A 4.10-mole sample of helium gas at 28°C takes up a volume of 3.28 L. Determine the pressure of helium in units of atm.

n = number of mole of sample of helium gas = 4.10

T = temperature of the gas = 28 °C = 28 + 273 = 301 K

V = Volume of helium gas = 3.28 L = 0.00328 m³

P = pressure of the helium gas

Using the equation

P V = n R T

P (0.00328) = (4.10) (8.314) (301)

P = 3.13 x 10⁶ Pa

P = (3.13 x 10⁶ Pa) (1 atm / (101325 Pa))

P = (3.13 x 10⁶) atm / (101325)

P = 30.89 atm