Equlibrium - CHemistry

Kc > 1

Kc >>1

Product favoured →

Very strongly product favoured ( Very little reactants remain)

Kc < 1

Kc <<1

Reactant Favoured <-

Very strongly Reactant favoured ( Very little Product remain)

Partial Pressure

Individual Gas Pressure within gas mixture

Le Chateliers Principle

If Eq system is subjected to a change, the system will adjust itself to partially oppose effect of that change

Factors affecting Eq position

Temp

Concentration

Pressure

Adding Reactant (Conc.)

Formation of more products (Net FR)

Eq shifts →

Adding Product (Conc.)

Formation of more Reactants (Net RR)

Eq shifts <-

Removing product (Conc.)

Favours formation of products

Removing Reactants (Conc.)

Favours Formation of Reactants

Increasing pressure

Shifts to side with LESS particles

Decreasing Pressure

Shifts to side with MORE particles

Raising Temp

Favours Endothermic Reaction

Kc Decreases

Lowering Temp

Favours Exothermic Reactions

Kc Increases

Why Kc changes only to Temp

For concentration increasing one thing shifts Eq to counteract by producing more of the other.

Increasing temp depends on Exo or Endo. Increasing or Decreasing causes no shift in opposite direction to counteract so there will be wither more R or P causing Kc to change.

Adding water

Dilutes everything

One with most ions Dilutes the most

Haber Process

N2 + 3H2 = 2NH (-92kJ)

Eq Yield

Amount of Product Present at Eq

Meaning of Eq Constant

How far forward reaction proceeds before Eq is establishes and the Eq yield

Ocean Acidification Reactions

Ocean Acidification

As CO2(aq) increases (H)+ ions increases

pH decreases and solid CaCO3 starts to dissolve

Buffer Solutions

Are able to resist change in pH when small amounts of acid or base are added

Buffer Solutions are made of:

Weak Acid + Conjugate Base

Weak Base + Conjugate Acid

Adding Acid to Buffer

Conjugate base combines with H3O+ to maintain stable pH

Adding Base to Buffer

Conjugate acid combines with OH= to maintain stable pH

Buffer Capacity

Measure of effectiveness of a buffer solution to resist a change in pH when strong acid or base is added

Buffer Capacity is greatest when:

• High conc. of weak acid and its conjugate base
• Conc. of acid and conjugate base are equal