chemistry-class-12-unit-04-chapter-05-chemical-kinetics-l-5-16-qgiyys7-clm

Chemical kinetics Lecture-5

Rate of reaction

$CH_3CHO(g) \rightarrow$ $CH_4(g)+ CO(g)$
$n^o_{CH_3CHO}$ $\quad \quad \quad$ $0$ $\quad \quad \quad \quad$ $0$
$n^o_{CH_3CHO}-\xi$ $\quad \quad$ $\xi$ $\quad\quad\quad\quad \xi$
Example-
$CH_3CHO (g) \rightarrow$ $CH_4 (g)+ CO (g)$
The rate of this reaction can be followed by measuring the pressure in the system at constant volume and temperature

Chemical kinetics Lecture-5

Assume ideal gas behaviour of the gases

Chemical kinetics Lecture-5

Assume ideal gas behaviour of the gases

Chemical kinetics Lecture-5

Expression of the total pressure

Chemical kinetics Lecture-5

Expression of the total pressure

Chemical kinetics Lecture-5

Expression of the total pressure

Chemical kinetics Lecture-5

Kinetic analysis of experimental data

Chemical kinetics Lecture-5

Kinetic reaction profile

Chemical kinetics Lecture-5

Instantaneous rate

Chemical kinetics Lecture-5

Initial rate of reaction

Chemical kinetics Lecture-5

Initial rate of reaction

Chemical kinetics Lecture-5

Key points

It is preferred to do the initial rate calculation based on product appearance
Initial rate calculation has to be done very close to the starting point of the reaction $\rightarrow$ within 5% of the reaction
Except chain reactions the initial rate line or tangent will be the one which is the steepest

Chemical kinetics Lecture-5

Dependence of reaction rate on concentration

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