Final answer:
The volume occupied by 2.0g of helium at 25°C and a pressure of 106kPa, using the Ideal Gas Law, is approximately b. 8.0 L. The temperature is converted to Kelvins, the mass of helium is converted to moles, and then these values along with the pressure are plugged into the Ideal Gas Law to find the volume.
Step-by-step explanation:
To determine the volume occupied by 2.0g of He (helium) at 25°C and a pressure of 106kPa, we can use the Ideal Gas Law, which is PV = nRT, where P is pressure, V is volume, n is number of moles, R is the universal gas constant, and T is the temperature in Kelvins.
First, we need to convert the mass of helium into moles by using the molar mass of helium (4.00 g/mol):
- moles of He = mass (2.0g) ÷ molar mass (4 g/mol) = 0.50 moles
Next, we convert the temperature into Kelvins:
- T = 25°C + 273.15 = 298.15 K
Since the universal gas constant R is 8.314 J/(mol·K), we can plug in the values to solve for V:
- V = (nRT) ÷ P = (0.50 moles × 8.314 J/(mol·K) × 298.15 K) ÷ 106000 Pa
Note that the pressure must be in Pascals (Pa), where 1 kPa = 1000 Pa.
After calculating, the volume V is found to be approximately 8.0 L, so the correct answer is B) 8.0 L.