What would happen if the following chemical were added to each of the chemical s

Question

What would happen if the following chemical were added to each of the chemical system at equilibrium? Add ammonia to 4NH_3 (g) + 5O_2(g) 4NO(g) + 6H_20(g) Add nitrogen to 2N_20(g) + N_2H_4(g) 3N_2 (g) + 2H_20(g) Add sulfuric acid to CH_3COOH(aq) + H_20(t) CH_3COO^-(aq) + H_3O^+(aq) Add hydrogen gas to H_2(g) + I_2(g) 2Hl(g) Add sodium hydroxide to Mg(OH)_2(s) Mg^2+ (aq) + 2Oh^- 9aq)Add hear to S0_2CI_2(g) S0_2(g) + Cl_2(g); Delta H = +67 kJ Add solid magnesium hydroxide to Mg (OH)_2 (s) Mg^2+ (aq) + 2Oh^-(aq)

Explanation / Answer

According to le chatelier's principle we can explain the change of equilibrium:

a.

if ammonia is added, there is an increase of concentration on reactant side, so the equilibrium will shift to right i.e., forward direction

b.

if nitrogen is added there is an increase of concentration of products, so the equilibrium will shift towards left i.e, backward direction.

c.

if sulphuric acid is added there is an increase of concentration of H+ ions i.e., increase of concentration on product side, so the equilibrium will shift towards to leftside i.e., backward direction

d.

hydrogen gas is added there is an increase of concentration on reactant side, so the equilibrium will shifts towards right i.e, forward direction.

e.

sodium hydroxide is added there is an increase of concentration of OH-ions on product side, so the equilibrium will shifts towards left i.e., backward direction

f.

It is endothermic reaction, so if heat is added the equilibrium shifts to right i.e., forward direction

g.

Addition of magnesium hydroxide will enhance the concentration of hydroxyl ions i.e., the product concentration increases so the equilibrium will shifts towards to left., i.e., backward direction.

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