Question

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 increase

NH3(g)+H2O(l) ⇋ NH4+(aq)+OH−(aq)

Drag the appropriate stresses to their respective bins.

Adding NH₄⁺(aq)     Adding NH_3(g)    Adding OH^-_(aq)      Removing NH₄⁺_(aq)      Removing OH^-_(aq)

Shifts in the direction of the reactants:

Shift in the direction of the products:

Answer 1

First, let us state the Le Chatelier principle which deals with changes in an equilibrium:

The statement is as follows:

If any equilibrium is disturbed, that is, change in conditions such as P,T, concentration, partial pressure, etc.., the system will counterbalance such change in order to favour the system's equilbirium.

• Change in concentration
• Change in pressure
• Change in temperature

For:

NH3(g)+H2O(l) ⇋ NH4+(aq)+OH−(aq)

Adding NH4+(aq) --> increases product, therefore, the reaciton shift to the LEFT

Adding NH3(g) --> increase in reactants, shift goes to the RIGTH

Adding OH-(aq) --> increases product, therefore, the reaciton shift to the LEFT

Removing NH4+(aq) --> decrease in products, therefore, the reactants must form more products to counterbalnce

Removing OH-(aq) -- >decrease in products, therefore, the reactants must form more products to counterbalnce