Please explain the proper reason of statement ​1 as the 2nd statement is incorrect.​

Please explain the proper reason of statement ​1 as the 2nd statement is incorrect.​ Statement-I : Enthalpy changes are positive when NazSOa.10H20, CuSOa.5H20 and salts like NaC\, KCI, etc., which do not form hydrates are dissolved in water. But enthalpy changes are negatb.æ when anhydrous salts capable of forming hydrates are dissolved in water. Because Staterrzlt-n : The differenæ the behauour is due to large differercz and anhydrous salts. The substances wdth larper molecular weights u*zly show' posiüve enthalpy charQes

Dear Student,

The enthalpy of the system is vital parameter in denoting whether the molecule is endothermic (or) exothermic in reaction, in exothermic reaction the water molecules gets dissipated as reaction evolves heat while in endothermic the reaction takes by supplying external source of heat form. As per statement 1 the given salt formation are occurred by endothermic reaction hence they are positive while in anhydrous salt which loses moisture on exposure to atmosphere by exothermal process hence they are negative in state. For statement 2 lets take an given NaCl molecule whose molar mass is higher than NaOH even though both salts contain sodium ion but their characteristics are differentiated by their molar constituents hence larger molar mass substance shows positive enthalpy as it requires external heat to breakdown representing endothermic while lower molar mass expresses exothermic.

Hence the molar mass also influences the enthalpy of the molecular formation and dissipation process.

Regards.