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28 terms

snarebear

# MCAT Chemistry Equations

###### STUDY

###### PLAY

Nernst Equation

Ecell=Eºcell- (RT/nF) (lnQ)

Gibbs Free Energy (in relation to EMF)

ΔG=-nFEcell

Standard Electromotive Force

EMF=Eºreduction-Eºoxidation

Standard Conditions

25º C, 1 atm Pressure, 1 M concentrations, most stable form of each compound

Faraday’s Constant

1 F=96487 J/V

Henderson-Hasselbach Equation

pH=pKa + log [conj. Base]/[weak acid]

Relation Between base and acid dissociation constants

Ka * Kb = Kw= 1E-14

Base dissociation Constant

Kb= [B⁺]*[OH⁻]/[BOH]

Acid dissociation constant

Ka=[H3O⁺]*[A⁻]/[HA]

Water dissociation constant

Kw=[H⁺]*[OH⁻]=1E-14; pH + pOH=14

pH

pH=-log([H⁺])=log(1/[H⁺])

Boyle’s Law

P₁V₁=P₂V₂

Charles’ Law

V₁/T₁=V₂/T₂

Avagadro’s Principle

n₁/V₁=n₂/V₂

Ideal Gas Law

PV=nRT

Ideal Gas Constant

0.0821 L

**atm/mol**k or 8.314 J/mol*KDalton’s Law of Partial Pressures

P(total)=Pa+Pb+Pc+…

Pa=Xa*P(total)

Pa=Xa*P(total)

Root Mean Square Speed

uRMS=√(3RT/MM), MM=molec mass

Graham’s Law of Diffusion/Effusion

r1/r2=√(MM2/MM1)

Freezing Point Depression

ΔTf=Kf*m; m=molality (moles/kg), Kf=freezing constant for solvent

Boiling point elevation

ΔTb=Kb*m; m=molality (moles/kg), Kb= boiling constant for solven

Osmotic Pressure

π=MRT; M=molarity (moles/L)

Raoult’s Law

ΔP=Xb

**Pºa; Pa=Xa**a*Pºa, where Pºa is the vapor pressure of pure a, Xa is the mole fraction of a.Dilution

M₁V₁=M₂V₂

Heat absorbed or released

q=mcΔT; where m is mass and c is specific heat

Enthalpy change

ΔHreaction=Hproducts-Hreactants; where positive, endothermic rxn, negative, exothermic

Entropy change

ΔS=Sfinal-Sinitial; where positive, disorder increases, negative, order increases

Gibbs Free Energy

ΔG=ΔH-TΔS, must be negative to be spontaneous

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