\( 2HI(g) \rightleftharpoons H_{2}(g) + I_{2}(g) \). The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of \( H_{2} \) and \( I_{2} \) are added to the system, the equilibrium constant will be
Show Hint
- 6.4
- 0.8
- 3.2
- 1.6
The Correct Option is A
Solution and Explanation
The equilibrium constant ($K$) is a characteristic constant for a given reaction.
Step 2: Dependency
$K$ depends only on the temperature for a specific chemical equation.
Step 3: Conclusion
Adding more reactants or products changes the equilibrium position but does not change the value of the equilibrium constant itself. It remains 6.4.
Final Answer: (a)
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