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roblem 1.12: calculate the average volume per molecule for an ideal gas at room temperature and atmospheric pressure. then take the cube root to get an estimate of the average distance between molecules. how does this distance compare to the size of a molecule like { n } { 2 }n 2 ​ or { h } { 2 }oh 2 ​ o?

Respuesta :

An ideal gas follows the ideal gas law stating PV = nRT. Obtain the average volume/mole by solving for V/n. Divide both sides by Avogadro’s constant Na. Multiplying n and Na gives the number of molecules N.   V/N is the average volume/molecule. 250C is the room temperature = 298.15K. The atmospheric pressure is 101325 Pa or 1 atm. Each molecule in a gas is spaced evenly and placed in a lattice. To obtain the space taken up by a cube, find the cube root of V/N to obtain the average intermolecular distance.  For small molecules such as N2 or H2, the angstroms order is 10^(-10)  m. The intermolecular distance is about 10 times the small molecules.

P V = nRT

V⁄n=RT⁄P

V⁄(nNa )=RT⁄(PNa )

V⁄N=((8.314 J/(mol.K))(298.15K))/((101325Pa)(6.02×10^23  molecules/mol))≈4.06×10^23  m^3/molecule

∛(V/N)≈3.44×10^(-9) m = 3.44 nm

The intermolecular distance is about 10 times the small molecules.

Find out more on intermolecular distance at: brainly.com/question/11184388

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