Answer :
To determine the mass of Neon gas in a 38.4 L tank at 41°C and 3.99 atm, use the Ideal Gas Law with the temperature converted to Kelvin and then multiply the number of moles by the molar mass of Neon to find that the tank contains approximately 100.29 grams of Neon gas.
To calculate the mass of Neon gas in a 38.4 L tank at 41°C and 3.99 atm of pressure, we can use the Ideal Gas Law, which is PV = nRT, where P is the pressure, V is the volume, T is the temperature in Kelvin, n is the number of moles, and R is the gas constant (0.0821 L·atm/mol·K).
First, convert the temperature to Kelvin:
T(K) = 41°C + 273.15 = 314.15 K
Now, rearrange the Ideal Gas Law to solve for n (number of moles):
n = PV / RT
Substitute the given values into the equation:
n = (3.99 atm * 38.4 L) / (0.0821 L·atm/mol·K * 314.15 K)
Calculate the number of moles of Neon gas:
n ≈ 4.97 moles
To find the mass, we multiply the moles by the molar mass of Neon (20.18 g/mol):
mass = n * molar mass of Ne
Calculate the mass of the Neon gas:
mass ≈ 4.97 moles * 20.18 g/mol
= 100.29 grams
Therefore, the tank contains approximately 100.29 grams of Neon gas.
