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speed of reaction (measuring speed of a chemical reaction (Δ in…
speed of reaction
measuring speed of a chemical reaction
Δ in temperature against time
Δ in pH against time
Δ in mass/volume against time
formation of precipitate against time
Δ in colour against time
factors that affect the speed of reaction
temperature
↑ temperature
leads to
↑ rate of reaction
↑ temperature
leads to
↑ kinetic energy of particles
leads to
↑ frequency of particles colliding
leads to
↑ chance of reaction taking place
↑ frequency of effective collisions
leads to
↑ rate of reaction
surface area
↑ surface area of a solid
leads to
↑ rate of reaction
↑ frequency of effective collisions
leads to
↑ rate of reaction
↑ surface of a solid reagent
leads to
↑ area over which collisions between the chemicals take place
leads to
frequency of collision
concentration
↑ concentration
leads to
↑ rate of reaction
↑ concentration of solution
means
↑ particles it contains per unit volume. frequency of collision ↑ since particles are closer together
↑ frequency of effective collisions
leads to
↑ rate of reaction
pressure
↑ pressure of gas
leads to
↑ rate of reaction
↑ pressure of gas forces the particles closer together, which
leads to
↑ frequency of collision
↑ frequency of effective collisions
leads to
↑ rate of reaction
catalyst
adding a catalyst
leads to
↑ rate of reaction
↓ activation energy of reaction by allowing the reaction to take place via an alternative pathway
↓ activation energy
leads to
↑ collisions between particles will have sufficient energy for a reaction to take place
↑ frequency of effective collisions
leads to
↑ of rate of reaction
common catalysts used
Iron [Fe]
manufacture of ammonia (harber process)
Nickel [Ni]
manufacture of margarine
Vanadium(V)Oxide [V2O5]
manufacture of sulfuric acid (contact process)
enzymes
biological catalysts that ↑ speed of reaction
very sensitive to temperature and pH
reaction falls rapidly at temperatures ↑ 40°C
only functions over a narrow pH range
a catalyst reduces the
activation energy
of a reaction by allowing the reaction to take place via an
alternative pathway
collision theory
during a chemical reaction
the reacting chemical molecules must
collide
with each other
the reacting chemical molecules must collide with
sufficient energy
, equal to or greater than the reaction's activation energy
if the energy is sufficient (or greater) the collision caused the chemical bonds to break
now that the original bonds are broken, new chemical bonds can be formed
resulting in new chemical products
molecules move around randomly (kinetic energy)
eventually colliding