Water,Ethanol,and Ether are all liquids at ro | vedclass

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(B) The boiling point of a liquid depends on the strength of the intermolecular forces holding the molecules together. $1$. Water $(H_2O)$ exhibits st

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Due to differences in the strength of intermolecular forces.

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(B) The boiling point of a liquid depends on the strength of the intermolecular forces holding the molecules together. $1$. Water $(H_2O)$ exhibits strong hydrogen bonding,leading to a high boiling point of $100 \ ^\circ C$. $2$. Ethanol $(C_2H_5OH)$ also exhibits hydrogen bonding,but it is weaker than in water due to the presence of the hydrophobic ethyl group,resulting in a boiling point of $78 \ ^\circ C$. $3$. Diethyl ether $((C_2H_5)_2O)$ lacks hydrogen bonding and is held together by weaker dipole-dipole interactions,resulting in a much lower boiling point of $34.6 \ ^\circ C$. Therefore,the difference in boiling points is primarily due to the varying strength of intermolecular forces.

Water,Ethanol,and Ether are all liquids at room temperature; why do their boiling points differ?

Similar Questions

Explain why,in spite of having nearly the same electronegativity,oxygen forms hydrogen bonding while chlorine does not.

The compound/s which will show significant intermolecular $H$-bonding is/are :
$(a)$ $o$-Nitrophenol
$(b)$ $N$-($4$-hydroxyphenyl)acetamide
$(c)$ $2,6$-di-tert-butylphenol

Which statement is correct?

Hydrogen bonding plays a central role in the following phenomena:
$(A)$ Ice floats in water.
$(B)$ Higher Lewis basicity of primary amines than tertiary amines in aqueous solutions.
$(C)$ Formic acid is more acidic than acetic acid.
$(D)$ Dimerisation of acetic acid in benzene.

How many water molecules present in $CuSO_4 \cdot 5 H_2 O$ are hydrogen bonded?

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