Important Equations chemistry Flashcards
enzyme velocity
V =
Vmax * [S])/(Km + [S]
osmotic pressure
Π = iMRT
Energy of electron - Bohr’s Model of the Hydrogen Atom
E = -Rh/n²
Electromagnetic energy of photons - Bohr’s Model of the Hydrogen Atom
E = hc/λ
Equilibrium constant for:
aA + bB ⇌ cC + dD
Kc = ([C]^c[D]^d)/([A]^a[B]^b)
calorimetry heat equation
q = mc∆T
Standard heat of reaction (∆H°rxn) - using heat of formations
∆H°rxn = (sum of ∆H°f of products) - (sum of ∆H°f of reactants)
Standard heat of reaction (∆H°rxn) - using bond dissociation energies
∆H°rxn = ∑∆Hbonds broken - ∑∆Hbonds formed
entropy
∆Suniverse = ∆Ssystem + ∆Ssurroundings
Gibbs free energy (G) - thermodynamics
∆G = ∆H - T∆S
Reaction Quotient for:
aA + bB ⇌ cC + dD
Q = ([C]^c x [D]^d)/([A]^a x [B]^b)
Boyle’s Law
PV = k; P₁V₁ = P₂V₂
Charles’s Law
V/T = k; V₁/T₁ = V₂/T₂
Gay-Lussac’s Law
P/T = k; P₁/T₁ = P₂/T₂
Avogadro’s Principle
n/V = k; n₁/V₁ = n₂/V₂
Combined Gas Law
(P₁V₁)/T₁ = (P₂V₂)/T₂
Ideal Gas Law
PV = nRT
Van der Waals equation of state
Partial Pressures:
Pt = Pa + Pb + Pc ….
root-mean-square speed
Urms = √(3RT/M)
Freezing-Point depression
∆T = i x (Kf) x molality
Boiling-Point elevation
∆T = i x (Kb) x molality
diffusion formula
r₁/r₂ = (1/2) * [√(m₂/m₁)]
percent composition by mass
(mass of solute/mass of solution) x 100%
mole fraction
(number of moles of compound)/(total number of moles in system)