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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 dissociation stops
- c)the reaction stops completely
- d)None of these
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
When H and I are mixed and equilibrium is attained, thena)amount of HI...
Explanation:
Equilibrium is a state where the rate of the forward reaction is equal to the rate of the backward reaction. In this state, the concentrations of the reactants and products remain constant.
When H and I are mixed, they may react to form HI. The reaction is as follows:
H2 + I2 ⇌ 2HI
a) Amount of HI formed is equal to the amount of H dissociated
At equilibrium, the amount of HI formed is not necessarily equal to the amount of H dissociated. The equilibrium constant (Kc) for this reaction is given by:
Kc = [HI]^2 / [H2][I2]
This means that the equilibrium position is determined by the ratio of the concentrations of the reactants and products. It is possible for the concentration of HI to be greater or less than the concentration of H or I.
b) HI dissociation stops
HI dissociation can occur in either direction of the reaction. At equilibrium, the rate of HI dissociation is equal to the rate of HI formation. This means that there is no net production or consumption of HI. However, HI dissociation does not stop completely, as it can still occur in either direction.
c) The reaction stops completely
The reaction does not stop completely at equilibrium. The forward and backward reactions are still occurring, but the rates are equal.
d) None of these
Option D is the correct answer because none of the statements are completely true. The reaction is still occurring, but the amounts of reactants and products have reached a state of equilibrium. The concentrations of H, I, and HI are constant, but not necessarily equal. HI dissociation can still occur, but the net production or consumption of HI is zero.
Equilibrium is a state where the rate of the forward reaction is equal to the rate of the backward reaction. In this state, the concentrations of the reactants and products remain constant.
When H and I are mixed, they may react to form HI. The reaction is as follows:
H2 + I2 ⇌ 2HI
a) Amount of HI formed is equal to the amount of H dissociated
At equilibrium, the amount of HI formed is not necessarily equal to the amount of H dissociated. The equilibrium constant (Kc) for this reaction is given by:
Kc = [HI]^2 / [H2][I2]
This means that the equilibrium position is determined by the ratio of the concentrations of the reactants and products. It is possible for the concentration of HI to be greater or less than the concentration of H or I.
b) HI dissociation stops
HI dissociation can occur in either direction of the reaction. At equilibrium, the rate of HI dissociation is equal to the rate of HI formation. This means that there is no net production or consumption of HI. However, HI dissociation does not stop completely, as it can still occur in either direction.
c) The reaction stops completely
The reaction does not stop completely at equilibrium. The forward and backward reactions are still occurring, but the rates are equal.
d) None of these
Option D is the correct answer because none of the statements are completely true. The reaction is still occurring, but the amounts of reactants and products have reached a state of equilibrium. The concentrations of H, I, and HI are constant, but not necessarily equal. HI dissociation can still occur, but the net production or consumption of HI is zero.
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When H and I are mixed and equilibrium is attained, thena)amount of HI formed is equal to the amount of H dissociatedb)HI dissociation stopsc)the reaction stops completelyd)None of theseCorrect answer is option 'D'. Can you explain this answer?
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