For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increasenh3(g)+h2o(l) ⇋ nh4+(aq)+oh−(aq)drag the appropriate stresses to their respective bins. adding nh4+(aq) adding nh3(g) adding oh-(aq) removing nh4+(aq) removing oh-(aq)shifts in the direction of the reactants: shift in the direction of the products:

Adding NH₄⁺ (aq) ⇒ Shift in the direction of the reactants.

Adding NH₃ (g)⇒ Shift in the direction of the product.

Adding OH⁻ (aq) ⇒ Shift in the direction of the reactants.

Removing NH₄⁺ (aq) ⇒ Shift in the direction of the product.

Removing OH⁻ (aq) ⇒ Shift in the direction of the product.

In the equilibrium system, according to Le Chatelier, if there is a reaction there will be action

If the concentration of one component is enlarged, the system reaction is to reduce the component, and vice versa, if the concentration of one component is reduced, the reaction system is to add to the component

From reaction:

NH₃ (g) + H₂O (l) ⇋ NH₄⁺ (aq) + OH⁻ (aq)

The system will react by decreasing the concentration of products by moving to the left ---> Shifts in the direction of the reactants

The system will react by decreasing the concentration of reagents by moving to the right > Shift in the direction of the product:

The system will react by decreasing the concentration of products by moving to the left -> Shifts in the direction of the reactants

The system will react by increasing the concentration of products by moving to the right > Shift in the direction of the product:

The system will react by increasing the concentration of products by moving to the right > Shift in the direction of the product:

Kc for reaction

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an equilibrium constant link

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Calculate the value of the equilibrium constant, Kc

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Concentration of HI at equilibrium

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c. 4.54 x 10–12 j happens to be correct