In which of the following pairs is the boiling point of first compound not more than the second?

K C l, C l_{2}

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N e, H e

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P H_{3}, A s H_{3}

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H F, H C l

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Solution

The correct option is B $P H_{3}, A s H_{3}$
Among $K C l$ and $C l_{2}$ , $K C l$ will have a higher boiling point due to its ionic nature. Ionic compounds have high boiling points.
Among $N e$ and $H e$ , $N e$ will have a higher bp because for inert gases, boiling point increases with increase in the atomic weight.
The boiling point of $P H_{3} (185.5 K)$ is lower than the boiling point of $A s H_{3} (210.6 K)$ . On moving down the group, the boiling point increases due to increase in the molar mass.
Among $H F$ and $H C l$ , $H F$ will have higher bp due to hydrogen bonding.
Hence, option C is correct.

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Similar questions

1. S b H_{3} > N H_{3} > A s H_{3} > P H_{3}

2. N H_{3} > P H_{3} > A s H_{3} > S b H_{3}

3. N H_{3} > P H_{3} > A s H_{3} > S b H_{3}

4. N H_{3} > P H_{3} > A s H_{3} > S b H_{3}

(i) H F, H C l, H B r, H I

(i i) H_{2} O, H_{2} S, H_{2} S e, H_{2} T e

(i i i) N H_{3}, P H_{3}, A s H_{3}, S b H_{3}

Arrange the following in the order of property indicated for each set:

$F_{2}, C l_{2}, B r_{2}, I_{2}$ - increasing bond dissociation enthalpy.

HF,HCl, HBr, HI- Increasing acid strength.

$N H_{3}, P H_{3}, A s H_{3}, S b H_{3}, B i H_{3}$ - increasing base strength.

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