Question

Calculate the density of NO₂ (g) at 50°C and 0.85 atm.

a) 2.3 g/L
b) 2.7 g/L
c) 3.1 g/L
d) 3.5 g/L

Answer 1

To calculate the density of NO₂ gas at 50°C and 0.85 atm, use the Ideal Gas Law to find the molar volume and divide the molar mass of NO₂ (46.01 g/mol) by this volume. The exact density value can be obtained by performing this calculation.

Step-by-step explanation:

To calculate the density of NO₂ (g) at 50°C and 0.85 atm, we can use the Ideal Gas Law, which relates the pressure (P), volume (V), temperature (T), and moles (n) of a gas through the equation PV = nRT.

The molar mass of NO₂ is needed for the density calculation and can be found by adding the molar masses of nitrogen (N) and oxygen (O) atoms. For NO₂, its molar mass is approximately 46.01 g/mol (14.01 for nitrogen plus 16.00 for each of the two oxygen atoms).

First, convert the temperature from Celsius to Kelvin: T(K) = 50°C + 273 = 323 K. Then, use the Ideal Gas Law rearranged to solve for the molar volume (V/n):

V/n = RT/P = (0.0821 L.atm.mol⁻¹.K⁻¹)(323 K) / 0.85 atm

Now we calculate the molar volume, and then use the molar mass of NO₂ to find its density (ρ = molar mass / molar volume):

ρ = 46.01 g/mol / V/n
The calculated value gives us the density of NO₂ at the specified conditions.