A 5.00 L container of unknown gas at 25.0 °C has a pressure of 2.45 atm.The mass of the gas is 32.1 g.What gas is in the container? A)Cl₂ B)F₂ C)NO₂ D)SO₃ E)SO₂

Question

Quizplus · Accepted Answer

We can use the ideal gas law to calculate the number of moles of gas present: PV = nRT n = PV/RT n = (2.45 atm)(5.00 L)/(0.0821 L·atm/mol·K)(298 K) (using T=25°C=298 K) n = 0.501 mol Next, we can use the molar mass of the gas to determine its identity: m/molar mass = n m/ (molar mass) = (0.501 mol) m = 0.501 mol x (molar mass) m = 0.501 mol x (32.1 g/mol) m = 16.1 g Since the mass of the gas in the container is 32.1 g, we can conclude that the gas is sulfur dioxide (SO2), which has a molar mass of 64.1 g/mol. Therefore, the answer is E) SO₂.

A 500 L Container of Unknown Gas at 25