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Consider the ammonia reaction. N2 (g) + 3 H2 (g) rightwards harpoon over leftwards harpoon 2...

Consider the ammonia reaction. N2 (g) + 3 H2 (g) rightwards harpoon over leftwards harpoon 2 NH3 (g) KP = 0.036 at 500 K If the reaction is at equilibrium and then the volume of the container is changed from 1 liter to 5 liters, what can be said about the reaction equilibrium? both the reactant and products amounts will decrease Q > KP so the reaction will proceed toward reactants Q < KP so the reaction will proceed toward products Q = KP so the reaction will still be at equilibrium

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Answer #1

As volume is decreased, so partial pressure of each component will decrease, and system will not be at equilibrium,

As reactant side has more gaseous components, so partial pressure of reactant will decrease more, hence Q > Kp

And in order to reach equilibrium again, reaction will proceed toward reactant side,  

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