Final answer:
The rate constant (k) for the first-order decomposition of SO2Cl2 reaction, with a half-life of 60 minutes, can be calculated as k = ln(2) / 60 minutes = 0.01155 min-1.
Step-by-step explanation:
The question asks for the calculation of the rate constant of a first-order reaction, specifically the decomposition of SO2Cl2, where the time required for the concentration to decrease to half its initial amount is given as 60 minutes. To calculate the rate constant (k) for a first-order reaction, we use the first-order rate law equation formulated as ln([A]0/[A]t) = kt, where [A]0 is the initial concentration and [A]t is the concentration at time t.
In this particular case, the concentration at time t is one-half of [A]0 since it takes 60 minutes to reach this point. Thus, the equation simplifies to ln(2) = kt. Since k is the only unknown and t is given as 60 minutes, we can solve for k. The rate constant k for the first-order reaction can then be calculated as k = ln(2) / 60 minutes = 0.01155 min-1, when expressing time in minutes.