What are the equilibrium partial pressures of pcl3 , cl2, and pcl5, respectively? express your answers numerically in atmospheres with three digits after the decimal point, separated by commas?

The question is incomplete, so I tried to find a similar problem online. It is shown in the attached picture. The reaction is

PCl₃ + Cl₂ ⇆ PCl₅

Then, we use the ICE (Initial-Change-Excess) approach as follows:

        PCl₃ + Cl₂ ⇆ PCl₅
I        0.5      0.5      0.3
C      -x         -x        +x
E    0.5-x    0.5-x    0.3+x

Total pressure: 0.5 - x + 0.5 - x + 0.3 + x = 1.3 

Kp = [PCl₅]/[PCl₃][Cl₂]
0.18 = (0.3+x)/(0.5-x)²
Solving for x,
x= 0.21

Partial pressures would be:
PCl₃ = 0.5 - 0.21 = 0.29 atm
Cl₂ = 0.5 - 0.21 = 0.29 atm
PCl₅ = 0.3+0.21 = 0.51 atm

I'm sorry but i'm only grade

The answer would be true