Question

The radioactive decay follows:
A.Zero order kinetics
B.First order kinetics
C.Second order kinetics
D.Pseudo first order kinetics

Answer 1

We know that radioactivity takes place when the nucleus of an unstable atom loses energy by emitting energy in form of electromagnetic waves (or) emitted particles known as radiation. In other words, it can be defined as the immediate emission of radiation in the form of high energy photons or the particles rising from the nuclear reaction is known as radioactivity. Radioactivity in other terms is radioactive decay, nuclear disintegration, and nuclear decay.

Complete step by step answer:
We have to remember that the radioactive decay (otherwise called atomic decay, radioactivity) is the cycle by which a precarious nuclear core loses energy by radiation. A material containing insecure cores is viewed as radioactive. Three of the most well-known kinds of decay are alpha decay, beta decay, and gamma decay, all of which include transmitting at least one particle or photons.
We need to know that the radioactive decay is viewed as the exemplary illustration of first-order kinetics. This isn't astonishing because in light of the fact that the energy of any atomic crash or cooperation is insignificant in contrast with the energies engaged with atomic cycles. As a result, the decay of radioactive isotopes is generally portrayed regarding half-lives instead of as far as rate constants. A table of half-existences of chosen radioactive isotopes is valuable in talking about atomic decay.
When managing radioactive isotopes the fixation is hard to quantify. This focus is less helpful than the real number N of cores of some sort present. The incorporated type of the integrated type of rate law is $ln\left( {N/{N_0}} \right) = - {\text{ }}kt$ .
Therefore, the option (B) is correct.

Note:
We need to know that the half-life of first-order kinetics under a given arrangement of response conditions is consistent. This isn't valid for zero-order and second-order reactions. The half-life of first-order kinetics is autonomous of the centralization of the reactants. The rate constant for a first-order reaction is known, we can use half-lives to determine the time required for the reaction to attain a definite percent completion.