Principles of Chemical Reactions

1.
The three principles are:
Collision – collision between the molecules must be effective in such a way that they bring
chemical change.
Activation energy – the molecules should possess internal energy in order to have successful
collision.
Orientation – not only the collision and activation energy are required for an effective reaction
but also the orientation matters. The molecules must also collide in the proper orientation for a
reaction to occur.
2.
The reaction is classified as exothermic.
During the reaction, formation of products resulted in release of energy more than that of the
reactants, that is equal to -803kJ/mol.
Negative sign indicates that the energy is released.
Thus, this reaction is exothermic and generates 803 kJ of energy per mole.
3.
B
Activation energy – the molecules should possess internal energy in order to have successful
collision.
4.
D
Heat released.
5.

“H” represents the activated complex.
Because of the activated complex, the exothermic reactions do not occur spontaneously. The
activated complex is the step in the reaction when the compound is not stable.
6.
Sketch of the effect of the addition of a catalyst.
7.
The factors are:
Reactant concentration – concentration of reactants is directly proportional to the rate of reaction.