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Water can decompose at an elevated temperature to give hydrogen and oxygen according to the equation below. At a particular temperature, the partial pressures of H2O, H2, and O2 are 0.055 atm, 0.0065 atm, and 0.0045 atm, respectively, at equilibrium. What is the value of the equilibrium constant, KP, for this reaction at this temperature?
2H2O(g) ? 2H2(g) + O2(g)
At 1045 K the partial pressures of an equilibrium mixture of H2O, H2, and O2 are 0.040, 0.0045, and 0.0030 atm, respectively. Calculate the value of the equilibrium constant Kp at 1045 K.
2 H2O <---> 2 H2 + O2
4. For the system, CO(g) + H2O(g) รขยย H2(g) + CO2(g), K = 1.30 at a certain temperature. If the partial pressure of CO and H2O is 0.355 atm and that for H2 and CO2 is 0.310 atm, what are the partial pressures of all four at equilibrium?