What volume would 2.4 moles of SF6 occupy at 0 °C and 1 atm?

To solve this problem, we can use the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles of the gas and the temperature, and inversely proportional to the pressure. The ideal gas law is usually written as PV=nRT, where:

P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

Given: n = 2.4 moles R = 0.0821 L·atm/(K·mol) (This is the value of the ideal gas constant in these units) T = 0 °C = 273.15 K (We have to convert the temperature to Kelvin because the ideal gas law requires it) P = 1 atm

We can solve for V by rearranging the ideal gas law to V=nRT/P.

Substituting the given values into this equation gives:

V = (2.4 moles)(0.0821 L·atm/(K·mol))(273.15 K) / 1 atm = 53.9 L

So, 2.4 moles of SF6 would occupy a volume of 53.9 liters at 0 °C and 1 atm.