Answer: Cl2 (Chlorine Gas)
Step-by-step explanation:
To determine the identity of the unknown gas, we can use the ideal gas law:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant
T = Temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin:
4°C + 273.15 = 277.15 K
Now, we can rearrange the ideal gas law to solve for the number of moles (n):
n = PV / RT
Plugging in the values:
n = (2.4 atm) * (4.22 g/L) / [(0.0821 L atm / mol K) * 277.15 K]
n ≈ 0.245 moles
Now that we have the number of moles, we can use the molar mass of the gas to identify it. The molar mass is calculated as:
Molar mass = Mass (g) / Moles (n)
Let's assume that the molar mass of the gas is M grams per mole.
Molar mass = 4.22 g / 0.245 moles ≈ 17.22 g/mol
Now, you need to find a gas with a molar mass close to 17.22 g/mol. This molar mass is approximately that of chlorine gas (Cl2), so the unknown gas could be chlorine gas, assuming it behaves ideally under these conditions.