The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A] = [A]oe-kt Now say we are particularly interested in the time it would take for the concentration to become one- half of its initial value. Then we could substitute [Alo for [A] and rearrange the equation to: t1/2 = 0.693 k This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life. Half-life equation for first-order reactions: t1/2 = 0.693 k where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹). Part A To calculate the half-life, plug the value for k into the half-life equation and solve. What is the half-life of a first-order reaction with a rate constant of 1.40x104 s-¹? Express your answer with the appropriate units. Value Submit A Units Review | Constants | Periodic Table Request Answer 21 ?
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A] = [A]oe-kt Now say we are particularly interested in the time it would take for the concentration to become one- half of its initial value. Then we could substitute [Alo for [A] and rearrange the equation to: t1/2 = 0.693 k This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life. Half-life equation for first-order reactions: t1/2 = 0.693 k where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹). Part A To calculate the half-life, plug the value for k into the half-life equation and solve. What is the half-life of a first-order reaction with a rate constant of 1.40x104 s-¹? Express your answer with the appropriate units. Value Submit A Units Review | Constants | Periodic Table Request Answer 21 ?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.23QE: Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure...
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![The integrated rate law allows chemists to predict
the reactant concentration after a certain amount of
time, or the time it would take for a certain
concentration to be reached.
The integrated rate law for a first-order reaction is:
[A] = [A]oe-kt
Now say we are particularly interested in the time it
would take for the concentration to become one-
half of its initial value. Then we could substitute
[A]o
for [A] and rearrange the equation to:
2
0.693
k
t1/2
This equation calculates the time required for the
reactant concentration to drop to half its initial
value. In other words, it calculates the half-life.
Half-life equation for first-order reactions:
0.693
k
where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹).
Part A
Value
To calculate the half-life, plug the value for k into the half-life equation and solve.
What is the half-life of a first-order reaction with a rate constant of 1.40x10-4 s-¹?
Express your answer with the appropriate units.
S
Submit
Units
Request Answer
t₁/2 =
www.
Review | Constants | Periodic Table
11 ?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F090d0c20-1704-4ae8-b5d0-3a8eb14a815e%2F2f5c8b86-7105-4dbc-b06c-275cad04db9b%2Fx9hr0m_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The integrated rate law allows chemists to predict
the reactant concentration after a certain amount of
time, or the time it would take for a certain
concentration to be reached.
The integrated rate law for a first-order reaction is:
[A] = [A]oe-kt
Now say we are particularly interested in the time it
would take for the concentration to become one-
half of its initial value. Then we could substitute
[A]o
for [A] and rearrange the equation to:
2
0.693
k
t1/2
This equation calculates the time required for the
reactant concentration to drop to half its initial
value. In other words, it calculates the half-life.
Half-life equation for first-order reactions:
0.693
k
where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹).
Part A
Value
To calculate the half-life, plug the value for k into the half-life equation and solve.
What is the half-life of a first-order reaction with a rate constant of 1.40x10-4 s-¹?
Express your answer with the appropriate units.
S
Submit
Units
Request Answer
t₁/2 =
www.
Review | Constants | Periodic Table
11 ?
Transcribed Image Text:b) What is the rate constant of a first-order reaction that
takes 248 secondsseconds for the reactant concentration
to drop to half of its initial value?
c) A certain first-order reaction has a rate constant of
6.70x10-³ s-1s-1. How long will it take for the reactant
concentration to drop to 1818 of its initial value?
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