Chemical Kinetics and Nuclear ChemistryHard

Question

For a first-order reaction, t0.75 = 1386 s. Its specific reaction rate is

Options

A.10−3 s−1
B.10−2 s−1
C.10−4 s−1
D.10−5 s−1

Solution

$t_{0.75} = 2 \times t_{0.50} \Rightarrow 1386\text{ sec = 2} \times \frac{0.693}{K}$

$\therefore K = 10^{- 3}\text{ }\text{s}^{- 1}$

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