Changing the catalyst.
Lowering the temperature.
Lowering the pressure.
Removing some of the hydrogen.
The reaction stops.
Equal amounts of reactants and products are present.
The ratio of the product concentration to the reactant concentration is constant.
The products of the forward reaction stop reacting altogether.
Adding more of A
Lowering the temperature
Removing some of C
Increasing the pressure
2NO (g) + O2(aq) 2NO2 (g)
N2 (g) + 3H2 (g) 2NH3 (g)
2NO2 (g) N2O4 (g)
CH4 (g) + H2O (g) CO (g) + 3H2 (g)
At equilibrium, the rate of the forward reaction is equal to the rate of the backward reaction.
The concentration of all reactants and products are independent of the external pressure.
Addition of dilute hydrochloric acid to precipitate silver chloride would cause the equilibrium to shift to the left.
The yield of silver metal could be significantly increased by adding a catalyst.
The system responds in a way so as to counteract the decreased temperature.
The system favours the forward reaction which is exothermic.
The system favours the forward reaction which is endothermic.
The system responds in a way in accordance with Le Chatelier's principle, replacing the heat lost by raising the temperature.
The volume of gas molecules decreases in the forward reaction.
The number of moles of gas molecules increases in the forward reaction.
An increase in pressure due to decreasing volume causes the reaction to shift to the side with the fewer moles of gas.
The position of equilibrium shifts to the right to favour the forward reaction.