1. Convert Pressure to Atmospheres
* 1 atm = 760 torr
* 7.50 x 10² torr * (1 atm / 760 torr) = 0.987 atm
2. Convert Temperature to Kelvin
* K = °C + 273.15
* 25.0°C + 273.15 = 298.15 K
3. Use the Ideal Gas Law
The ideal gas law is: PV = nRT
* P = Pressure (in atm) = 0.987 atm
* V = Volume (in L)
* n = Moles of gas
* R = Ideal gas constant = 0.0821 L atm/mol K
* T = Temperature (in K) = 298.15 K
We want to find the density (ρ), which is mass (m) per unit volume (V):
* ρ = m/V
We can rearrange the ideal gas law to solve for density:
* n/V = P/RT
* Since n = m/M (where M is molar mass), we can substitute:
* (m/M)/V = P/RT
* ρ = (m/V) = (PM)/RT
4. Calculate Density
* ρ = (0.987 atm * 70.9 g/mol) / (0.0821 L atm/mol K * 298.15 K)
* ρ ≈ 2.84 g/L
Therefore, the density of chlorine gas at 7.50 x 10² torr and 25.0°C is approximately 2.84 g/L.
