2 H 2 + O 2 → 2 H 2 O. +. 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.
Identify the factors that could affect the rate of a chemical reaction.
Rate of reaction increases with increased surface area(crushing, grinding) .
More particles involved, more frequent collisions.
Rate of reaction increases with increased concentration (mol/L) of particles.
Moreparticles with activation energy -
more chances of a successful collision.
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.
Rate of reaction increases with increased temperature.
MoreKEperparticles – more frequentcollisions and moreEA.
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)
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)
(g) faster> (l) > (s)
A catalyst speeds up or starts a reaction by lowering the activation energy.
Enzymes are known as biological catalysts.
An inhibitor is the opposite of a catalyst.
To decrease reaction rate - do the opposite....