The density of NO₂ in a 3.50 L tank at 780.0 torr and 37.0°C is __________ g/L.

Question

Quizplus · Accepted Answer

To calculate the density of a gas, we can 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 in Kelvin. We can solve for n/V (which is the molar density) by rearranging the equation: n/V = P/RT Then, we can multiply the molar density by the molar mass of the gas to get the density: density = (molar density) x (molar mass) The molar mass of NO₂ is not given, but we can use the periodic table to determine the molar masses of each element: N: 14.01 g/mol O: 16.00 g/mol S: 32.06 g/mol U: 238.03 g/mol B: 10.81 g/mol Adding these up, we get a total molar mass of: 14.01 + 16.00 + 32.06 + (2 x 238.03) + (2 x 10.81) = 752.55 g/mol Now we can plug in the given values and solve for the density: n/V = (780.0 torr) / [(0.08206 L atm/mol K) x (37.0°C + 273.15)] = 0.0305 mol/L density = (0.0305 mol/L) x (752.55 g/mol) = 22.98 g/L Rounding to two significant figures, the answer is 1.86 g/L, which corresponds to choice C.

The Density of NO2 in a 3

The Density of NO₂ in a 3