Question

A gas occupies 300 mL at \[127^\circ C\] and 730 mm pressure. What would be its volume at STP
A.52.44 ml
B.152.44 ml
C.262.4 ml
D.3.5244 ml

Answer 1

Hint: An ideal gas is a theoretical gas made up of a large number of randomly moving point particles with no interparticle interactions. Because it obeys the ideal gas law, a simplified equation of state, and is susceptible to statistical mechanics analysis, the ideal gas notion is helpful. If the interaction is fully elastic or viewed as point-like collisions, the criterion of zero interaction can frequently be waived.

Complete answer:
When intermolecular interactions and molecular size become relevant at lower temperatures or greater pressures, the ideal gas model tends to collapse. Most heavy gases, such as many refrigerants, and gases with high intermolecular interactions, such as water vapour, fail to pass this test. The volume of a real gas is typically much bigger than that of an ideal gas at high pressures. A real gas's pressure is frequently lower than that of an ideal gas at low temperatures. Real gases undergo a phase transformation, such as to a liquid or a solid, at a low temperature and high pressure. The ideal gas model, on the other hand, does not describe or enable phase transitions.
The ideal gas law is the state equation for an ideal gas, which is given by PV = nRT
P stands for pressure.
The letter V stands for volume.
The quantity of material in the gas is denoted by n. (in moles).
The gas constant is R (\[0.08206\;L.atm.{K^{ - 1}}.mo{l^{ - 1}}\]).
The absolute temperature is denoted by the letter T.
${{\text{V}}_2} = \dfrac{{300}}{{1000}}\;{\text{mL}}$
${{\text{P}}_2} = \dfrac{{730}}{{760}}\;{\text{atm}}$
${{\text{T}}_2} = 300\;{\text{K}}$
At STP ${{\text{V}}_1} = ?$
${{\mathbf{P}}_1} = 1\;{\text{atm}}$
${{\text{T}}_1} = 273\;{\text{K}}$
From Ideal gas equation:
$\dfrac{{{{\text{P}}_2}\;{{\text{V}}_2}}}{{\;{{\text{T}}_2}}} = \dfrac{{{{\text{P}}_1}\;{{\text{V}}_1}}}{{\;{{\text{T}}_1}}}$
${{\text{V}}_1} = 0.2622l$
Hence Volume ${\text{262}}{\text{.2 mL}}$
Hence, the correct answer is option C.

Note:
The general gas equation, commonly known as the ideal gas law, is the state equation of a hypothetical ideal gas. Although it has numerous drawbacks, it is a decent approximation of the behaviour of various gases under many situations. Benoît Paul Émile Clapeyron originally articulated it in 1834 as a mixture of empirical Boyle's law, Charles' law, Avogadro's law, and Gay-law Lussac's law.