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.

a galvanic cell( aka voltaic cell) and electrolytic cell

explanation:

stan bts (kpop group)

follow my insta yoongi_jams

subscribe to my yt yoongi jmz

answer: c.

explanation: