A radioactive substance undergoes decay as follows: $$\begin{array}{cc}\hline \text { Time (days) } & \text { Mass (g) } \\\\\hline 0 & 500 \\\1 & 389 \\\2 & 303 \\\3 & 236 \\\4 & 184 \\\5 & 143 \\\6 & 112 \\\\\hline\end{array}$$ Calculate the first-order decay constant and the halflife of the reaction.

The concept of first-order decay is a fundamental principle in understanding how certain processes, like the decay of radioactive substances, behave over time. When we say a reaction is first-order, it means that the rate of decay is directly proportional to the amount of the substance that remains at any given time. Mathematically, this can be expressed by the equation:
\[ N = N_0 e^{-kt} \]
In this equation, \(N\) represents the amount of substance remaining after time \(t\), \(N_0\) represents the initial amount of the substance, and \(k\) is the decay constant, which is unique to each radioactive substance. This first-order rate law indicates that as time progresses, the quantity of the substance decreases exponentially. The mention of 'exponential' is crucial here, as this distinguishes first-order decay from other types, such as zero-order or second-order decay, where the relationship between rate and concentration is not exponential.

The decay constant, denoted as \(k\), is an essential parameter in the context of radioactive decay, as it quantifies the speed at which a substance undergoes decay. To determine the decay constant from experimental data, we require the initial amount \(N_0\) and the amount remaining \(N\) after a certain time period \(t\).
The decay constant is calculated using the rearranged first-order decay equation:
\[ k = \frac{1}{t} \times \text{ln}\bigg(\frac{N_0}{N}\bigg) \]
Where \(\text{ln}\) denotes the natural logarithm. When calculating \(k\), it is crucial that the units of time are consistent to ensure that the decay constant is accurate. Knowing the decay constant is pivotal as it not only helps us understand the behavior of the radioactive decay over time but also assists in calculating the half-life of a substance, another vital concept in radioactivity. It's worth noting that a larger decay constant means a more rapidly decaying substance, which should be taken into account in safety and handling protocols.

The term half-life is widely recognized in the realm of radioactive decay. It refers to the time required for half of a radioactive substance to decay and can be considered a practical way to gauge how quickly a substance breaks down. The half-life, denoted as \(T_{1/2}\), is intricately linked to the decay constant and can be computed once the decay constant is known. The relation between half-life and decay constant for a first-order decay process is expressed by the equation:
\[ T_{1/2} = \frac{\text{ln}(2)}{k} \]
Using the natural logarithm of 2 accounts for the 'half' in half-life. This calculation shows that regardless of the initial amount of the substance, the half-life remains constant because it is determined by the decay constant. Consequently, a shorter half-life indicates that the substance will decay more quickly, meaning a relatively lively and potentially hazardous radioactive environment depending on the substance involved. Conversely, a longer half-life represents a slower decay process. This property is not only crucial in scientific calculations and predicting future amounts of a substance but also highly informative for understanding the potential long-term environmental and health impacts of radioactive substances.