Answer :
the density of nitrogen gas at 44.8ºC and 141 kPa is approximately 0.807 kg/m³.
The density of nitrogen gas (N2) at 44.8ºC (114.35ºF) and 141 kPa (1.05 atm) is approximately 0.807 kg/m³. This value can be found using the ideal gas law and the known values for temperature, pressure, and molecular weight of nitrogen (28.013 g/mol). The calculation is as follows:
P = n * R * T / V
where P is the pressure (in this case, 141 kPa), n is the number of moles of gas (in this case, we're not given a specific volume, so we'll assume a volume of 1 liter), R is the ideal gas constant (8.31 J/mol·K), and T is the absolute temperature (in this case, 44.8ºC + 273.15 K = 318.05 K).
Substituting these values into the ideal gas law and solving for V:
V = n * R * T / P
V = (1 mol) * (8.31 J/mol·K) * (318.05 K) / (141 kPa)
V = 0.0222 m³/mol
Now we can find the density by dividing the mass of one mole of nitrogen by its volume:
Density = Mass / Volume
Density = (28.013 g/mol) / (0.0222 m³/mol)
Density = 1,265 g/L = 0.807 kg/m³
Therefore, the density of nitrogen gas at 44.8ºC and 141 kPa is approximately 0.807 kg/m³.
