Certainly! Let's analyze the problem step-by-step.
We are given the equilibrium equation:
[tex]\[ N_2(g) + O_2(g) \rightleftharpoons 2 NO(g) \][/tex]
### Understanding Equilibrium
At equilibrium, the rate of the forward reaction (forming NO) is equal to the rate of the reverse reaction (forming [tex]\(N_2\)[/tex] and [tex]\(O_2\)[/tex]). According to Le Chatelier's principle, if a system at equilibrium is disturbed, the system will adjust itself to counteract that disturbance and restore a new equilibrium.
### Applying Le Chatelier's Principle
If additional [tex]\(N_2\)[/tex] is added to the system, the concentration of [tex]\(N_2\)[/tex] increases. Le Chatelier's principle tells us that the system will respond by shifting the equilibrium to the right to reduce the effect of the added [tex]\(N_2\)[/tex]. This shift to the right means that more [tex]\(NO\)[/tex] will be produced as [tex]\(N_2\)[/tex] and [tex]\(O_2\)[/tex] react.
### Analyzing the Options
Let’s evaluate each option:
A. More [tex]\(O_2\)[/tex] and [tex]\(NO\)[/tex] would form.
- This is incorrect because adding [tex]\(N_2\)[/tex] will not independently increase the concentration of [tex]\(O_2\)[/tex], but will instead drive the reaction to form [tex]\(NO\)[/tex].
B. More [tex]\(NO\)[/tex] would form.
- This is correct. Adding [tex]\(N_2\)[/tex] shifts the equilibrium to the right, resulting in the formation of more [tex]\(NO\)[/tex].
C. More [tex]\(N_2\)[/tex] and [tex]\(O_2\)[/tex] would form.
- This is incorrect because adding [tex]\(N_2\)[/tex] will not shift the reaction to the left to form more [tex]\(N_2\)[/tex] and [tex]\(O_2\)[/tex]. Instead, it shifts to the right, forming more [tex]\(NO\)[/tex].
D. [tex]\(K_{\text{eq}}\)[/tex] would decrease.
- This is incorrect. [tex]\(K_{\text{eq}}\)[/tex], the equilibrium constant, is dependent only on temperature and is not affected by changes in the concentrations of reactants or products.
### Conclusion
Based on the equilibrium principles and the shift in the reaction due to the addition of [tex]\(N_2\)[/tex], the correct answer is:
B. More [tex]\(NO\)[/tex] would form.
