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

Explain the following sequence of IE's in group IIIA. B(801), Al(577), Ga(579), In(558), Tl(589) kJmol^(-1) .

Explain the following (c ) Variation of nature of oxides in the Group - 1:

How much charge is required for the following reductions: (i) 1 mol of Al^(3+) to Al. (ii) 1 mol of Cu^(2+) to Cu. (iii) 1 mol of MnO_(4)^(-) to Mn^(2+) .

The enthalpy changes for the following processes are listed below: Cl_(2(g)) rarr 2Cl_((g)) , DeltaH = 242.3 kJ mol^(-1) I_(2(g)) rarrr 2I_((g)) , DeltaH = 151.0 kJ mol^(-1) ICl_((g)) rarr I_((g)) + Cl_((g)) , DeltaH = 211.3 kJ mol^(-1) I_(2(s)) rarr I_(2(g)) , DeltaH = 62.76 kJ mol^(-1) Given that the standard states for iodine and chlorine are I_(2(s)) and Cl_(2(g)) , the standard enthalpy of formation for ICT is:

alpha -maltose can be hydrolysed to glucose according to the following reaction. Given Standard enthalpies of formation of C_(12) H_(22)O_(11) (aq) = -2238 kJ/mol Standard enthalpies of formation of H_(2)O (l) = -285kJ//mol Standard enthalpies of formation of C_(6)H_(12)O_(6) (aq) = -1263kJ//mol {:("Time (min)",0,1.0,100),("Conc. Of -maltose(M)",4.0,1.0,0.25):} Which of the following statements(s) is/are true?

The first ionization enthalpy values (in kJ mol^(-1) ) of group 13 elements are: {:(B,Al,Ga,In,Ti),(801,577,579,558,589):} How do you explain this deviation from the general trend?

Calculate heat of solution of NaCl from the following data Hydration energy of Na^(+) = -389kJ mol^(-1) Hydration energy of Cl^(-) = -382kJ mol^(-1) Lattice energy of NaCl = +776 kJ mol^(-)