1. 2 H2 + O2 → 2 H2O +

2. Identify the factors that could affect the rate of a chemical reaction.
Use the Collision Theory to explain the factors influencing the rate of a reaction.
Explain the effect these factors have on the shape of a kinetic energy distribution curve.

3. Factors Affecting Reaction Rates
temperature
concentration or pressure of a reactant
surface area (particle size)
presence/absence of a catalyst.
nature of the reactants

4. More particles involved, more frequent collisions.
Effect of Particle Size (surface area)
Rate of reaction increases with increased surface area (crushing, grinding) .
More particles involved, more frequent collisions.

5. Effect of Concentration
Rate of reaction increases with increased concentration (mol/L) of particles.
More particles with activation energy -
more chances of a successful collision.

6. Closer particles – more chance of collisions.
Effect of Pressure
Only affects reaction rates of gaseous reactions.
Rate of reaction increases with decreased volume of the container - mimics higher [ ].
Closer particles – more chance of collisions.

7. More KE per particles – more frequent collisions and more EA.
Effects of a Temperature Change
Rate of reaction increases with increased temperature.
More KE per particles – more frequent collisions and more EA.

8. 10°C increase in temp usually doubles reaction rate.

9. Less bonds to break, faster the reaction.
Effect of the Nature of Reactants
1. Comparing reactions with similar compounds:
Less bonds to break, faster the reaction.
2 NO(g) + O2(g) → 2 NO2(g)
2 C8H18(g) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)

10. KNO3(aq) + NaI(aq) → KI(aq) + 2 NaNO3(aq)
2. Comparing reactions with similar bond numbers:
Covalent bonds takes longer to break than aqueous.
(aq) are already separated into ions, so are instantaneous.
H2(g) + I2(g) → 2 HI(g)
KNO3(aq) + NaI(aq) → KI(aq) + 2 NaNO3(aq)

11. KNO3(aq) + NaI(aq)→ KI(aq) + NaNO3(aq)

12. (g) faster > (l) > (s)
3. Comparing similar compounds and similar bond
numbers:
(g) faster > (l) > (s)
Stronger IMF to overcome
Less KE per particle
Less collisions
Less Surface area

13. Effect of Catalysts
A catalyst speeds up or starts a reaction by lowering the activation energy.
Does not alter products or ΔH.
Not involved in the overall chemical reaction
Appears unchanged.
Enzymes are known as biological catalysts.
An inhibitor is the opposite of a catalyst.

16. Things that increase reaction rate:
increased surface area
increased concentration
increased pressure
increased temperature
fewer bonds, aqueous or gas states
catalyst
To decrease reaction rate - do the opposite....