Chemical Kinetic

$t_{1/2}=\dfrac{0.693}{k}$

$t_{1/2}=0.693k$

$k=0.693t_{1/2}$

$kt_{1/2}=\dfrac{1}{0.693}$

0

1

2

3

Potential energy

Bond energy

Thermal energy

Activation energy

0

1

1.5

2

rate of slowest step.

rate of fastest step.

average rate of various steps.

instantaneous rate of fast step.

rate $=k[A][B]^{2}$

rate $=[A][B]^{2}$

rate $=k[A]^{2}[B]$

rate $=k[A]^{0}[B]^{2}$

$s^{-1}$

of collision frequency

of rate constant

$\mathrm{mol}{\mathrm{dm}}^{-3}s^{-1}$

1.5

2.5

+1

4

one

zero

two

three

the amount of product formed increases linearly with time

the rate decreases linearly with time

the rate is linearly related to the concentration of the reactant

the concentration of the reactant decreases linearly with time.

$5.76\times{10}^{-3}s^{-1}$

$1.086\times{10}^{-3}s^{-1}$

$-2.5\times{10}^{-3}s^{-1}$

$2.5\times{10}^{-3}s^{-1}$

double of half-life period

finite

infinity

dependent on concentration of the reactant

$t_{1/2}\propto a$

$t_{1/2}\propto 1/a$

$t_{1/2}\propto a^{0}$

$t_{1/2}\propto 1/a^{2}$

$\dfrac{-E_{a}}{R}$

$\ln A$

$\ln k$

$\log_{10} A$

Nature of the reactants

Concentration of the reactants

Temperature of the reaction

Molecularity of the reaction