Volume,

V = \( \dfrac{mRT}{Mp}\)

= \( \dfrac{0.184 \; \times \; R \; \times \; 290}{ 2 \; \times \; p}\)

Let M be the molar mass of the unknown gas.

Volume occupied by the unknown gas is,

= \( \dfrac{mRT}{Mp}\)

= \( \dfrac{2.9 \; \times \; R \; \times \; 368}{ M \; \times \; p}\)

According to the ques,

\( \dfrac{0.184 \; \times \; R \; \times \; 290}{ 2 \; \times \; p} \)

\( = \dfrac{2.9 \; \times \; R \; \times \; 368}{ M \; \times \; p} \dfrac{0.184 \; \times \; 290}{ 2 } \)

\( = \dfrac{2.9 \; \times \; 368}{ M }\)

M = \( \dfrac{2.9 \;\times \; 368 \; \times \; 2}{0.184 \; \times \; 290}\)

= 40g mol^{-1}

Therefore, the molar mass of the gas is 40g mol^{-1}

Explain the physical significance of Van der Waals parameters.

Critical temperature for carbon dioxide and methane are 31.1°C and – 81.9°C respectively. Which of these has stronger intermolecular forces and why?

In terms of Charles’ law explain why -273°C is the lowest possible temperature.

What would be the SI units for the quantity \(\dfrac{pV^2 T^2}{n}\)

A mixture of dihydrogen and dioxygen at one bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.