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.

Question

How do I solve this. What’s the formula

Answer 1

Assume an ideal gas and work with

PV = nRT

P = nRT/V

n = number of moles = 4.10

R = universal gas constant (look it up in your book, in appropriate units)

T = absolute temperature = (28 + 273) kelvins

V = volume = 3.28 L

P = pressure (should come out in atm if you have R in the appropriate units)