Question

16 grams of helium gas (He) applies 380 mmHg pressure at a temperature of 0 °C. Assume ideal gas behavior. The ideal gas constant is 62.36 (L· mmHg)/(K·mol), and the molar mass of helium is 4 g/mol. (Hint: Remember that temperature needs to be in Kelvins.)How much volume does the gas occupy?

Answer 1

D. 179.2 L

Step-by-step explanation

Given parameters:

Molar mass of He, M = 4 g/mol

Reacting mass of He, m = 16 grams

Pressure, P = 380 mmHg

Temperature, T = 0 °C = 0 + 273 K = 273 K

Ideal gas constant, R = 62.36 (L· mmHg)/(K·mol)

What to find:

The volume, V that the gas occupies.

Step-by-step solution:

The ideal gas equation formula is PV = nRT

But n = reacting mass/molar mass. i.e m/M

Therefore, the ideal gas equation becomes:

`PV=(m)/(M)RT`

Substitute the values of P, R, T, and M into the equation to get V:

`\begin{gathered} 380* V=(16)/(4)*62.36*273 \\ 380V=4*62.36*273 \\ 380V=68097.12 \\ \text{Divide both sides by 380} \\ (380V)/(380)=(68097.12)/(380) \\ V=179.2\text{ L} \end{gathered}`

Hence, the gas occupies 179.2 L.