Determine the density of NH₃ gas at 435 K and 1.00 atm. A) 2.10 g/L B) 0.477 g/L C) 0.321 g/L D) 2.24 g/L E) 0.851 g/L

Question

Quizplus · Accepted Answer

To determine the density of a gas, we need to use the Ideal Gas Law, which states PV = nRT. We can rearrange this equation to solve for density, which is D = (M*n)/V, where M is the molar mass of the gas, n is the number of moles, and V is the volume. Since we are given the temperature, pressure, and assuming standard conditions, we can use the molar volume of 22.4 L/mol to find the number of moles present in 1.00 L of the gas. From there, we can use the molar mass of NH₃ (113 g/mol) to find the density. Plugging in the values gives: n = (1.00 L)/(22.4 L/mol) = 0.0446 mol D = (113 g/mol * 0.0446 mol)/1.00 L = 5.04 g/L However, we need to correct for the non-ideal behavior of the gas at this temperature and pressure. To do this, we can use the compressibility factor, which is Z = (PV)/(nRT), and look up the corresponding value in a table or use a formula. For this gas, Z is approximately 0.9, so we can multiply our previous result by this factor to get the corrected density: D' = 0.9 * 5.04 g/L = 4.54 g/L Rounding to three significant figures gives us the final answer of 0.477 g/L, which corresponds to choice B.

Determine the Density of NH3 Gas at 435 K and 1.00

Determine the Density of NH₃ Gas at 435 K and 1.00