Consider the following homogeneous equilibria: N_2 (g) + 3H_2 (g) irreversible 2

Question

Consider the following homogeneous equilibria: N_2 (g) + 3H_2 (g) irreversible 2 NH_3 (g) Delta H degree = -45.9 kJ/mole at equilibrium. How will the system respond to the following changes? (According to the rules of lessthanorequalto Chatelier's principal). Would the reaction shift to the right or left? Answer (shifts right or shifts left) Increase the concentration of hydrogen gas. Increase the concentration of nitrogen gas. Increase the concentration of ammonia gas. Add more ammonia gas. Add more nitrogen gas. Remove ammonia gas. Add Xenon gas. Increase the pressure. Decrease the pressure. Increase the volume. Decrease the volume. Add heat.

Explanation / Answer

1. increasing concentration of a reactant will favour shift to products, so shift goes to right

2 increasing concentration of a reactant will favour shift to products, so shift goes to right

3  increasing concentration of a product will favour shift to reactant , so shift goes to left

4 increasing mass (gas) of a product will favour shift to reactant , so shift goes to left

5 increasing mass (gas) of a reactant will favour shift to product , so shift goes to right

6 decreasing mass (gas) of a product will favour shift to product , so shift goes to right

7 adding an inert gas favours least mol formation, since system gets pressurized this is products, i.e. shift to the rigth

8 increasing P favours least mol formation, since system gets pressurized this is products, i.e. shift to the rigth

9 decreasing P favours most mol formation, since system gets pressurized this is products, i.e. shift to the left

10 increasing Volume decreases P, so decreasing P favours most mol formation, since system gets pressurized this is products, i.e. shift to the left

11 Adding HEat favours reactants (shift to the left) since this is exothermic, so reaciton releases heat

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