Answer:
The density of this gas is 1.079 g/L
Explanation:
Step 1: Data given
Temperature of the gas = 59.1 °C = 273.15 + 59.1 = 332.25 Kelvin
Pressure of the gas = 1.05 atm
Molar mass of the gas = 28.01 g/mol
Step 2: Calculate density
Density ρ = mass / volume
p*V = n*R*T
⇒ with p = the pressure of the gas = 1.05 atm
⇒with V= the volume of the gas = unknown
⇒ with n = the number of moles
⇒ with R = the gas constant = 0.08206 L*atm/K*mol
⇒ with T = the temperature of the gas = 332.25 Kelvin
Since we don't know the number of moles, either the volume; we will calculate n/v
n/V =P/RT
Since ρ = m/V
and mass m = moles n * Molar mass MM
We can say that: (P*MM)/RT = (n*MM)/v = m/V = ρ
so ρ = (P*MM)/RT
ρ = (1.05 atm*28.01g/mol) / (0.08206 L*atm/K*mol *332.25 Kelvin)
ρ = 1.079 g/L
The density of this gas is 1.079 g/L
