what would happen to a weak base dissociation equilibrium if more products
were added?
a. the equilibrium constant would shift to a new constant
o
b. the concentration of reactants would increase.
o
c. the equilibrium concentrations would stay the same,
d. the concentration of products would increase

Both B and D are correct.

Explanation:

B + H₂O ⇌ BH⁺ + OH⁻

If you add more products, the position of equilibrium will shift to the left to decrease their concentrations (Le Châtelier's Principle). The concentration of reactants will increase, but the equilibrium concentrations of products will also be higher than they were initially.

A is wrong. The equilibrium constant is a constant. It does not change when you change concentrations.

C is wrong. Per Le Châtelier's Principle, the concentrations must change when you ad a stress to a system at equilibrium.

(This is a poorly-worded question. "They" are probably expecting answer D.)

the equation that correctly represent the reaction for formation of ammonia is

n2+ 3h2 → 2nh3 (answer d)

1 mole of nitrogen gas (n2) react with 3 moles of hydrogen gas (h2) to form 2 moles of ammonia ( nh3). this is in a process known as haber process were iron is used as a catalyst and reaction take place that a higher temperature and pressure. the process is exothermic hence energy is released.

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