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At a certain temperature, only 50% HI is dissociated at equilibrium in the following reaction: 2HI(g) ⇌ H2(g) + I2(g). The equilibrium constant for this reaction is:
- a)0.25
- b)1.0
- c)3.0
- d)0.5
Correct answer is option 'A'. Can you explain this answer?
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2HI(g) ⇌ H2(g) + I2(g)
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At a certain temperature, only 50% HI is dissociated at equilibrium i...
Equilibrium Constant (Kc)
The equilibrium constant (Kc) is a measure of the extent to which a reaction proceeds to form products at equilibrium. It is determined by the concentrations of the reactants and products at equilibrium.
Equilibrium Expression
For a reaction of the form:
aA + bB ⇌ cC + dD
The equilibrium expression is written as:
Kc = [C]^c [D]^d / [A]^a [B]^b
Where [A], [B], [C], and [D] represent the molar concentrations of A, B, C, and D at equilibrium, respectively.
Equilibrium Constant for the Given Reaction
The given reaction is:
2HI(g) ⇌ H2(g) + I2(g)
The equilibrium constant expression for this reaction is:
Kc = [H2][I2] / [HI]^2
Given Information
At a certain temperature, only 50% of HI is dissociated at equilibrium. This means that the concentration of HI at equilibrium is half of its initial concentration.
Using the Given Information
Let's assume the initial concentration of HI is x. At equilibrium, the concentration of HI will be x/2.
Since the equilibrium constant (Kc) is a ratio of the concentrations at equilibrium, we can substitute the concentrations into the equilibrium constant expression:
Kc = [H2][I2] / [HI]^2
= [H2][I2] / (x/2)^2
= [H2][I2] / (x^2/4)
= 4[H2][I2] / x^2
Using the Given Information (contd.)
We know that only 50% of HI is dissociated at equilibrium. This means that the concentration of H2 and I2 at equilibrium is half of the concentration of HI at equilibrium. So, [H2] = [I2] = (x/2).
Substituting these values into the equilibrium constant expression:
Kc = 4[H2][I2] / x^2
= 4(x/2)(x/2) / x^2
= 4x^2/4x^2
= 1
Conclusion
Therefore, the equilibrium constant (Kc) for the given reaction is 1.0.
The equilibrium constant (Kc) is a measure of the extent to which a reaction proceeds to form products at equilibrium. It is determined by the concentrations of the reactants and products at equilibrium.
Equilibrium Expression
For a reaction of the form:
aA + bB ⇌ cC + dD
The equilibrium expression is written as:
Kc = [C]^c [D]^d / [A]^a [B]^b
Where [A], [B], [C], and [D] represent the molar concentrations of A, B, C, and D at equilibrium, respectively.
Equilibrium Constant for the Given Reaction
The given reaction is:
2HI(g) ⇌ H2(g) + I2(g)
The equilibrium constant expression for this reaction is:
Kc = [H2][I2] / [HI]^2
Given Information
At a certain temperature, only 50% of HI is dissociated at equilibrium. This means that the concentration of HI at equilibrium is half of its initial concentration.
Using the Given Information
Let's assume the initial concentration of HI is x. At equilibrium, the concentration of HI will be x/2.
Since the equilibrium constant (Kc) is a ratio of the concentrations at equilibrium, we can substitute the concentrations into the equilibrium constant expression:
Kc = [H2][I2] / [HI]^2
= [H2][I2] / (x/2)^2
= [H2][I2] / (x^2/4)
= 4[H2][I2] / x^2
Using the Given Information (contd.)
We know that only 50% of HI is dissociated at equilibrium. This means that the concentration of H2 and I2 at equilibrium is half of the concentration of HI at equilibrium. So, [H2] = [I2] = (x/2).
Substituting these values into the equilibrium constant expression:
Kc = 4[H2][I2] / x^2
= 4(x/2)(x/2) / x^2
= 4x^2/4x^2
= 1
Conclusion
Therefore, the equilibrium constant (Kc) for the given reaction is 1.0.
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At a certain temperature, only 50% HI is dissociated at equilibrium in the following reaction: 2HI(g) ⇌ H2(g) + I2(g). The equilibrium constant for this reaction is:a)0.25b)1.0c)3.0d)0.5Correct answer is option 'A'. Can you explain this answer?
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