent or between ionic in aqueous solution
`IE_(1)` of `Al = 5140 kJ mol^(-1)`
`Delta_("hyd")H^(ɵ)(Al^(3+)) = -4665 kJ mol^(-1)`
`Delta_("hyd")H^(ɵ)(Cl^(ɵ)) = -380 kJ mol^(-1)`

Anhydrous AlCl_(3) is covalent. From the date given below, predict whether it would remain covalent or become ionic in aqueous solution. (Ionisation energy for Al is 1537 kJ mol^(-1) ) Delta_("hydration") for Al^(3+) = - 4665 kJ mol^(-1) Delta_("hydration") for Cl^(Ө) = - 381 kJ mol^-1 .

Preduct that anhyrous AICI_(3) is covalent form the data given below, ionisation enegry for AI = 5137 kJ mol^(-1), Delta_(hyd) H for AI^(3+) =- 4665 kJ "mole"^(-1), Delta_(hyd)H for CI^(Theta) =- 381 kJ mol^(-1))

Calculate the standard enthalpy of solution of AgCl(s) in water DeltaH_(f)^(0)(AgCl,s)= -127.07kJ mol^(-1), Delta H_(f)^(0)(Ag^(+),aq)=105.58 kJ mol^(-1) ,DeltaH_(f)^(0)(Cl^(-),aq)= -167.35 kJ mol^(-1)

Calculate the standard enthalpy of solution of AgCl(s) in water DeltaH_(f)^(0)(AgCl,s)= -127.07kJ mol^(-1), Delta H_(f)^(0)(Ag^(+),aq)=105.58 kJ mol^(-1),DeltaH_(f)^(0)(Cl^(-),aq)= -167.35 kJ mol^(-1)

Anhydrous AlCl_3 is covalent compound. Select the correct statement regarding AlCl_3 based on the given information. Given, the energy to ionise AlCl_3 is 5215 kJ mol^-1 , Delta_hydration for Al^(3+) is -4670 kJ mol^-1 and Delta_hydration for Cl^- is -381 kJ mol^-1

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)

Calculate the lattice energy from the following data (given 1 eV = 23.0 kcal mol^(-1) ) i. Delta_(f) H^(ɵ) (KI) = -78.0 kcal mol^(-1) ii. IE_(1) of K = 4.0 eV iii. Delta_("diss")H^(ɵ)(I_(2)) = 28.0 kcal mol^(-1) iv. Delta_("sub")H^(ɵ)(K) = 20.0 kcal mol^(-1) v. EA of I = -70.0 kcal mol^(-1) vi. Delta_("sub")H^(ɵ) of I_(2) = 14.0 kcal mol^(-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 enthalpy of combustion of benzene (l) on the basis of the following data: a. Resonance energy of benzene (l) =- 152 kJ// mol b. Enthalpy of hydrogenation of cyclohexene (l) =- 119 kJ//mol c. Delta_(f)H^(Theta)C_(6)H_(12)(l) =- 156 kJ mol^(-1) d. Delta_(f)H^(Theta) of H_(2)O(l) =- 285.8 kJ mol^(-1) e. Delta_(f)H^(Theta)of CO_(2)(g) =- 393.5 kJ mol^(-1)

Calculate the enthalpy change for the process C Cl_(4)(g) rarr C(g)+4Cl(g) and calculate bond enthalpy of C-Cl in C Cl_(4)(g) . Delta_(vap)H^(Θ)(C Cl_(4))=30.5 kJ mol^(-1) Delta_(f)H^(Θ)(C Cl_(4))=-135.5 kJ mol^(-1) Delta_(a)H^(Θ)(C )=715.0 kJ mol^(-1) , where Delta_(a)H^(Θ) is enthalpy of atomisation Delta_(a)H^(Θ)(Cl_(2))=242 kJ mol^(-1)