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For an autocatalytic second order reaction R → P, the rate law is [where v is rate of the reaction and k is the rate constant]
- a)v = k[R]
- b)v = k[R][P]
- c)v = k[R]2
- d)v = k[P]2
Correct answer is option 'B'. Can you explain this answer?
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For an autocatalytic second order reaction R →P, the rate law is...
The correct answer for the given rate law of an autocatalytic second-order reaction R → P is option 'B': v = k[R][P]. Let's understand why this is the correct answer.
1. Introduction to autocatalytic reactions:
- Autocatalytic reactions are those in which one of the reactants acts as a catalyst for the reaction.
- In this case, the product P is formed by the reaction of reactant R, and the reactant R itself acts as a catalyst for the reaction.
2. Rate law for autocatalytic reactions:
- The rate law describes how the rate of a reaction depends on the concentrations of the reactants.
- For an autocatalytic reaction, the rate of the reaction is directly proportional to the concentrations of both the reactant and the catalyst.
- Since the reaction is second order, the rate law will involve the concentrations of both reactant R and product P.
3. Deriving the rate law for the given reaction:
- Let's assume the rate constant for the reaction is denoted by k.
- The rate of the reaction (v) can be expressed as the change in concentration of product P with time.
- Since the reaction is autocatalytic, the rate of the reaction is also proportional to the concentration of reactant R.
- Therefore, the rate law for this reaction can be expressed as v = k[R][P], where [R] represents the concentration of reactant R and [P] represents the concentration of product P.
4. Option analysis:
- Option 'A' (v = k[R]): This option considers only the concentration of reactant R and not product P, which is incorrect for a second-order reaction.
- Option 'B' (v = k[R][P]): This option includes the concentrations of both reactant R and product P, which is correct for an autocatalytic second-order reaction.
- Option 'C' (v = k[R]^2): This option considers the square of the concentration of reactant R, which is incorrect for a second-order reaction.
- Option 'D' (v = k[P]^2): This option considers the square of the concentration of product P, which is incorrect for a second-order reaction.
Therefore, the correct answer is option 'B' (v = k[R][P]), as it accurately represents the rate law for an autocatalytic second-order reaction.
1. Introduction to autocatalytic reactions:
- Autocatalytic reactions are those in which one of the reactants acts as a catalyst for the reaction.
- In this case, the product P is formed by the reaction of reactant R, and the reactant R itself acts as a catalyst for the reaction.
2. Rate law for autocatalytic reactions:
- The rate law describes how the rate of a reaction depends on the concentrations of the reactants.
- For an autocatalytic reaction, the rate of the reaction is directly proportional to the concentrations of both the reactant and the catalyst.
- Since the reaction is second order, the rate law will involve the concentrations of both reactant R and product P.
3. Deriving the rate law for the given reaction:
- Let's assume the rate constant for the reaction is denoted by k.
- The rate of the reaction (v) can be expressed as the change in concentration of product P with time.
- Since the reaction is autocatalytic, the rate of the reaction is also proportional to the concentration of reactant R.
- Therefore, the rate law for this reaction can be expressed as v = k[R][P], where [R] represents the concentration of reactant R and [P] represents the concentration of product P.
4. Option analysis:
- Option 'A' (v = k[R]): This option considers only the concentration of reactant R and not product P, which is incorrect for a second-order reaction.
- Option 'B' (v = k[R][P]): This option includes the concentrations of both reactant R and product P, which is correct for an autocatalytic second-order reaction.
- Option 'C' (v = k[R]^2): This option considers the square of the concentration of reactant R, which is incorrect for a second-order reaction.
- Option 'D' (v = k[P]^2): This option considers the square of the concentration of product P, which is incorrect for a second-order reaction.
Therefore, the correct answer is option 'B' (v = k[R][P]), as it accurately represents the rate law for an autocatalytic second-order reaction.
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For an autocatalytic second order reaction R →P, the rate law is...
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For an autocatalytic second order reaction R →P, the rate law is [where v is rate of the reaction and k is the rate constant]a)v = k[R]b)v = k[R][P]c)v = k[R]2d)v = k[P]2Correct answer is option 'B'. Can you explain this answer?
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