Question

The molar enthalpy of vaporosation of acetone is less than that of water. Why?
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Answer 1

$\huge \mathfrak {Answer:-}$

=> Acetone does not have hydrogen bond.

=> Thus, intermolecular forces are comparatively weaker which makes it boil/evaporates fast.

=> Thus, reducing the molar enthalpy of vaporization.

=> Also, Acetone does not polar O-H bond contributing to low enthalpy.

=> Water has non-polar region and also has strong hydrogen bond.

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