What volume would 12.0 grams of helium occupy at 1.7 atmospheres of pressure and a temperature of 300 K?

Question

Quizplus · Accepted Answer

We can use the ideal gas law to solve for the volume of helium:
PV=nRT

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

First, we need to solve for the number of moles of helium using its molar mass:
n = m/M
where m is the mass in grams and M is the molar mass of helium (4.003 g/mol).

n = 12.0 g / 4.003 g/mol = 2.998 mol

Now we can plug in the values and solve for V:
V = nRT / P

V = (2.998 mol)(0.08206 L·atm/mol·K)(300 K) / 1.7 atm

V = 43.4 L

Therefore, the answer is (D) 43.4 L.

What Volume Would 12