![]() ![]() The rate of effusion of sulfur dioxide through an orifice is 4.48 mL/s. Since the grams are in 1.00 L, the density is 1.10 g/Līonus Problem #2: At 25.0 ☌ and 380.0 mmHg, the density of sulfur dioxide is 1.31 g/L. N = 0.044638 mol (this is the moles of gas in 1.00 L) ![]() I will call the unknown r 2 because that will put its molar mass in the numerator (making for an easier solution sequence).ģ) Since we know everything was at STP, the density is as follows: This is a mistake that the ChemTem has made. ![]() It is a common mistake in this type of problem to use the times directly in the solution to the problem. The molecular weight of the other gas = x.Ģ) By Graham's Law (see the solution to problem #1), we have:Ġ.0004 = 2.016 / x 1.00 L / 6.60 min = 0.1515152 L/min Problem #2: What is the molecular weight of a gas which diffuses 1/50 as fast as hydrogen? It does so at 3.16 times the rate of the argon. Problem #1: If equal amounts of helium and argon are placed in a porous container and allowed to escape, which gas will escape faster and how much faster? ![]() ChemTeam: Graham's Law of Effusion: Probs 1-10 ![]()
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