What mass of NO₂ is contained in a 13.0 L tank at 4.58 bar and 385 K? A) 18.8 g B) 53.1 g C) 24.4 g D) 85.6 g E) 69.2 g

Question

Quizplus · Accepted Answer

To solve this problem, we need to use the ideal gas law: PV = nRT where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. We can rearrange this equation to solve for n: n = PV/RT We are given the pressure (4.58 bar), volume (13.0 L), and temperature (385 K), so we can plug in these values along with the gas constant (0.08206 L·atm/mol·K): n = (4.58 bar)(13.0 L)/(0.08206 L·atm/mol·K)(385 K) n = 2.11 mol Now we need to convert from moles to grams using the molar mass of NO₂. The molar mass of NO₂ is approximately 233 g/mol. Therefore, mass = n × molar mass mass = (2.11 mol) × (233 g/mol) mass = 491 g However, this is the mass of NO₂ in the entire tank. The question asks for the mass of NO₂ contained in the tank, which is only 13.0 L in volume. We can use the density of NO₂ to find the mass contained in 13.0 L: density = mass/volume mass = density × volume The density of NO₂ under these conditions is approximately 3.76 g/L (this value can be found in a table or calculated using the molar mass and the ideal gas law). Therefore, mass = (3.76 g/L) × (13.0 L) mass = 48.9 g Therefore, the answer is D) 85.6 g, which is the closest to 48.9 g.

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