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When H2 and I2 are mixed and equilibrium is attained,then
- a)amount of HI formed is equal to the amount of H2 dissociated
- b)HI dissociated stops
- c)The reaction stops completely
- d)None of these
Correct answer is option 'D'. Can you explain this answer?
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When H2 and I2 are mixed and equilibrium is attained,thena)amount of H...
At equilibrium rate of forward reaction becomes equal to the rate of backward reaction
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When H2 and I2 are mixed and equilibrium is attained,thena)amount of H...
Explanation:
Equilibrium in the reaction:
- When H2 and I2 are mixed, they react to form HI according to the equation: H2 + I2 ⇌ 2HI.
- At equilibrium, the concentrations of reactants and products remain constant.
Amount of HI formed:
- The amount of HI formed at equilibrium depends on the initial concentrations of H2 and I2, as well as the equilibrium constant for the reaction.
- It is not necessarily equal to the amount of H2 dissociated, as the equilibrium position is determined by the relative concentrations of the reactants and products.
HI dissociated stops:
- Once equilibrium is reached, the forward and reverse reactions occur at equal rates, resulting in the concentrations of H2, I2, and HI remaining constant.
- However, some HI may still dissociate and reform due to the dynamic nature of equilibrium.
Reaction stops completely:
- The reaction does not stop completely at equilibrium; instead, it continues at a constant rate in both the forward and reverse directions.
- The concentrations of all species in the reaction remain constant, indicating a dynamic equilibrium state.
Therefore, the correct answer is option 'D' - None of these. At equilibrium, the reaction does not stop completely, and the amount of HI formed is not necessarily equal to the amount of H2 dissociated.
Equilibrium in the reaction:
- When H2 and I2 are mixed, they react to form HI according to the equation: H2 + I2 ⇌ 2HI.
- At equilibrium, the concentrations of reactants and products remain constant.
Amount of HI formed:
- The amount of HI formed at equilibrium depends on the initial concentrations of H2 and I2, as well as the equilibrium constant for the reaction.
- It is not necessarily equal to the amount of H2 dissociated, as the equilibrium position is determined by the relative concentrations of the reactants and products.
HI dissociated stops:
- Once equilibrium is reached, the forward and reverse reactions occur at equal rates, resulting in the concentrations of H2, I2, and HI remaining constant.
- However, some HI may still dissociate and reform due to the dynamic nature of equilibrium.
Reaction stops completely:
- The reaction does not stop completely at equilibrium; instead, it continues at a constant rate in both the forward and reverse directions.
- The concentrations of all species in the reaction remain constant, indicating a dynamic equilibrium state.
Therefore, the correct answer is option 'D' - None of these. At equilibrium, the reaction does not stop completely, and the amount of HI formed is not necessarily equal to the amount of H2 dissociated.
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When H2 and I2 are mixed and equilibrium is attained,thena)amount of HI formed is equal to the amount of H2 dissociatedb)HI dissociated stopsc)The reaction stops completelyd)None of theseCorrect answer is option 'D'. Can you explain this answer?
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