If the molecular weight of air is 28.9, what is the density of air at atmospheric pressure and a temperature of 354.5 k? 1 atm = 1.013 × 105 n/m2 , the mass of a proton is 1.67262 × 10−27 kg , avogadro’s number is 6.02214 × 1023 mol−1 and k = 1.38065 × 10−23 n · m/k . answer in units of kg/m3

0.993 kg/m³

Explanation:

If the molecular weight of air is 28.9, what is the density of air at atmospheric pressure and a temperature of 354.5 K?

We can calculate the density (ρ) of air using the ideal gas equation.

where,

P is the pressure (P = 1.00 atm)

V is the volume

n is the number of moles

m is the mass

M is the molar mass (28.9 g/mol)

R is the ideal gas constant (0.08206 atm.L/mol.K)

T is the temperature (T = 354.5K)

the body's situation won't change the forces are equal opposit and on the same body

multiply 2kg by latent heat of vap