Question

At normal temperature and pressure, what is the molar volume of an ideal gas?

Answer 1

Standard temperature and pressure are conditions that must be established for experimental measurements in order to make comparisons between different sets of data. NTP stands for normal temperature and pressure, whereas STP stands for standard temperature and pressure. The STP values for temperature and pressure for gas, according to IUPAC, are 273.15 K and 0.987 atm, respectively. The NTP temperature and pressure values are 293.15 K and 1atm, respectively.

Complete answer:
The molar volume is the volume occupied by one mole of a chemical element or a chemical compound at standard temperature and pressure (STP). It is determined by multiplying the molar mass by the mass density. A molar gas volume is the volume of one mole of any gas at a particular temperature and pressure.
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. Many actual gases behave qualitatively like an ideal gas under various temperature and pressure circumstances, with the gas molecules (or atoms in the case of monatomic gases) acting as the ideal particles.
${{\mathbf{V}}_{{\text{molar }}}} = {\mathbf{293K}}{\text{x}}{\mathbf{0}}.{\mathbf{0820L}}.{\mathbf{atm}}{({\mathbf{molK}})^{ - 1}}$
${{\mathbf{V}}_{{\text{molar }}}}{\text{ }} = {\mathbf{2404L}}{\text{ }}$
Hence at normal temperature and pressure, 2404 L is the molar volume of an ideal gas.

Note:
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, also fail. 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.