Cesium chloride is formed according to the following equation \(\mathrm{Cs}(\mathrm{s})+0.5 \mat....

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Cesium chloride is formed according to the following equation \(\mathrm{Cs}(\mathrm{s})+0.5 \mathrm{Cl}_2(\mathrm{~g}) \rightarrow \mathrm{CsCl}(\mathrm{s})\). The enthalpy of sublimation of \(\mathrm{Cs}\), enthalpy of dissociation of chlorine, ionization energy of Cs and electron affinity of chlorine are \(81.2,243.0,375.7\) and \(348.3 \mathrm{~kJ} \mathrm{~mol}^{-1}\). The energy change involved in the formation of \(\mathrm{CsCl}\) is \(-388.6 \mathrm{~kJ} \mathrm{~mol}^{-1}\). Calculate the lattice enthalpy of \(\mathrm{CsCl}\). 📲PW App Link - https://bit.ly/YTAI_PWAP 🌐PW Website - https://www.pw.live



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