Ask Question
6 July, 09:15

An unknown gas at 59.1 ∘C and 1.05 atm has a molar mass of 28.01 g/mol. Assuming ideal behavior, what is the density of the gas?

+5
Answers (1)
  1. 6 July, 09:45
    0
    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
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “An unknown gas at 59.1 ∘C and 1.05 atm has a molar mass of 28.01 g/mol. Assuming ideal behavior, what is the density of the gas? ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers