Co(g)+h2o(g)⇌co2(g)+h2(g) kp=0.0611 at 2000 k a reaction mixture initially contains a co partial pressure of 1320 torr and a h2o partial pressure of 1760 torr at 2000 k. calculate the equilibrium partial pressure of co2.

According to the reaction:
by set ICE table:
                   CO(g) + H2O(g) ↔ CO2(g) + H2(g)
initial         1320      1760              0              0
change        -X         -X                +X             +X
initial      (1320-X)    (1760-X)        X               X

when Kp = (pressure products)/ (pressure reactants )
 Kp = P(H2)* P(CO2) /P(CO) * P(H2O)
by substitution:
0.0611 = (X * X) / (1320-X) * (1760-X)
0.0611 = X^2 / (X^2-3080X + 2323200)

∴X = 301 torr 
∴P(CO2) = X = 301 torr

The answers is a nuclear changes