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

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

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

Create a free account to view solution

View Solution Free
Topic: Chemical Kinetics and Nuclear Chemistry·Practice all Chemical Kinetics and Nuclear Chemistry questions

More Chemical Kinetics and Nuclear Chemistry Questions

For a third order reactions : 3X → Y + Z the initial rate is 5 × 10-2 mol L-1S-1 when the conc. of X is 0.1 m...The half-life of a first-order reaction is 10 minutes. In what time, the rate of reaction will decrease from 6.0 × 1021 ...For the reaction A (g) + 2B(g) → C(g) + D(g) = k [A] [B]2 Initial pressure of A and B are respectively 0.60 atm an...Which is not true for a second order reaction ?...Consider following reaction, Zn + 2H+ → Zn2+ + H2Half-life period is independent of concentration of Zn at constan...