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Addition of inert gas to system N(2)(g...

Addition of inert gas to system
`N_(2)(g) + 3H_(2)(g) at equillibrium at constant volume. Then

A

`N_2 and H_2` are formed in abundance

B

`N_2, H_2 and NH_3` will have the same molar concentration

C

The production of ammonia increases

D

No change in the equilibrium

Text Solution

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The correct Answer is:
To solve the problem regarding the effect of adding an inert gas to the equilibrium system at constant volume, we can follow these steps: ### Step 1: Understand the Reaction The given equilibrium reaction is: \[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \] ### Step 2: Recognize the Conditions We are told that the volume of the system is constant. This is crucial because it affects how the concentrations of the reactants and products behave when an inert gas is added. ### Step 3: Effect of Adding Inert Gas at Constant Volume When an inert gas is added to a system at constant volume, the total pressure of the system increases. However, since the volume is constant, the number of moles of the reactants and products does not change, and thus their concentrations remain unchanged. ### Step 4: Analyze Concentrations Since the concentrations of \( N_2 \), \( H_2 \), and \( NH_3 \) do not change, we can conclude that: - The molar concentrations of \( N_2 \), \( H_2 \), and \( NH_3 \) remain the same. ### Step 5: Evaluate the Options Given the options: 1. \( N_2 \) and \( H_2 \) are formed in abundance. (Incorrect) 2. \( N_2 \), \( H_2 \), and ammonia will have the same molar concentration. (Correct) 3. The equilibrium will shift to the right. (Incorrect) 4. The equilibrium will shift to the left. (Incorrect) The correct conclusion is that the concentrations of all species remain unchanged. ### Final Conclusion The addition of an inert gas at constant volume does not affect the equilibrium concentrations of the reactants and products in the given reaction. ---
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