The density of N₂O at 1.53 atm and 45.2 °C is g/L. A) 9.99 B) 0.388 C) 1.76 D) 18.2 E) 2.58

Question

Quizplus · Accepted Answer

To calculate the density, we can use the ideal gas law: PV = nRT where P is the pressure in atm, V is the volume in L, n is the number of moles, R is the gas constant (0.0821 L·atm/mol·K), and T is the temperature in K (converted from 45.2 °C to 318.35 K). We can rearrange the equation to find the number of moles: n = PV/RT We can then use the molar mass of N₂O (which we will assume is given) to convert moles to grams: m = n × MM where MM is the molar mass in g/mol. Finally, we can divide the mass by the volume to get the density: ρ = m/V Putting it all together, we get: n = (1.53 atm) × V / [(0.0821 L·atm/mol·K) × (318.35 K)] n = 0.0612 V m = n × MM ρ = m/V = (n × MM) / V Without the molar mass, we cannot calculate the density, so we cannot determine the answer.

The Density of N2O at 1

The Density of N₂O at 1