Pressure exerted by 1 mole of methane in a 0.25 L container at 300 K using van der Waals’ equation is $\left( {{\rm{Given}},{\rm{\;}}a = 2.253\;\,\,{\rm{atm\;}}\,\,{{\rm{L}}^2}\;\,\,{\rm{mo}}{{\rm{l}}^{ - 2}},\;\,\,b = 0.0428\;\,\,{\rm{L\;}}\,\,{\rm{mo}}{{\rm{l}}^{ - 1}}} \right)$

NEET UG CHEMISTRY MCQ: STATES OF MATTER

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Pressure exerted by 1 mole of methane in a 0.25 L container at 300 K using van der Waals’ equation is

\left( {\mathrm{Given},\mathrm{\;}a = 2.253\;\,\,\mathrm{atm\;}\,\,{\mathrm{L}^2}\;\,\,\mathrm{mo}{\mathrm{l}^{ - 2}},\;\,\,b = 0.0428\;\,\,\mathrm{L\;}\,\,\mathrm{mo}{\mathrm{l}^{ - 1}}} \right)

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Correct option: A

82.82\,\,\mathrm{ }atm

Option A (82.82 atm) is correct because it is calculated using the van der Waals equation with the given parameters.

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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}

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