Kinetics

rate of reaction ~ amount of substance produced per second 

FIVE WAYS OF INCREASING RATE:

• increase surface area = more particles exposed = greater collision frequency
• increase concentration = particles closer together = greater collision frequency
• increase temperature = particles have more energy, move faster = greater collision frequency + more successful collisions = double effect on rate of reaction 
• add a catalyst = lower activation energy = more successful collsions
• increase pressure = has to involved gases = same effect as concentration

a graph showing the distribution of molecular energies in a gas

• x-axis labelled "energy", y-axis labelled "number of molecules"
• area under curve gives total number of particles in sample
• starts at (0,0) because there no molecules with zero energy 

Increasing temperature:

• lowers peak of the curve
• shifts distribution to the right ~ more molecules with higher energies

Decreasing Temperature:

• raises the peak
• shifts the distribution to the left ~ less molecules with energy greater than activation energy

definition - a substance that increases the rate of reaction without going under any permanent change 

• in terms of Maxwell-Boltzmann distribution ~ lowering activation energy= more molecules have a energy greater than activation energy = so more collisions will be successful = rate will increase
• Catalyst do NOT appear in the equation for a reaction ~ written on top of arrow