NEET UG 2026 Formula List: What Toppers Revise One Day Before Exam

Chapter/ Unit

Formula Name

Formulas

Notes

Kinematics

Projectile Range

R=gu2sin2θ​

Max range at θ=45∘

Gravitation

Variation of g (Height)

gh​=g(1−R2h​)

Valid for h<<R

Electrostatics

Electric Potential

V=4πϵ0​1​rq​

Scalar quantity

Current Electricity

Drift Velocity

vd​=meEτ​

τ is relaxation time

Ray Optics

Lens Maker’s Formula

f1​=(μ−1)(R1​1​−R2​1​)

Use the sign convention

Modern Physics

De-Broglie Wavelength

λ=2mK​h​

K is Kinetic Energy

Modern Physics

Radioactive Decay

N=N0​e−λt

λ=T1/2​0.693​

Chapter/ Unit

Formulas

Notes

Mole concept

n=wMn = \dfrac{w}{M}n=Mw

nnn = moles, www = mass, MMM = molar mass

n=NNAn = \dfrac{N}{N_A}n=NAN

NNN = number of particles, NAN_ANA = Avogadro’s number

n=V22.4n = \dfrac{V}{22.4}n=22.4V (at STP, gas)

STP = 0°C, 1 atm; 1 mol gas = 22.4 L

Concentration terms

Molarity M=nVLM = \dfrac{n}{V_{\text{L}}}M=VLn

VVV in litres

Molality m=nWkgm = \dfrac{n}{W_{\text{kg}}}m=Wkgn

WWW = mass of solvent in kg

Normality N=M×basicity / acidityN = M \times \text{basicity / acidity}N=M×basicity / acidity

For acids/bases

M1V1=M2V2M_1 V_1 = M_2 V_2M1V1=M2V2

Dilution formula

Gas laws

PV=nRTPV = nRTPV=nRT

Ideal gas equation

P∝1VP \propto \dfrac{1}{V}P∝V1 (constant T)

Boyle’s law

V∝TV \propto TV∝T (constant P)

Charles’s law

PT=constant\dfrac{P}{T} = \text{constant}TP=constant

Gay‑Lussac’s law

Thermodynamics

ΔU=q+w\Delta U = q + wΔU=q+w

First law (sign convention as per NCERT)

ΔH=ΔU+ΔngRT\Delta H = \Delta U + \Delta n_g RTΔH=ΔU+ΔngRT

Enthalpy–internal energy relation

ΔG=ΔH−TΔS\Delta G = \Delta H - T\Delta SΔG=ΔH−TΔS

Gibbs free energy

ΔG∘=−RTln⁡K\Delta G^\circ = -RT \ln KΔG∘=−RTlnK

Relation with the equilibrium constant

Chemical equilibrium

Kc=[C]c[D]d[A]a[B]bK_c = \dfrac{[C]^c [D]^d}{[A]^a [B]^b}Kc=[A]a[B]b[C]c[D]d

Law of mass action

Kp=Kc(RT)ΔnK_p = K_c (RT)^{\Delta n}Kp=Kc(RT)Δn

Relation between KpK_pKp and KcK_cKc

For weak acid: Ka=[H+][A−][HA]K_a = \dfrac{[H^+][A^-]}{[HA]}Ka=[HA][H+][A−]

Acid dissociation constant

For weak base: Kb=[BH+][OH−][B]K_b = \dfrac{[BH^+][OH^-]}{[B]}Kb=[B][BH+][OH−]

Base dissociation constant

Ionic equilibrium

pH =−log⁡[H+]= -\log[H^+]=−log[H+]

-

pOH =−log⁡[OH−]= -\log[OH^-]=−log[OH−]

-

pH + pOH = 14 (25°C)

-

Kw=[H+][OH−]=10−14K_w = [H^+][OH^-] = 10^{-14}Kw=[H+][OH−]=10−14

Ionic product of water

Electrochemistry

Q=ItQ = I tQ=It

Charge passed

m=QMnFm = \dfrac{Q M}{n F}m=nFQM

Faraday’s law of electrolysis

Ecell=Ecathode−EanodeE_{\text{cell}} = E_{\text{cathode}} - E_{\text{anode}}Ecell=Ecathode−Eanode

Cell potential

Nernst equation: E=E∘−0.059nlog⁡QE = E^\circ - \dfrac{0.059}{n} \log QE=E∘−n0.059logQ (25°C)

-

Chemical kinetics

Rate =k[A]n= k[A]^n=k[A]n

Rate law

For 1st order: t1/2=0.693kt_{1/2} = \dfrac{0.693}{k}t1/2=k0.693

Half‑life

Arrhenius: k=Ae−Ea/RTk = A e^{-E_a / RT}k=Ae−Ea/RT

Temperature dependence

Solutions

Relative lowering of vapour pressure =p∘−pp∘=x2= \dfrac{p^\circ - p}{p^\circ} = x_2=p∘p∘−p=x2

Raoult’s law (non‑volatile solute)

Elevation in boiling point ΔTb=Kbm\Delta T_b = K_b mΔTb=Kbm

-

Depression in freezing point ΔTf=Kfm\Delta T_f = K_f mΔTf=Kfm

-

Osmotic pressure π=CRT\pi = CRTπ=CRT

CCC = molar concentration

Surface chemistry (quick)

Freundlich Adsorption: xm=kP1/n\dfrac{x}{m} = k P^{1/n}mx=kP1/n

Empirical relation

Chapter/ Unit

Concept/ Value

Formulas

Notes

Genetics

Hardy-Weinberg

p2+2pq+q2=1

Allele frequency stability

Respiration

Respiratory Quotient

RQ=O2​ consumedCO2​ evolved​

Carbohydrates = 1.0

Physiology

Cardiac Output

SV×HR=CO

Normal ≈5000 ml/min

Ecology

Species-Area

logS=logC+ZlogA

Z is the slope of the line

Biomolecules

DNA Rules

A+G=T+C

Chargaff's Rule