In which of the following, the first compound does not have higher boiling point than the second?

H_{2} O

and

H_{2} S

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C H_{4}

and

S i H_{4}

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H F

and

H C l

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H I

and

H B r

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Solution

The correct option is C $C H_{4}$ and $S i H_{4}$
The boiling point of $C H_{4}$ is $- {161.5}^{o} C$ and that of $S i H_{4}$ is $- {111.7}^{o} C$ .

The molecular weight of $C H_{4}$ is lesser than that of $S i H_{4}$ which leads to a lesser magnitude of London depression forces. Hence, $C H_{4}$ has a lower boiling point than $S i H_{4}$ .

So, the correct option is $B$

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Similar questions

Which of the following substance have abnormally high boiling points and why?

H_{2} S, H_{2} O, H F, H I, {C H}_{4}, C_{2} H_{5} O H

Q. The boiling points of

H F, H C l, H B r

and

H I

follows the order:

The correct order of boiling points of HF , HCl , HBr and HI is

Q. Arrange the following hydrides in their increasing acid strength

[C H_{4}, H_{2} S, P H_{3} a n d S i H_{4}]

Use the information and date given below to answer the question (a) to (c),

Stronger intermolecular forces result in higher boiling point.

Strength of London forces increases with the number of electrons in the molecule.

Boiling point of HF,HCl, HBr and Hi are 293 k, 189 k, 206 k and 238 k respectively.

(a) Which type of intermolecular forces are present in the molecules HF, HCl, HBr an HI?

(b) Looking at the trend of boiling points of HCl, HBr and HI, explain out of dipole-dipole interaction and London interaction, which one is predominant here.

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