Question

The density of NO2 in a 4.50 L tank at 760.0 torr and 25.0 °C is ________ g/l.

A) 1.64.
B) 9.30.
C) 1.68.
D) 1.88.
E) 3.27

Answer 1

The density of NO2 in a 4.50 L tank at 760.0 torr and 25.0 °C is approximately 1.64 g/L.

Step-by-step explanation:

To calculate the density of NO2 in a 4.50 L tank at 760.0 torr and 25.0 °C, we can use the ideal gas law and the molar mass of NO2. The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Rearranging the equation, we have n = PV/RT. First, we need to calculate the number of moles of NO2 in the tank. We can calculate this by dividing the pressure in torr by the ideal gas constant (0.08206 L atm/K mol), multiplied by the temperature in Kelvin. Then we can divide the calculated number of moles by the volume of the tank to get the molar concentration. Finally, we can divide the mass of NO2 by the volume of the tank to get the density. Using this method, the density of NO2 in the 4.50 L tank at 760.0 torr and 25.0 °C is approximately 1.64 g/L (Option A).