Ref: Nelson Chemistry 12

1. By
Mohd Ruzaini Ridhwan

2.  The frequently of collisions and
 The fraction of those collision that are
effective

3. The minimum kinetic energy required to
convert kinetic energy to activation
energy during the formation of the
activated complex

4. Molecules are not all moving at the
same speed; some are moving
quickly and some slowly, but most
are in the mid-range of kinetic
energy.

5.  Particles require a minimum activation energy and
correct alignment for a collision to be effective. The
collision must provide sufficient energy to cause the
breaking and forming of bond, producing new
particles.
 Many reactions occurs as a sequence of elementary
steps that make up the overall reaction mechanism.

6.  Factor such as the atomic structure of the reactant and
the nature of their bonds, as well as the type of
reaction occurring.
 The rate of any depends on the nature of the chemical
substance reacting, because both the strength of
bond(s) to be broken and the location of the bond(s)
in the particle structure effect the likelihood that any
given collision is effective

8.  An increase in initial reactant concentration or in
reactant surface are increase the rate of a reaction
because the total number of collision possible per unit
time increase proportionately.
 A higher concentration of reactant means a greater
number of particles per unit volume, which are more
likely to collide as they move randomly within a fixed
space.
 The rate of reaction is generally directly proportional
to the concentration of a reaction.

10.  Meanwhile, surface area only applies to heterogeneous
reaction, such as gas react with solid or solid with a
liquid. Surface area affects a collision frequently
because reactants can collide only at the surface where
the substances are in contact. The surface are of solid
is fixed while the are of surface exposed for given
quantity depends on how finely divided the sample of
solid is.

11.  A rise in temperature increase the rate of a reaction for
two reasons: the total number of collision possible per
unit time is increased slightly; and, more importantly,
the fraction of collision that are sufficiently energetic
to be effective is increased dramatically.

13.  A catalyst increase the rate of reaction by providing an
alternative pathway, with lower activation energy, to
the same product formation. A much larger fraction of
collisions is effective following the changed reaction
mechanism. Catalysts are involved in the reaction
mechanism at some point, but are regenerated before
the reaction is complete.

14.  Heterogeneous catalyst – a catalyst in a reaction in
which the reaction in which the reactants and the
catalyst are in the different physical states
 Homogeneous catalyst - a catalyst in a reaction in
which the reaction in which the reactants and the
catalyst are in the same physical states

16. THE END