Kinetics - 6, 16

1. reactant particles must collide with the correct orientation

2. reactant particles must collide with sufficient E(a)

Minimum amount of energy that colliding particles must require for a reaction to occur.

energy between reactants - energy in transition state

highest energy state on a reaction coordinate, point at which new bonds are being formed and old bonds are being broken

In an ideal gas, the kinetic energy of the molecules is spread over a range of values

Total number of particles in the sample

Curve flattens out

curve is taller and leaner

Higher speed, curve flattens

slower, taller & leaner

The lower the activation energy the more particles are eligible to take part in the reaction, shaded region larger

lnK = (-E(a)/R) x (1/t) x lnA *divide by 1000 as R is in J

ln(k1/k2) = -Ea/R (1/T2 - 1/T1)

Change in concentration or pressure of a reactant or products per unit of time.

1. c = n/v = 0.04/2.5 = 0.016

2. ROR = Δc/Δt = 0.016/20 seconds

3. average ROR = 8 x 10^-4 mol/dm^3/s

Δc/Δt

1. Draw a tangent to the curve at a particular time

2. divide Δy/Δx to find gradient

Salt + H2

Salt + water

salt + CO2 + H2O

Salt + water

1. as concentration increases

2. number of collisions increase

3. between reactant particles

4. leading to greater successful collisions

1. as temperature increases

2. particles gain kinetic energy

3. leading to frequent collisions

4. leading to greater successful collisions

1. as surface area increases

2. more reactant particles are exposed to other reactant particles

3. leading to greater successful collisions

1. As pressure in a system increases

2. distance between reactant particles decreases

3. leading to more frequent collisions

4. leading to greater successful collisions

1. substance that alters ROR

2. by lowering its activation energy

3. through an alternate path

4. without getting used up during the reaction

1. surface of transition metals are slightly positive due to transition metals

2. lone pairs in reactant particles are attracted to slightly positive charge.

3. temporary polar bonds formed till other reactant particles collide with it.

4. lowering activation energy

s^-1

mol^-1dm^3s^-1

mol^-2dm^6s^-1

frequency of collisions & probability that collisions are in the correct orientation.

Graph of lnK vs 1/T where m = -Ea/R

1. Elementary steps must add up to give the overall balanced equation

2. Reaction mechanisms must be consistent with experimental data

Reactants - concentration/pressure vs time

Products - concentration/pressure vs time

Surface area = powder vs granules on product conc.