What would happen if [tex]$N _2$[/tex] were added to [tex]$N _2(g)+ O _2(g)=2 NO (g)$[/tex] at equilibrium?
A. More [tex]$O _2$[/tex] and NO would form.
B. [tex]$K$[/tex]eq would decrease.
C. More [tex]$N _2$[/tex] and [tex]$O _2$[/tex] would form.
D. More NO would form.
Answer (2)
Adding N 2 to the equilibrium N 2 ( g ) + O 2 ( g ) i g h t ha r p oo n u p 2 NO ( g ) creates a stress on the system.
According to Le Chatelier's principle, the equilibrium shifts to relieve this stress.
The equilibrium shifts to the right, consuming N 2 and O 2 to produce more NO .
Therefore, more NO forms. D
Explanation
Understanding the Problem and Applying Le Chatelier's Principle The problem describes a chemical reaction at equilibrium: N 2 ( g ) + O 2 ( g ) i g h t ha r p oo n u p 2 NO ( g ) . We are asked to determine what happens when more N 2 is added to the system. To solve this, we'll use Le Chatelier's principle.
Le Chatelier's Principle Le Chatelier's principle states that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress. In this case, the stress is the addition of N 2 .
Shifting the Equilibrium To relieve the stress of added N 2 , the equilibrium will shift to the right, favoring the forward reaction. This means more N 2 will react with O 2 to produce more NO .
Conclusion Therefore, adding N 2 will result in more NO being formed.
Examples
Le Chatelier's principle is widely used in industrial chemistry to optimize reaction conditions. For example, in the Haber-Bosch process for ammonia synthesis ( N 2 + 3 H 2 i g h t ha r p oo n u p 2 N H 3 ), increasing the pressure shifts the equilibrium towards ammonia production, as the forward reaction reduces the number of gas molecules. Similarly, controlling temperature and reactant concentrations allows for maximizing the yield of desired products in various chemical processes, making the production more efficient and cost-effective. This principle helps chemical engineers to design and operate chemical reactors to achieve the highest possible conversion and yield.
Adding N2 to the equilibrium reaction increases its concentration, leading the system to shift right according to Le Chatelier's principle. This shift results in the production of more NO. Therefore, the correct answer is option D.
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