chemistry laws

Boyle’s Law

as pressure goes up, volume goes down, vice versa

assumes mass/temp stay constant

inversely proportional relationship

P₁ x V₁ = P₂ x V₂

Charles’ Law

as volume goes up, temperature goes down, vice versa

assumes pressure stays constant

directly proportional

V₁ / T₁ = V₂ / T₂

Gay-Lussac’s Law

as pressure goes up, temperature goes up, vice versa

assumes volume stays constant

directly proportional

P₁ / T₁ = P₂ / T₂

Le Chatelier’s Principle

when stress is added to system at equilibrium, it will readjust to lower stress

(Le chatelier’s) As concentration increases/products or reactants are added…

reaction shifts away from what is added

think: moving away from what is already full

(Le chatelier’s) As concentration decreases/products or reactants are removed…

reaction shifts toward removed

think: taking the place of what is removed

(Le chatelier’s) As pressure increases…

reaction shifts to smaller number of gas moles

REMEMBER: only count moles of (g)

(Le chatelier’s) As pressure decreases…

reaction shifts to larger number of gas moles

REMEMBER: only count moles of (g)

(Le chatelier’s) As temperature increases…

reaction shifts to favor endothermic reaction

think: goes away from heat/energy since heat/energy spot is “full”

(Le chatelier’s) As temperature decreases…

reaction shifts to favor exothermic reaction

think: moves into place of heat/energy since heat/energy is leaving

What is the function of catalysts?

• lower activation energy

• equilibrium is reached faster