Answer: The time taken is 9764.4 seconds
Explanation:
Rate law expression for first order kinetics is given by the equation:
[tex]k=\frac{2.303}{t}\log\frac{[A_o]}{[A]}[/tex]
where,
k = rate constant = [tex]1.42\times 10^{-4}s^{-1}[/tex]
t = time taken for decay process = ? sec
[tex][A_o][/tex] = initial amount of the reactant = 100 grams
[A] = amount left after decay process = 25 grams
Putting values in above equation, we get:
[tex]1.42\times 10^{-4}=\frac{2.303}{t}\log\frac{100}{25}\\\\t=9764.4s[/tex]
Hence, the time taken is 9764.4 seconds
