Pls ! part 1. determine the molar mass of a 0.314-gram sample of gas having a volume of 1.6 l at 287 k and 0.92 atm. show your work. part 2. describe the temperature and pressure conditions at which the gas behaves like an ideal gas.

Part 1: 1.721 g/mol.

Part 2: at high T and low P.

Explanation:

Part 1:

where, P is the pressure of the gas in atm (P = 0.92 atm).

V is the volume of the gas in L (V = 1.6 L).

n is the no. of moles of the gas in mol (n = ??? mol).

R is the general gas constant (R = 0.0821 L.atm/mol.K),

T is the temperature of the gas in K (T = 287 K).

∴ n = PV/RT = (0.92 atm)(1.6 L)/(0.0821 L.atm/mol.K)(287 K) = 0.1825 mol.

n = mass/molar mass

∴ molar mass of the gas = mass/n = (0.314 g)/(0.1825 mol) = 1.721 g/mol.

Part 2:

1. Its particles have zero volume.

2. have intermolecular forces are also zero.

"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."