Chemical Equilibria

Finals

Sulfuric acid, ammonia, ethylene, propylene, phosphoric acid, chlorine, nitric acid, urea, benzene, methanol, ethanol, and ethylene glycol

are examples of chemicals produced at scales of many billions of kg per year worldwide.

a major industry synthesis.

The transformation of raw materials into products of greater value by means of chemical reaction

Chemical Kinetics

• Study of reaction rates and

• Besides information about the speed at which reactions occur, kinetics also sheds light on the reaction mechanism (exactly how the reaction occurs).

SIGN CONVENTION

positive (+) for a product and negative (−) for a reactant

∣ν_i∣

is a stoichiometric coefficient

A_i

represents a chemical formula

ν_i

itself is called a stoichiometric number, and by the sign convention

zero

inert species

dε

a single variable representing the extent to which the reaction has proceeded,

ε

called the reaction coordinate, characterizes the extent or degree to which a reaction has taken place.

Collision Theory

When two chemicals react, their molecules have to collide with each other (in a particular orientation) with sufficient energy for the reaction to take place

1. There must be enough activation energy (Ea).

2. The reactant particles must collide with proper orientation.

TEMPERATURE

• INCREASES

• At higher temperatures, reactant molecules have more kinetic energy, move faster, and collide more often and with greater energy.

CONCENTRATION

• INCREASES

• As the concentration of reactants increases, so does the likelihood that reactant molecules will collide

CATALYST

• INCREASES

• Speed up reactions by lowering activation energy.

SURFACE AREA

INCREASES

More area for reactants to be in contact.

CATALYST

• A substance that fastens the reaction without getting consumed in the reaction.

• Provides an alternative pathway that has a lower activation energy.

Label all the Parts

• Energy

• X, Y, Z

• E_a (no catalyst)

• E_a (with catalyst)

• Delta G

• Reaction Progress