Question

What is the density of a sample of hydrogen gas that exerts 2.85 atm of pressure at 225K? Select the correct answer below. O 2.881 01.29 O 0.31] O 0.957 FEEDBACK MORE INSTRUCTIC

Answer 1

By ideal gas

PV = nRT

or, P = $\frac{nRT}{V}$

or, P =

WRT MV

or, P =$\frac{dRT}{M}$

,or d =(PM/RT)

P is pressure , d is density, T is temperature in kelvin , M is molar mass, R is universal gas constant .

Given, P = 2.85 atm

T = 225 K

Molar mass of Hydrogen (M) = 2 g/mol.

R = 0.082 L-atm /mol.K.

so, d = ( PM/RT)

putting the values

density (d) =

[2.85atm ×2(g/mol)/0.082(Latm/molK)×225 K]

or, d = 0.31 (g/L) .