A container was charged with hydrogen, nitrogen, and ammonia gases at 120 degree

Question

A container was charged with hydrogen, nitrogen, and ammonia gases at 120 degrees C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature?

3H2(g) + N2(g) -->2NH3(g)

a. There will be no effect.

b. More ammonia will be produced at the expense of hydrogen and nitrogen.

c. Hydrogen and nitrogen will be produced at the expense of ammonia.

d. The equilibrium constant will increase.

e. The equilibrium constant will decrease.

Please answer with an explanation for how you got that answer.

Explanation / Answer

Increasing the volume will decrease the pressure and favor the formation of reactants. According to Le Chatelier's Principle, an increase in pressure will shift the equilibrium to the side with fewer mols. When you increase the volume, the pressure decreases hence it will shift the equilibrium towards the side with more number of moles. here reactants have more number of moles. hence the equilibrium will shift towards N2+H2. so the answer is

c. Hydrogen and nitrogen will be produced at the expense of ammonia.

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