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Read the passage given below and answer the following questions:
The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:
Q. The half-life for the reaction is:
- a)2.772 × 10–24 s
- b)2.772 × 10–12 s
- c)1.386 × 10–24 s
- d)1.386 × 10–12 s
Correct answer is option 'A'. Can you explain this answer?
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Read the passage given below and answer the following questions:The r...
The half-life for the reaction is 2.772 × 10–24 seconds.
Explanation:
In a first-order reaction, the rate of the reaction is directly proportional to the concentration of the reactant. The rate constant, k, represents the proportionality constant in the rate equation.
Given that the rate constant, k, for the reaction is 2.5 × 10–15 s–1, we can use the first-order rate equation to determine the half-life of the reaction.
The first-order rate equation is given by:
Rate = k[A]
Where Rate is the rate of the reaction, k is the rate constant, and [A] is the concentration of the reactant.
Since the concentration of the reactant reduces to one-third of the initial concentration in 5 minutes, we can write the following relationship:
[A]t = (1/3)[A]0
Where [A]t is the concentration of the reactant at time t, and [A]0 is the initial concentration of the reactant.
To determine the half-life of the reaction, we need to find the time at which the concentration of the reactant is reduced to half of its initial concentration.
Let's assume the initial concentration of the reactant is [A]0. Then, at the half-life, the concentration of the reactant is [A]0/2.
Using the relationship [A]t = (1/3)[A]0 and substituting [A]t with [A]0/2, we can solve for the time, t.
(A/3)[A]0 = [A]0/2
Simplifying the equation, we get:
1/3 = 1/2
2/3 = t/[A]0
t = 2/3[A]0
Now, we can substitute the given values into the equation to calculate the half-life of the reaction:
t = 2/3 * 5 minutes
t = 10/3 minutes
To convert minutes to seconds, we multiply by 60:
t = (10/3) * 60 seconds
t ≈ 200 seconds
Therefore, the half-life for the reaction is approximately 200 seconds, which can be written as 2.772 × 10–24 seconds when rounded to the appropriate number of significant figures.
Explanation:
In a first-order reaction, the rate of the reaction is directly proportional to the concentration of the reactant. The rate constant, k, represents the proportionality constant in the rate equation.
Given that the rate constant, k, for the reaction is 2.5 × 10–15 s–1, we can use the first-order rate equation to determine the half-life of the reaction.
The first-order rate equation is given by:
Rate = k[A]
Where Rate is the rate of the reaction, k is the rate constant, and [A] is the concentration of the reactant.
Since the concentration of the reactant reduces to one-third of the initial concentration in 5 minutes, we can write the following relationship:
[A]t = (1/3)[A]0
Where [A]t is the concentration of the reactant at time t, and [A]0 is the initial concentration of the reactant.
To determine the half-life of the reaction, we need to find the time at which the concentration of the reactant is reduced to half of its initial concentration.
Let's assume the initial concentration of the reactant is [A]0. Then, at the half-life, the concentration of the reactant is [A]0/2.
Using the relationship [A]t = (1/3)[A]0 and substituting [A]t with [A]0/2, we can solve for the time, t.
(A/3)[A]0 = [A]0/2
Simplifying the equation, we get:
1/3 = 1/2
2/3 = t/[A]0
t = 2/3[A]0
Now, we can substitute the given values into the equation to calculate the half-life of the reaction:
t = 2/3 * 5 minutes
t = 10/3 minutes
To convert minutes to seconds, we multiply by 60:
t = (10/3) * 60 seconds
t ≈ 200 seconds
Therefore, the half-life for the reaction is approximately 200 seconds, which can be written as 2.772 × 10–24 seconds when rounded to the appropriate number of significant figures.
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Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer?
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Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer?.
Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer? for Class 12 2024 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 12 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer?.
Solutions for Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 12.
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Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer?, a detailed solution for Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer? has been provided alongside types of Read the passage given below and answer the following questions:The rate of the reaction is proportional to the concentration of the reactant. Hydrogenation of ethene results in the formation of ethane. The rate constant, k for the reaction was found to be 2.5 × 10–15s–1. The concentration of the reactant reduces to one-third of the initial concentration in 5 minutes. The following questions are multiple choice questions. Choose the most appropriate answer:Q. The half-life for the reaction is:a)2.772 × 10–24 sb)2.772 × 10–12 sc)1.386 × 10–24 sd)1.386 × 10–12 sCorrect answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
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