The density of NO2 gas at 25.0 °C and 2.56 atm is approximately 4.82 g/L based on the step-by-step calculation using the ideal gas law and the molar mass of NO2.
Certainly, let's go through the step-by-step calculation for the density of NO2 gas at 25.0 °C and 2.56 atm using the ideal gas law. 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 in Kelvin.
Convert Temperature to Kelvin:
T = 25.0 °C + 273.15 = 298.15 K
Rearrange Ideal Gas Law to Solve for n/V:
n/V = P/RT
Solve for n:
n = (2.56 atm * V) / (0.0821 L·atm/(mol·K) * 298.15 K)
Calculate Mass (m) using Molar Mass (M) of NO2:
m = n * M = (2.56 atm * V * 46 g/mol) / (0.0821 L·atm/(mol·K) * 298.15 K)
Use Density Formula (d = m/V):
d = P * M / (R * T) = (2.56 atm * 46 g/mol) / (0.0821 L·atm/(mol·K) * 298.15 K)
Perform the Calculation:
d ≈ 117.76 / 24.422 ≈ 4.82 g/L