A sample of pure gas has a density of $1.60\,{\rm{g}}\,{\rm{litr}}{{\rm{e}}^{ - 1}}$ at $26.5\,^\circ C$ and $680.2\,{\rm{mm}}\,\,{\rm{Hg}}$. Which of the following is present in the sample?

NEET UG CHEMISTRY MCQ: STATES OF MATTER

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A sample of pure gas has a density of

1.60\,\mathrm{g}\,\mathrm{litr}{\mathrm{e}^{ - 1}}

26.5\,^\circ C

and

680.2\,\mathrm{mm}\,\,\mathrm{Hg}

. Which of the following is present in the sample?

View answer and explanation

Correct option: C

\mathrm{C}{\mathrm{O}_2}

Option C is correct because, using the ideal gas law and the given density, temperature, and pressure, the calculated molar mass is approximately 44 g/mol, which corresponds to CO2.

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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}}}

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