Question

A sample of chlorine gas has a density of g\L At a pressure of 1.04 for ATM and a temperature of 34°C. Assume Ideal behavior

Answer 1

Answer:

2.93 g/L

Explanation:

We can use the Ideal Gas Law to calculate the density of chlorine.

   pV = nRT

      n = m/M                                  Substitute for n

   pV = (m/M)RT                            Multiply both sides by M

pVM = mRT                                   Divide both sides by V

  pM = (m/V) RT

     ρ = m/V                                   Substitute for m/V

 pM = ρRT                                    Divide each side by RT

    ρ = (pM)/(RT)

===============

p = 1.04 atm

M = 70.91 g/mol

R = 0.082 06 L·atm·K⁻¹mol⁻¹

T = 34 °C = 307.15 K                     Solve for ρ

===============

ρ = (1.04 × 70.91)/(0.082 06 × 307.15)

ρ = 73.74/25.20

ρ = 2.93 g/L