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An equilibrium mixture at 700 K of 0.05M...

An equilibrium mixture at 700 K of 0.05M `N_(2)(g) and 0.2 M NH_(3)(g)` is present in a container .Now if this equilibrium is disturbed by adding `N_(@)` (g) so that its concentration becomes 0.15M just after addition then which of the following graph represents the above situation more appropriately:

A

B

C

D

Text Solution

AI Generated Solution

The correct Answer is:
To solve the problem, we need to analyze the equilibrium reaction and the changes that occur when we add \( N_2(g) \) to the system. ### Step-by-Step Solution: 1. **Identify the Initial Conditions**: - The initial concentrations before adding \( N_2(g) \) are: - \( [N_2] = 0.05 \, M \) - \( [NH_3] = 0.2 \, M \) 2. **Disturb the Equilibrium**: - After adding \( N_2(g) \), the concentration becomes \( [N_2] = 0.15 \, M \). 3. **Determine the Change in Concentration**: - The change in concentration of \( N_2 \) is: \[ \Delta [N_2] = 0.15 \, M - 0.05 \, M = 0.10 \, M \] 4. **Apply Le Chatelier's Principle**: - According to Le Chatelier's principle, if we increase the concentration of a reactant, the system will shift to the right to counteract the change, thereby producing more products. 5. **Stoichiometry of the Reaction**: - The balanced reaction for the formation of ammonia from nitrogen and hydrogen is: \[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \] - From the stoichiometry of the reaction: - For every 1 mole of \( N_2 \) that reacts, 3 moles of \( H_2 \) are consumed and 2 moles of \( NH_3 \) are produced. 6. **Calculate Changes in Concentration**: - Since \( N_2 \) increases by \( 0.10 \, M \): - The decrease in \( H_2 \) will be \( 3 \times 0.10 \, M = 0.30 \, M \). - The increase in \( NH_3 \) will be \( 2 \times 0.10 \, M = 0.20 \, M \). 7. **Final Concentrations**: - After the changes, the new concentrations will be: - \( [N_2] = 0.15 \, M \) - \( [H_2] = 0.2 \, M - 0.30 \, M = -0.10 \, M \) (impossible, indicating that the reaction will not proceed further) - \( [NH_3] = 0.2 \, M + 0.20 \, M = 0.4 \, M \) 8. **Graph Representation**: - The graph that represents this situation will show a decrease in \( H_2 \) concentration, an increase in \( NH_3 \) concentration, and a slight change in \( N_2 \) concentration. ### Conclusion: The correct graph that represents the changes in concentrations of \( N_2 \), \( H_2 \), and \( NH_3 \) after the addition of \( N_2(g) \) is option D, as it matches the stoichiometric changes predicted by the equilibrium shift.
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