A quick-revision sheet of the core Plus Two (Class 12) Chemistry formulas — physical chemistry numericals made easy. From Veda Topper International, Irinjalakuda.
Mole concept & solutions
- Moles n = given mass / molar mass
- Number of particles = n × 6.022 × 10²³ (Avogadro number)
- Molarity (M) = moles of solute / volume of solution (L)
- Molality (m) = moles of solute / mass of solvent (kg)
- Mole fraction x = moles of component / total moles
Colligative properties
- Relative lowering of vapour pressure (Raoult): (P° − P)/P° = x_solute
- Boiling-point elevation: ΔT_b = K_b · m
- Freezing-point depression: ΔT_f = K_f · m
- Osmotic pressure: π = CRT
- van't Hoff factor i is multiplied in for electrolytes
Thermodynamics
- ΔU = q + w; w = −PΔV (at constant pressure)
- ΔH = ΔU + Δn_g RT
- ΔG = ΔH − TΔS
- ΔG° = −RT ln K = −2.303 RT log K
- ΔG° = −nFE°_cell
Electrochemistry
- E°_cell = E°_cathode − E°_anode
- Nernst (298 K): E = E° − (0.059/n) log Q
- Conductivity: molar conductivity Λ_m = κ × 1000 / M
- Faraday: charge Q = n × F (F = 96500 C/mol)
Chemical kinetics
- Rate = k [A]^x [B]^y (x + y = order)
- First-order: k = (2.303/t) log ([A₀]/[A])
- First-order half-life: t½ = 0.693 / k
- Arrhenius: k = A e^(−Ea/RT)
Equilibrium & ionic equilibrium
- pH = −log[H⁺]; pH + pOH = 14; K_w = 1 × 10⁻¹⁴
- Henderson: pH = pK_a + log([salt]/[acid])
- K_p = K_c (RT)^Δn_g
- Degree of dissociation & K_a for weak acids: K_a = cα²/(1−α)
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