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If C + CO2 <--> Co, when equilibirum is established at 1000 K, the total pressure in the system is 4.70 atm. If Kp= 1.72, what are the partial pressures of CO and CO2?

  • Chemistry -

    C(g) + CO2(g) ==> CO(g)

    Kp = 1.72 = pCO/pCO2
    I would set up an ICE chart where p = pressure of CO and 4.70 = pressure CO2 at equilibrium. Substitute into Kp expression and solve for p.

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