Caesium chlorides is formed according to the following equation `Cs(s)+0.5Cl_(2)(g)rarrCaCl(s)`. The enthalpy of sublimation of Cs, enthalpy of dissocitation of chlorine, ionization energy of Cs and electron affinity of chlorine are 81.2,243.0,375.7 and -348.3 kJ`mol^(-1)`. The energy change involved in the formation of CsCl is -388.6 kJ `mol^(-)`. Calculate the lattice energy of CsCl.

Options

A. 618.7 kJ `mol^(-1)`
B. 1237.4 kJ `mol^(-1)`
C. `1237.4 kJ mol^(-1)`
D. `-532.7 KJ mol^(-1)`

Answer

D

Explanation

`-12250x - 13000(1-x)= -12500`
`750xx500 rArr x=2//3`
So , required ratio is =`(2)/(1)`