Advertisements
Advertisements
प्रश्न
Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is ______.
पर्याय
first
second
third
zero
Advertisements
उत्तर
Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is first.
APPEARS IN
संबंधित प्रश्न
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.
Answer the following in brief.
What is a zeroth-order reaction?
In a first-order reaction, the concentration of the reactant decreases from 20 mmol dm−3 to 8 mmol dm−3 in 38 minutes. What is the half-life of reaction?
Solve
A first-order reaction takes 40 minutes for 30% decomposition. Calculate its half-life.
For a first-order reaction, the rate constant is 6.909 min−1 the time taken for 75% conversion in minutes is
Assertion: rate of reaction doubles when the concentration of the reactant is doubles if it is a first-order reaction.
Reason: rate constant also doubles.
The time for half change in a first order decomposition of a substance A is 60 seconds. Calculate the rate constant. How much of A will be left after 180 seconds?
A reaction that is of the first order with respect to reactant A has a rate constant 6 min−1. If we start with [A]0 = 0.5 mol dm−3, when would [A] reach the value 0.05 mol dm−3?
If [A] is the concentration of A at any time t and [A]0 is the concentration at t = 0, then for the 1st order reaction, the rate equation can be written as ____________.
A first order reaction completes its 10% in 20 minutes, then the time required to complete its 19% is ____________.
If [A]0 is the initial concentration, then the half life of zero order reaction 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 ____________.
Reaction given below follows first order kinetics:
\[\ce{2N2O2 -> 4NO2 + O2}\]
Calculate the rate constant of reaction if concentration of N2O2 is 0.05 M and rate of reaction is 1.5 × 10−6 mol L−1 s−1?
The slope of a graph, log [A]t versus 't' for a first order reaction is −2.5 × 10−3 s−1. The rate constant for the reaction is ____________.
The initial concentration of reactant (A) is 2 mol dm−3 for a zero order reaction \[\ce{A -> B}\]. The rate constant (k) is related to its half-life `("t"_(1//2))` by the equation:
For a first order reaction, \[\ce{A -> B}\], if [A] = 1 M and rate is 4 × 10−2 M s−1. What is the rate constant of the reaction?
A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction?
0.0210 M solution of N2O5 is allowed to decompose at 43°C. How long will it take to reduce to 0.0150 M?
(Given k = 6.0 × 10−4 sec−1)
The integrated rate equation is Rt = log C0 – log Ct, then the straight-line graph is obtained by plotting.
The integrated rate law is a direct relationship between time and ______
Define the half-life of a first-order reaction.
The rate constant and half-life of a first order reaction are related to each other as ______.
Which of the following is correct for a first-order reaction?
Half-life of a first order reaction is 30 minutes and initial concentration of reactant is 0.1 M.
What is half-life of the reaction if initial concentration of reactant is doubled?
Consider the following reaction.
\[\ce{SO2(g) + 1/2 O2(g) <=>[K1] SO3(g)}\]
\[\ce{2SO3(g)<=>[K2] 2SO2(g) + O2(g)}\]
What is the relation between K1 and K2?
What is the rate constant of a first order reaction if 0.08 mole of reactant reduces to 0.02 mole in 23.03 minutes?
What are integrated rate laws?
Calculate the time required to decrease the concentration of reactant of first order reaction from 0.8 M to 0.1 M if rate constant is 0.1155 hour−1.
Which of the following equations exhibits the integrated rate law equation for first order reaction?
