For a beaker containing the reaction below that is at equilibrium, using LeChatlier's Principle, predict which way the equilibrium conditions will shift (type in left, right, or no change) if silver chloride was added to a beaker.
AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)

LeChatlier's principle states that any change in pressure, temperature, or concentration of a reactant applied to a system in equilibrium, the equilibrium will shift so as to tend to counteract the effect of the change.

In our question,[tex]AgCl[/tex] is added.

[tex]AgCl[/tex] is a product.

When product concentration increases,the reaction goes to the left so as to decrease the product concentration.

For a beaker containing the reaction below that is at equilibrium, using LeChatlier's Principle, predict which way the equilibrium conditions will shift (type in left, right, or no change) if silver chloride was added to a beaker. AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)

Respuesta :

Answer:Left

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For a beaker containing the reaction below that is at equilibrium, using LeChatlier's Principle, predict which way the equilibrium conditions will shift (type in left, right, or no change) if silver chloride was added to a beaker.
AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)