What is the density of carbon dioxide gas at –25.2°c and 98.0 kpa? (r = 0.08206 l • atm/k • mol, 1 atm = 101,325 pa)

Answer is: 2,09 g/L.
T (CO₂) = -25,2°C = -25,2 + 273,15 = 247.95 K, temperature.
p (CO₂) = 98 kPa = 0.967 atm, pressure.
R = 0.08206 L • atm/K, gas constant.
Ideal gas law pV =nRT, can write down pV = (m/M)RT.
m - mass, M - molar mass.
Since density is: d = m/V, can write MPV=mRT and than (M·P)/(R·T) = m/V.
d = 44g/mol · 0,967atm / 0,08206 L • atm/K · 247.95 K = 2,09 g/L.

Is there a diagram/picture you can provide? it seems this question goes along with a

It is a product