Q17.99CP - Chemistry: Molecular Nature Of Matter And Change

Question

When ammonia is made industrially, the mixture of ${\mathbf{\text{N}}}_{\mathbf{2}}\mathbf{,}{\mathbf{\text{H}}}_{\mathbf{2}}$ , and data-custom-editor="chemistry" ${\mathbf{\text{NH}}}_{\mathbf{3}}$ that emerges from the reaction chamber is far from equilibrium. Why does the plant supervisor use reaction conditions that produce less than the maximum yield of ammonia?

Step-by-Step Solution

Answer

Because ammonia develops slowly at low temperatures, the process is inefficient.

Step 1: Definition of equilibrium

Chemical equilibrium is the state in which no net change in the amounts of reactants and products occurs during a reversible chemical reaction.

Step 2: Why does the plant supervisor use reaction conditions

The reaction is,

${\text{N}}_2+3{\text{H}}_2=2{\text{NH}}_3$ .

If the temperature will increase, the position of the equilibrium will change to decrease the temperature. In the  endothermic  direction, the equilibrium will move. If the equilibrium shifts then the yield will decrease. But at low temperatures, the rate of the reaction is very low. Ammonia forms slowly at low temperatures, this results to the process being uneconomical.