Question

At 25°C, gaseous decomposes to and to the extent that 14.5% of the original (by moles) has decomposed to reach equilibrium. The total pressure (at equilibrium) is 0.670 atm. Calculate the value of for this system.

Answer 1

The value of Kp for the system = 0.0128 atm

Step-by-step explanation:

Let, the gaseous substance is SO₂Cl₂

SO₂Cl₂ ⇄ SO₂ + Cl₂

Initially x 0 0

At equilibrium (x - 14.5%x) 14.5%x 14.5%x

= 85.5 % x

Total moles of gases at equilibrium

= 85.5 % x + 14.5%x + 14.5%x

= 114.5 % x

Partial pressure of SO₂ (
`Pso_(2)`) =
`(14.5x)/(114.5x) X0.67= 0.08`

Partial pressure of Cl₂
`(Pcl_(2)) =(14.5x)/(114.5x) X0.67 = 0.08`

Partial pressure of SO₂Cl₂
`(Pso_(2)cl_(2) )=(85.5x)/(114.5x) X0.67= 0.5`

So,

`Kp = (Pso_(2) XPcl_(2) )/(Pso_(2)cl_(2))\\ \\=(0.08X0.08)/(0.5) \\\\=0.0128`