The lattice energy of CsI(s) is 604 KJ/mol, and theenthalpy of solution is 33 KJ

Question

The lattice energy of CsI(s) is 604 KJ/mol, and theenthalpy of solution is 33 KJ/mol. Calculate the enthalpy ofhydration (KJ) of 0.49 moles of CsI.
Note that lattice energy is defined as the enery released whenthe crystal lattice is formed. Thus to break down the lattice theenergy would be positive. The lattice energy of CsI(s) is 604 KJ/mol, and theenthalpy of solution is 33 KJ/mol. Calculate the enthalpy ofhydration (KJ) of 0.49 moles of CsI.
Note that lattice energy is defined as the enery released whenthe crystal lattice is formed. Thus to break down the lattice theenergy would be positive.

Explanation / Answer

We Know that :     H ( hydration ) = numberof moles x [ H ( lattice energy ) ] + number ofmoles x [ H ( enthalpy of solution ) ]                                = 0.49 moles x -604 kJ / mol + 0.49 mole x 33 kJ /mol                                 = -279.79 kJ

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