A container with a one-liter capacity at 27°C is filled with helium to a pressure of 2.0 atm. (1 atm = 1.0 × 10⁵ N/m².) How many moles of helium does it hold?

Question

Quizplus · Accepted Answer

We can use the Ideal Gas Law to solve for the number of moles of helium:

PV = nRT

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

First, we need to convert the temperature from Celsius to Kelvin:

T = 27°C + 273 = 300 K

We can then rearrange the Ideal Gas Law to solve for n:

n = PV/RT

Plugging in the given values, we get:

n = (2.0 atm)(1.0 L)/(0.0821 L*atm/mol*K)(300 K) = 0.081 mol

Therefore, the container holds 0.081 moles of helium, which is answer choice B.

A Container with a One-Liter Capacity at 27°C Is Filled