Advertisements
Advertisements
Question
For a first order reaction \[\ce{A ->Product}\] with initial concentration x mol L−1, has a half life period of 2.5 hours. For the same reaction with initial concentration `("x"/2)` mol L−1 the half life is
Options
(2.5 × 2) hours
`(2.5/2)` hours
2.5 hours
Without knowing the rate constant, t1/2 cannot be determined from the given data
Advertisements
Solution
2.5 hours
APPEARS IN
RELATED QUESTIONS
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?
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 first order reaction has a rate constant 0.00813 min-1. How long will it take for 60% completion?
The rate of the reaction \[\ce{A + B -> C}\] is 3.6 × 10−2 mol dm−3 s−1 when [A] = 0.3 mol dm−3 and [B] = 0.2 mol dm−3. Calculate k if reaction is first order in A and zero order in B.
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?
The rate constant of a reaction has same units as the rate of reaction. The reaction is of ____________.
The rate constant of a first order reaction is 3 × 10−6 per s. If the initial concentration is 0.10 mol dm−3, the initial rate of reaction is ____________.
If time required to decrease concentration of reactant from 0.8 M to 0.2 M is 12 hours, the half life of this first order reaction is ____________.
Half-life period of a first order reaction, \[\ce{A -> product}\] is 3.0 hours. What is the value of rate constant?
For a first order reaction, the plot of log k against 1/T is a straight line. The slope of the line is equal to ______.
