At 450oC, Kp = 6.5 × 10-3 for the ammonia synthesis reaction. Assume that a reaction vessel with a movable piston initially contains 3.0 moles of H2(g) and 1.0 mole of N2(g). Make a plot to show how the partial pressure of NH3(g) present at equilibrium varies for the total pressures of 1.0 atm, 10.0 atm, 100. atm, and 1000. atm (assuming that Kp remains constant). [Assume these total pressures represent the initial total pressure of H2(g) plus N2(g), where PNH3 = 0.]
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