CHEMICAL KINETICS

This branch of Science deals with rates of chemical reactions, mechanism of reaction and factors influencing the reaction.

TYPES OF CHEMICAL REACTION

Very fast (instantaneous) Reaction:

  • Reaction is so fast, that the determination of rate of reaction is difficult.
  • Involve ionic species.
  • Occurs within 10-14 to10-16 seconds.

Examples:

AgNo3 + NaCl →AgCl + NaNO3

BaCl2 + H2SO4 → BaSO4 + 2HCl

HCl + NaOH → NaCl + H2O

Very Slow Reaction:

  • Reaction is slow, extremely slow
  • Determination of rate of reaction is difficult task.
  • Take months to show measurable change.

Examples:

KE Very Slow Reaction

Moderate Reactions:

  • Occurs at moderate and measurable rates at room temp.
  • Study of kinetics is simple.
  • Molecular in nature.

Examples:

2H2O2 → 2H2O + O2
2N2O5 → 2N2O4 + O2
CH3COOC2H5 + NaOH → CH3COONa + C2H5OH
C12H22O11 + H2O → C6H12O6 + C6H12O6
Cane sugar                         Glucose          Fructose
NO2 + CO → NO + CO2
2FeCl3 + SnCl2 → 2FeCl2 + SnCl4 (aqueous phase)

Elementary Reaction:

The reactions in which the rate equation corresponds to a stoichiometric equation called elementary reaction.

Non-Elementary Reaction:
The reactions which have no relation between stoichiometric equation and rates of reaction, called non-elementary reactions.

Single Reaction:
When single stoichiometric equation and single rate equation are chosen to represent the progress of the reaction we have single reaction.

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