Question

calculate the pressure in atm of 1.0 mole of helium in a 2.0 dm3 container at 20.0 degree celsius​

Answer 1

Answer:

No. of moles of helium, n = 1.0 mole

Volume, V = 2.0 dm³ = 2 L ……. [∵ 1 dm³ = 1 L]

Temperature, T = 20 ℃ = 20 + 273 K = 293 K

Ideal gas constant , R = 0.082057 L atm mol⁻¹ K⁻¹

Let the pressure in atm be denoted as “P” .

Using the Ideal Gas Law, we get

PV = nRT

⇒ P = nRT/V

⇒ P = [1 * 0.082057 * 293] / 2

⇒ P = 12.02 atm

Hence, the pressure is 12.02 atm .