A sample of gas at $35\,^\circ C$ and 1 atmospheric pressure occupies a volume of $3.75\,\,{\rm{litre}}$. At what temperature should the gas be kept, if it is required to reduce the volume to $3.0$ litre at the same pressure?

NEET UG CHEMISTRY MCQ: STATES OF MATTER

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Application +4 | -1

A sample of gas at 

35\,^\circ C

and 1 atmospheric pressure occupies a volume of

3.75\,\,\mathrm{litre}

. At what temperature should the gas be kept, if it is required to reduce the volume to

3.0

litre at the same pressure?

View answer and explanation

Correct option: A

- 26.6\,^\circ C

Option A is correct because, using Charles's Law (V1/T1 = V2/T2), and converting to Kelvin, the final temperature is calculated to be -26.6°C.

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\begin{array}{cccccccccccccccccccc} {\underline {{\text{Gas}}} }&{\underline {\,{\text{Critical}}\,\,{\text{temperature}}} } \\ {\text{A}}&{{T_{{C_1}}}} \\ {\text{B}}&{{T_{{C_2}}}} \\ {\text{C}}&{{T_{{C_3}}}} \\ {\text{D}}&{{T_{{C_4}}}} \end{array}

{T_{{C_1}}} > {T_{{C_2}}} > {T_{{C_3}}} > {T_{{C_4}}}

{r^x}

r

x