Practicing Success
All natural and artificial radioactive decay of unstable nuclei follows which order kinetics? |
Zero order First order Second order None of these |
First order |
The correct answer is option 2. First order. First-order kinetics describes a type of chemical or physical process where the rate of the reaction or decay is directly proportional to the concentration of one of the reactants or components involved. In the context of radioactive decay, it specifically refers to the rate at which unstable nuclei undergo decay to form stable nuclei. Here is a detailed explanation: \(\frac{d[N]}{dt} = -k[N] \) where \( k \) is the rate constant specific to the radioactive decay process. Exponential Decay: The solution to the differential equation for first-order kinetics results in an exponential decay function. The concentration of the radioactive substance decreases exponentially over time according to the equation: \([N] = [N]_0 \times e^{-kt} \) where: \( [N] \) is the concentration of the radioactive substance at time \( t \). \( [N]_0 \) is the initial concentration of the radioactive substance at \( t = 0 \). \( k \) is the rate constant. \( e \) is the base of the natural logarithm. This equation describes how the concentration of the radioactive substance decreases with time, with a characteristic exponential decay curve. Half-Life: In first-order kinetics, the concept of half-life is particularly significant. The half-life (\( t_{1/2} \)) is the time required for the concentration of the radioactive substance to decrease to half of its initial value (\( [N]_0 / 2 \)). For first-order reactions, the half-life is constant and independent of the initial concentration of the substance. Applications: First-order kinetics is observed in various natural and artificial radioactive decay processes, including the decay of isotopes such as uranium, thorium, carbon-14, and others. It's also applicable in fields such as nuclear physics, radiology, carbon dating, and environmental science. |