Chem 1 Unit 3 Review

ΔH > 0 (What process is this?)

Endothermic (Chart up)

ΔH

Enthalpy

ΔH < 0 (What process is this?)

Exothermic (Chart down)

1st Law of Thermodynamics

ΔE_univ = ΔE_sys + ΔE_sur = 0

where ΔE_sys = q + w

and ΔE_sur = -ΔE_sys

ΔS

Entropy

ΔS > 0

When moles of gas increases (Chart moves up)

ΔS < 0

When moles of gas decreases (Chart moves down)

ΔS = 0

When moles of gas stay the same

When is ΔG Spontaneous?

ΔG < 0

When is ΔG Spontaneous in relation to ΔH and ΔS? (chart)

ΔH	ΔS	ΔG < 0 (spontaneous)
-	+	Always
+	-	Never
+	+	At high T
-	-	At low T

Equilibrium constant formula

K_eq = (Products^charge)^moles / (Reactants^charge)^moles

^{(Do not include Solids/Liquids)}

Rate of Forward rxn

R_f = K_f (REACTANTS^charge)^moles

Rate of reverse rxn

R_r = K_r (PRODUCTS^charge)^moles

Le Chatlier’s principle

More products/ Less reactants = shifts LEFT (decreases products, increases reactants)

Less Products/ More reactants = shifts RIGHT (decreases reactants, Increases products)

In an exothermic reaction, heat is a (reactant/product)

Product (ΔH < 0)

In an endothermic reaction, heat is a (reactant/product)

Reactant (ΔH > 0)

Concentration formula

Moles/Liters

Difference between hydrophobic and hydrophilic solutions

Hydrophobic = Polar

Hydrophilic = non-polar

Is H₂O Polar or non polar?

Polar

Do ions dissolve well in polar or non-polar solvents?

Polar solvents

Electrolytes vs Nonelectrolytes

Electrolytes = Ions, strong acids + bases. (Aq. solutions conduct electricity)

Nonelectrolyes= Molecules. (Aq. solutions do not conduct electricity

Name the Strong acids (to be electrolytes)

HCl, HBr, Hl, HNO_3, HClO_{3 ,} HClO₄ , H₂SO₄

Name the strong bases (to be electrolytes)

LiOH, NaOH, RbOH, CSOH, KOH, Ba(OH)₂ , Sr(OH)_2, Ca(OH)₂

K_sp in relation to solubility

Larger K_sp = more soluble

(Note: K_sp uses the same formula as K_eq )

A good Oxidizing agent is one in

empty low e orbitals

A good reducing agent is one in

High energy E orbitals

When is E cell spontaneous and non spontaneous?

When E Cell > 0 , ΔH < 0 (SPONTANEOUS)

When E Cell < 0, ΔH > 0 (non-spontaneous)

What energy is converted in a galvanic cell?

Chemical to Electrical energy

In a galvanic cell, electrons flow from the ____ to the ____

Cathode to anode

In a galvanic cell, the cathode electrode usually (grows/shrinks) while the anode electrode (grows/shrinks)

Cathode electrode GROWS, anode electrode SHRINKS

In a galvanic cell, the cathode department (reduces/increases) in redox ion and holds the (reduction/oxidation) compartment

Reduces, reduction

In a galvanic cell, the anode department (reduces/increases) in redox ion and holds the (reduction/oxidation) compartment

Increases, Oxidation

galvanic vs electrolytic cell

Galvanic cell = spontaneous (chemical to electrical)

Electrolytic cell = non-spontaneous (electrical to chemical)

Components of an Alkaline/dry cell battery

Zinc (Zn), Manganese dioxide (MnO₂ ) and KOH

Components of a button battery

Ag₂O , Zn, MnO₂

Components of a car battery

Pb, H₂SO₄

Components of a lithium-ion battery

Lithium compounds

Components of a Nickel-metal hydride battery

HNi

Galvanization

Protection of one metal by adding a more reactive metal

a more reactive metal is one that is more negative/higher up on the reduction potential chart.