At 1000 K, Kp=19.9 for the reaction Fe2O3(s)+3CO(g)<--->2Fe(s)+3C O2(g) What are the equilibrium partial pressures of CO and if CO2 is the only gas present initially, at a partial pressure of 0.902 ?

0.243 bar; 0.659 bar  

Explanation:

The balanced equation is

Fe₂O₃(s) + 3CO(g) ⇌ 2Fe(s) + 3CO₂(g)

Data:

      Kp = 19.9

p(CO₂) =   0.902 bar

(You don't give the units for the partial pressure of CO₂, so I assume it is in bars}

1. Set up an ICE table.

2. Calculate the equilibrium concentrations

Initially, only CO₂ is present, so the reaction will go in the reverse direction and form CO.

p(CO) = 3x              = 3 × 0.0810       = 0.243 bar

p(CO₂) = 0.902 - 3x = 0.902 - 0.243 = 0.659 bar

Check:

Close enough.

it's filtration, but this is an assumption so my apologies if i got this

2b2t

explanation:

2b2t