Advertisements
Advertisements
प्रश्न
For first order reaction, the rate constant for the decomposition of N2O5 is 6 × 10–4 s –1. The half-life period for decomposition in seconds is ______.
पर्याय
11.55
115.5
1155
1.155
Advertisements
उत्तर
For first order reaction, the rate constant for the decomposition of N2O5 is 6 × 10–4 s –1. The half-life period for decomposition in seconds is 1155.
संबंधित प्रश्न
Answer the following in one or two sentences.
What are the units for rate constants for zero-order and second-order reactions if time is expressed in seconds and concentration of reactants in mol/L?
Answer the following in one or two sentences.
Write the relationships between rate constant and half-life of the first order and zeroth-order reactions.
What are pseudo-first-order reactions?
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?
The rate of catalysed reaction is large than the uncatalysed reaction as _______.
Give one example of a pseudo first-order reaction.
What is half life of first order reaction if time required to decrease concentration of reactants from 0.8 M to 0.2 M is 12 hours?
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 \[\ce{A ->Product}\] 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
For a first-order reaction, the rate constant is 6.909 min−1 the time taken for 75% conversion in minutes is
Write the rate law for the following reaction.
A reaction that is second order in NO and first order in Br2.
Give two examples for zero order reaction.
From the following data, show that the decomposition of hydrogen peroxide is a reaction of the first order:
| t (min) | 0 | 10 | 20 |
| V (ml) | 46.1 | 29.8 | 19.3 |
Where t is the time in minutes and V is the volume of standard KMnO4 solution required for titrating the same volume of the reaction mixture.
The integrated rate equation for first-order reaction, A → product, 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 ____________.
The rate and the rate constants of the reaction, \[\ce{A + 2B -> C + D}\] are 8 × 10−3 mol dm−3 s−1 and 2 × 10−3 s−1 respectively. The concentrations of A and B are 4 mol dm−3 each. The overall order of the reaction is ____________.
For first order reaction the slope of the graph of log10 [A]t Vs. time is equal to ____________.
The time taken for 80% of a first order reaction to be complete is approximately ____________.
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?
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 ____________.
A certain zero order reaction has rate constant 0.025 M s-1. What will be the concentration of reactant 'A' after 15 seconds, if initial concentration is 0.50 M?
The expression to calculate time required for completion of zero order reaction is ______.
Obtain the expression for half-life and rate constant of the first-order reaction.
Which of the following reactions is not of the first order?
Calculate half-life of a first order reaction in minute if the rate constant is 1 × 10-3 s-1.
Which is the relation between half life and rate constant for a zero order?
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?
Calculate half life of reaction if rate constant of first order reaction is 0.0178 minute−1.
