Question

What is the volume of 2.3 mol of helium at 17 C and 0.89 atm? Assume helium behaves as an ideal gas.

Answer 1

39.446L

Step-by-step explanation:

since helium is ideal gas, we can use PV = nRT

P = pressure

V = volume

n = moles

R = gas constant

T = temperature in Kelvin

we are solving for V

V =
`(nRT)/(P)`

C to K temp transfer: K = C + 273, so K = 290 since C = 17

our gas constant is 0.08206 atm L/mol K, this gas constant r will change depending on what unit of pressure you are using (mmHg, atm, etc).

plug and chug

V =
`((2.3mol)(290K)((0.08206 atmL)/(molK)) )/(1 atm)`

canceling out units

V =
`(2.3 * 209 * 0.08206L)/(1)` = 39.446