Advertisements
Advertisements
Question
Answer the following in one or two sentences.
How do the half-lives of the first order and zero-order reactions change with the initial concentration of reactants?
Advertisements
Solution
i. The half-life of the first-order reaction is independent of the initial concentration of the reactant.
ii. The half-life of zero-order reactions is proportional to the initial concentration of the reactant.
APPEARS IN
RELATED QUESTIONS
Answer the following in brief.
Obtain the relationship between the rate constant and half-life of a first-order reaction.
Answer the following in brief.
Derive the integrated rate law for the first-order reaction.
Solve
The half-life of a first-order reaction is 1.7 hours. How long will it take for 20% of the reactant to react?
Answer the following in brief.
Give one example and explain why it is pseudo-first-order.
Write order of the following reaction:
\[\ce{2NH_{3(g)} -> N_{2(g)} + 3H_{2(g)}}\]
The rate constant of the first order reaction is 1.386 min–1. Calculate the time required for 80% reactant to decompose?
For a first-order reaction \[\ce{A -> B}\] the rate constant is x min−1. If the initial concentration of A is 0.01 M, the concentration of A after one hour is given by the expression.
A zero-order reaction \[\ce{X -> Product}\], with an initial concentration 0.02 M has a half-life of 10 min. if one starts with concentration 0.04 M, then the half-life is
This reaction follows first-order kinetics. The rate constant at particular temperature is 2.303 × 10−2 hour−1. The initial concentration of cyclopropane is 0.25 M. What will be the concentration of cyclopropane after 1806 minutes? (log 2 = 0.3010)
Describe the graphical representation of first order reaction.
A zero order reaction is 20% complete in 20 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?
The integrated rate law is a direct relationship between ____________ and ____________.
The rate constant of a reaction has same units as the rate of reaction. The reaction is of ____________.
In a first order reaction, the concentration of the reactant, decreases from 0.8 mol dm−3 to 0.4 mol dm−3 in 15 minutes. The time taken for the concentration to change from 0.1 mol dm−3 to 0.025 mol dm−3 is ____________.
In a first order reaction, the concentration of the reactant is reduced to 25% in one hour. The half-life period of the reaction is ____________.
A first order reaction is 75% completed in 60 minutes, the time required for it's 50% completion is ____________.
In a reaction \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\], if the rate of disappearance of N2(g) is 2.6 × 10−4 M/s, the rate of disappearance of H2(g) in M/s is ____________.
For the first order reaction A → B, the rate constant is 0.25 s-1, if the concentration of A is reduced to half, the value of rate constant will be ________.
Half-life of first order reaction is 20 minutes. What is the time taken to reduce the initial concentration of the reactant to `1/10`th?
Rate constant for zero order reaction is 2 × 10-2 mol L-1 s-1. If the concentration of the reactant after 25 sec. is 0.5 M, what is the initial concentration of reactant?
For zero order reaction, when [A]t is plotted against time (t), the slope of the straight line obtained is equal to ______.
The integrated rate law is a direct relationship between time and ______
Which one of the following reactions is a true first-order reaction?
Which of the following is correct for a first-order reaction?
Which is the relation between half life and rate constant for a zero order?
A first order reaction takes 10 minute for 30% completion. Find rate constant of the reaction.
Which of the following equations exhibits the integrated rate law equation for first order reaction?
