Integrated Rate Equations
Chemistry ⇒ Chemical Kinetics and Equilibrium
Integrated Rate Equations starts at 11 and continues till grade 12.
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A reaction is found to have a constant rate regardless of the concentration of reactant. What is the order of the reaction?
Describe how you would determine the order of a reaction using integrated rate equations and experimental data.
Explain why the half-life of a second-order reaction depends on the initial concentration.
Explain why the integrated rate law for a first-order reaction is useful in radioactive decay studies.
A first-order reaction has a rate constant of 2.31 × 10-2 s-1. How long will it take for the concentration to drop to one-fourth of its initial value?
A reaction follows the rate law: rate = k[A]2. If the initial concentration of A is 0.5 mol/L and after 20 seconds it is 0.25 mol/L, calculate the rate constant k.
A reaction has a rate constant of 0.05 min-1. How long will it take for the concentration to fall to 1/8th of its original value in a first-order reaction?
A reaction has the rate law: rate = k[A]. If [A]0 = 0.6 mol/L and after 10 min [A] = 0.3 mol/L, what is the value of k?
Which of the following graphs is linear for a first-order reaction?
(1) [A] vs t
(2) ln[A] vs t
(3) 1/[A] vs t
(4) [A] vs 1/t
Which of the following is NOT a correct integrated rate law?
(1) [A] = [A]0 - kt (zero-order)
(2) ln[A] = ln[A]0 - kt (first-order)
(3) 1/[A] = 1/[A]0 + kt (second-order)
(4) [A] = [A]0ekt (first-order)
Which of the following is the correct expression for the half-life of a first-order reaction?
(1) t1/2 = 0.693/k
(2) t1/2 = 1/(k[A]0)
(3) t1/2 = [A]0/(2k)
(4) t1/2 = 2k/[A]0
Which of the following is the integrated rate equation for a first-order reaction?
(1) [A] = [A]0 - kt
(2) ln[A] = ln[A]0 - kt
(3) 1/[A] = 1/[A]0 + kt
(4) [A] = [A]0ekt
For a first-order reaction, the time required for the concentration to decrease from [A]0 to [A] is given by t = ______.
For a first-order reaction, the time taken for the concentration to decrease from [A]0 to [A]0/n is ______.
For a second-order reaction, the half-life is ______ proportional to the initial concentration.
For a zero-order reaction, the plot of ______ versus time is a straight line.
For a zero-order reaction, the half-life is directly proportional to the initial concentration. True or False?
The half-life of a first-order reaction is independent of the initial concentration. True or False?
The integrated rate equation for a zero-order reaction is [A] = [A]0 - kt. Yes or No?
The integrated rate law for a first-order reaction can be used to determine the rate constant from experimental data. Yes or No?
