Final answer:
The density of dinitrogen monoxide gas at 30°C and 1 atm is found using the Ideal Gas Law, and by substituting the known values including its molar mass, is 0.591 g/L.
Step-by-step explanation:
The density of dinitrogen monoxide gas at 30°C and 1 atm pressure can be calculated using the ideal gas law equation PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the temperature from Celsius to Kelvin. T(K) = T(C) + 273.15 = 30 + 273.15 = 303.15 K.
Next, we can rearrange the ideal gas law equation to solve for density, which is mass divided by volume. The molar mass of dinitrogen monoxide gas (N2O) is 44.013 g/mol.
Therefore, the density of dinitrogen monoxide gas at 30°C and 1 atm pressure is:
Density = (Molar mass x Pressure) / (R x Temperature)
Density = (44.013 g/mol x 1 atm) / (0.0821 L.atm.mol-1K-1 x 303.15 K) = 0.591 g/L.
The density of dinitrogen monoxide gas at 30°C (which is 303K) and 1 atm pressure can be calculated using the Ideal Gas Law formula, which is PV = nRT. Where P is the pressure, V is volume, n is the number of moles, R is the ideal gas constant and T is the temperature in Kelvin. First, we determine the volume that one mole of gas occupies under these conditions. Using the provided information and the formula (molar mass)P/(RT), we can rearrange for density (ρ) to be ρ = (molar mass)(P)/(RT). The molar mass of dinitrogen monoxide (N₂O) is 44.01 g/mol. Substituting the values, we get ρ = (44.01 g/mol)(1.00 atm) / ((0.0821 L.atm.mol⁻¹K⁻¹)(303K)). This calculation will yield the density in g/L.