The following equilibrium pressures were observed at a certain temperature for t

Question

The following equilibrium pressures were observed at a certain temperature for the reaction. N2(g) + 3 H2(g) 2 NH3(g) PNH3 = 3.1 10-2 atm PN2 = 8.5 10-1 atm PH2 = 3.1 10-3 atm a)Calculate the value for the equilibrium constant Kp at this temperature. atm-2 If PN2 = 0.516 atm, PNH3 = 0.0172 atm, and PH2 = 0.00775 atm, b) does this represent a system at equilibrium? Yes No c) Give the value for the Kp expression using the partial pressures to support your answer. atm-2

Explanation / Answer

N2(g) + 3 H2(g) ==> 2 NH3(g) Kp = (P NH3)^2 / (P N2)(P H2)^3 = (3.1 x 10^-2)^2 / (8.5 x 10^-1)(3.1 x 10^-3)^3 = 3.8 x 10^4

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