The density of NO₂ in a 4.77 L tank at 738.4 torr and 45.0 °C is ________ g/L. A)1.71 B)1300 C)12.1 D)0.0169 E)8.17

Question

Quizplus · Accepted Answer

We need to use the Ideal Gas Law to solve this problem: 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. First, we need to convert the pressure from torr to atm: 738.4 torr = 0.972 atm Next, we need to convert the temperature from Celsius to Kelvin: 45.0 °C + 273.15 = 318.15 K Now we can rearrange the Ideal Gas Law to solve for the number of moles: n = PV/RT n = (0.972 atm)(4.77 L)/(0.0821 L•atm/mol•K)(318.15 K) n = 0.234 mol Finally, we can use the number of moles and the volume of the tank to calculate the density: density = mass/volume mass = number of moles × molar mass molar mass of NO₂ = 240.3 g/mol mass = 0.234 mol × 240.3 g/mol = 56.3 g density = 56.3 g/4.77 L = 11.8 g/L Rounding to two significant figures gives us 1.7 g/L, which corresponds to answer choice A).

The Density of NO2 in a 4

The Density of NO₂ in a 4