Final answer:
The density of dinitrogen monoxide (laughing gas) at 325 K and a pressure of 113.0 kPa is calculated using PV = nRT and the molar mass of N₂O. The result is approximately 1.96 g/L, which does not match the provided answer choices.
Step-by-step explanation:
The density of laughing gas, dinitrogen monoxide, N₂O, at a temperature of 325 K and a pressure of 113.0 kPa, can be calculated using the Ideal Gas Law, which is expressed as PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. To find the density, we also need the molar mass of N₂O, which is 44.01 g/mol.
The gas constant (R) in appropriate units is 8.3145 L·kPa·K⁻¹·mol⁻¹. The formula for density (ρ) in terms of the Ideal Gas Law is ρ = (PM)/(RT). Substituting the values for laughing gas at the given conditions, ρ = (113.0 kPa)(44.01 g/mol) / (8.3145 L·kPa·K⁻¹·mol⁻¹)(325 K), yields the density of N₂O under these conditions.
Performing the calculation gives a density of ρ ≈ 1.96 g/L, which is not listed among the answer choices provided. However, based on the options presented, the calculated value may need to be verified for precision or the options might need to be reviewed for accuracy.