Comprehensive List of Physics and Chemistry Formulas for Effective Exam Preparation

Physics Formulas

Physics is a subject that emphasizes understanding rather than rote memorization. It is particularly challenging as it demands a high level of attentiveness. At Dream Big Institution, the team provides a collection of formulas that not only enhance comprehension but also expand thinking capabilities. These formulas serve as a valuable resource, enabling students to delve deeper into the subject and develop a broader perspective.

Physics Formulas	Formulas
Average Speed Formula	S = d/t
Acceleration Formula	a =v-u/t
Density Formula	P=m/V
Power Formula	P=W/t
Newton’s Second Law	F = m × a
Weight Formula	W=mg
Pressure Formula	P=F/A
Ohm’s Law Formula	V= I × R
Kinetic Energy Formula	E = ½ mv²
Frequency Formula	F =v/λ
Pendulum Formula	T = 2π√L/g
Fahrenheit Formula	F = (9/5× °C) + 32
Work Formula	W = F × d × cosθ
Torque Formula	T = F × r × sinθ
Displacement Formula	ΔX = Xf–Xi
Mass Formula	F = m × a or m = F/m
Amplitude Formula	x = A sin (ωt + ϕ)
Tension Formula	T= mg+ma
Surface Charge Density Formula	σ = q / A
Linear Speed Formula	V(linear speed) = ΔS/ΔT
Position Formula	Δx=x2−x1
Heat of Fusion Formula	q = m × ΔHF
Gravity Formula	F α m₁m₂/r₂
Spring Potential Energy Formula	P.E=1/2 k × x2
Physics Kinematics Formula	v2=v2o+2a(x-xo)
DC Voltage Drop Formula	V=I ×  R
Hubble’s Law Formula	v = Ho r
Induced Voltage Formula	e = – N(dΦB/dt)
Latent Heat Formula	L = Q / M
Wavelength Formula	λ = v/f
Gravitational Force Formula	F = G(m1m2)/R2
Potential Energy Formula	PE = mgh
Strain Energy Formula	U = Fδ / 2
Friction Force Formula	f = μN
Cell Potential Formula	E0cell = E0red − E0oxid
Shear Modulus Formula	(shear stress)/(shear strain) = (F/A)/(x/y)
Water Pressure Formula	Water pressure= ρ g h
Refractive Index Formula	n = c/v
Centroid Formula	C = [(x1 + x2 + x3)/ 3, (y1 + y2 + y3)/ 3]

Important Physics Formulas

Given below is the most important Physics formulae list:

• Planck constant h = 6.63 × 10−34 J.s = 4.136 × 10-15 eV.s
• Gravitation constant G = 6.67×10−11 m3 kg−1 s−2
• Boltzmann constant k = 1.38 × 10−23 J/K
• Molar gas constant R = 8.314 J/(mol K)
• Avogadro’s number NA = 6.023 × 1023 mol−1
• Charge of electron e = 1.602 × 10−19 C
• Permittivity of vacuum 0 = 8.85 × 10−12 F/m
• Coulomb constant 1/4πε0 = 8.9875517923(14) × 109 N m2/C2
• Faraday constant F = 96485 C/mol
• Mass of electron me = 9.1 × 10−31 kg
• Mass of proton mp = 1.6726 × 10−27 kg
• Mass of neutron mn = 1.6749 × 10−27 kg
• Stefan-Boltzmann constant σ = 5.67 × 10−8 W/(m2 K4)
• Rydberg constant R∞ = 1.097 × 107 m−1
• Bohr magneton µB = 9.27 × 10−24 J/T 
• Bohr radius a0 = 0.529 × 10−10 m 
• Standard atmosphere atm = 1.01325 × 105 Pa 
• Wien displacement constant b = 2.9 × 10−3 m K .
• Wave = ∆x ∆t wave = average velocity ∆x = displacement ∆t = elapsed time.
• Vavg = (vi + vf*)2

Vavg = The average velocity 

vi = initial velocity 

vf = final velocity

• a = ∆v ∆t,

a = acceleration 

∆v = change in velocity 

∆t = elapsed time.

• ∆x = vi∆t + 1/2 a(∆t)2

∆x = the displacement 

vi = the initial velocity 

∆t = the elapsed time 

a = the acceleration 

• ∆x = vf∆t − 1/2 a(∆t)2

∆x = displacement 

vf = is the final velocity 

∆t = elapsed time

a = acceleration 

• F = ma 

F = force 

m = mass 

a = acceleration

• W = mg 

W = weight 

m = mass 

g = acceleration which is due to gravity.

• f = µN 

f = friction force 

µ = coefficient of friction 

N = normal force 

• p = mv
• W = F d cos θ or W = F!d 

W = work t

F = force 

d = distance 

θ = angle between F and the direction of motion

• KE  = 1/2 mv2 K

KE = kinetic energy

m = mass

v = velocity

• PE = mgh 

PE = potential energy 

m = mass 

g = acceleration due to gravity 

h = height

• W = ∆(KE) 

W = work done 

KE = kinetic energy. 

• P = W ∆t 

P = power

W = work

∆t = elapsed time

Solved Examples

Q.1. Calculate the dc voltage drop if the circuit length is 500 cms and in it 10 A of current flows in 20 s ?

Solution: 

The DC voltage drop is given as : V=L×I/T

where, I = current through the circuit in Amperes.

L = Length of the circuit in metres

T = time for which the current has flowed through the circuit in seconds

V = Voltage in Volts.

So, 

V=500×10/20

V = 0.25 Volts.

Q.2. The spring constant of a stretched string is 50Nm−1 and displacement is 20 cm. Compute potential energy stored in the stretched string.

Solution: 

Given parameters are,

k=50Nm−1

x = 20 cm = 0.2 m

Potential energy will be:

P.E=1/2k×x2

=½ X 50×(0.2)2

= 1 J

Q.3. A body moves along the x- axis according to the relation x=1–2t+3t2x=1–2t+3t2x = 1 – 2 t + 3t^{2}, where x is in metres and t is in seconds. Find the Acceleration of the body when t = 3s

Solution: 

We have,

x=1–2t+3t2x=1–2t+3t2x = 1 – 2 t + 3t^{2}then;

Velocity v= dx/dt= −2+6t

v= dx/dt= −2+6t

Acceleration:  v=dv/dt =6(m/s2)

Q.4. Calculate the weight of an object on the moon which weighs 50kg on earth.

Solution: 

Here weight = mass x gravitational acceleration

= m x g

= 50 kg x 1.6 m/s2

= 80 Kg m/s2

Q.5. Find the displacement covered by an object which accelerates from rest to 60 m/s in 3s. 

Solution: 

Initial velocity = 0 and final velocity = 60 m/s

Time taken = 3s

Therefore, acceleration = 60/3 = 20m/s2.

Displacement (S) = ut + ½ at2

= 90 m

Q.6. A person goes from Point A to Point B in 10s and returns back in 8s. If the distance between A and B is 36m, find the average speed of the person.

Solution: 

Here total distance covered = 72m

Total time taken = 18s

Therefore, average speed  = Total distance covered/Total time taken

=72/18

Total distance covered total time taken=7218

= 4 m/s.

Q.7. If an object is moving with a velocity of 5 m/s and has a kinetic energy of 100J, Find its mass.

Solution: 

We know that KE = ½ mv2

100 = ½ x m x 5 x 5

100 = 25 m/2

m = 100×2/25 = 200/25

= 8 kg

Q.8. A long thin rod of length 50 cm has a total charge of 5 mC uniformly distributed over it. Find the linear charge density.

Solution:

q = 5 mC = 5 × 10–3 C, l= 50 cm = 0.5 m. λ=?

λ=ql

=(5×10^−3)/0.5

=(5×10^−3)/0.5

=10^-2Cm^−1

Q.9. A car is travelling with a velocity of 10 m/s and it has a mass of 250 Kg. Compute its Kinetic energy?

Solution: 

As given here,

Mass of the body, m = 250 Kg,

Velocity of it, v = 10 m/s,

So Kinetic energy will be as:

E = 1/2mv^2

E = 1/2×250×10^2

= 125 ×100

E = 12500 joules

Q.10. The heat needed for a phase transfer of a 2 kg substance is 400k.cal. Determine its latent heat.

Solution: 

Given parameters are,

Q = 400 k.cal

M = 2 kg

The formula for latent heat is given by,

L = Q / M

L = 400 / 2

L = 200 k.cal/kg

How to use Physics formulas effectively

When you reach class 11, the practical application of physics becomes more apparent, especially in mechanics. This branch of physics offers a multitude of fascinating concepts to explore. Here, you will learn how to apply physics formulas to solve numerical problems and how to integrate multiple concepts seamlessly. Whether you are tackling objective or subjective questions, two crucial elements come into play: a clear understanding of the underlying concepts and the skillful utilization of physics formulas.

To effectively utilize physics formulas, it is advisable to begin by thoroughly studying the chapter. Alongside this, you can download the Physics Wallah physics formula sheet specific to that chapter. Familiarize yourself with all the formulas and then proceed to solve numerical problems. This approach enables you to develop a solid grasp of the subject matter and comprehend the practical application of the physics formulas.

Furthermore, the physics formula sheet proves invaluable during last-minute revisions, particularly in the week leading up to your exams. By reviewing the entire sheet of physics formulas before the final exam, you can expedite the syllabus completion process and enhance the efficiency of your revision. Last-minute revisions have the potential to significantly improve your grades, making it highly recommended to create personalized notes with the aid of the physics formula sheet. Writing down the formulas and concepts reinforces your understanding and aids in retaining the information effectively.

Chemistry Formulas

Chemistry, a branch of science that explores the physical and chemical properties of substances, plays a crucial role in the formation of new materials. It encompasses the study of all the elements present in nature, each possessing a distinct name derived from chemical investigations. These chemical proportions and compositions are represented by formulas, commonly known as chemical formulas.

Chemical formulas serve as a means for scientists to express the precise arrangement of atoms within a molecule or a chemical compound. They utilize the symbols of chemical elements along with numerical subscripts to indicate the number of atoms involved. To facilitate comprehension, a chemistry formula table is often employed to aid in understanding and applying these formulas effectively.

Types of Chemistry Formulae or Chemical Formulae

There are three types of chemical formulae:

• Molecular Formula
• Empirical Formula
• Structural Formula

Molecular Formula: Molecular formula also known as true formula provides us with the exact number of atoms of every element present in a molecule. The numerical subscripts after the chemical symbols denote the total number of atoms present. The molecular formula also tells us about the type of atom present in a molecule of a compound. Below is an example of a molecular formula.

Molecular Formula of glucose: C₆H₁₂O₆ 

It represents the actual number of atoms of each constituent (Carbon, Hydrogen and Oxygen) in one molecule of glucose.

Empirical Formula: The word empirical represents something that can be assessed through observation. As such the empirical formula which is more than often emanated from experimental data is defined as the simplest ratio of all the atoms present in the elements that make up a compound. An example of empirical formula extracted by simplifying the molecular formula of glucose:

Empirical formula of glucose: CH₂O

It represents the whole ratio number of the atoms present that is, C, H and O

Structural Formula: While it is good to have chemical formulas in an easy and compact manner, it is also important to know the arrangements of atoms in them. The structural formula tells us about atomic bonding and their arrangement in spaces. It helps us to identify which atoms are bonded with one another and which are not. Given below is an example of the structural formula of glucose which represents the atomic bonding and arrangement.

How to Write Chemical Formulas?

A chemical formula can be written by the name of the elements that constitute a compound along with some basic rules and in a reverse manner.

1. Chemical formulas of binary compounds which are made of two different elements can be written with the help of valency.
2. The capacity of the combination of the elements to form a compound or compound is known as valency. 
3. Firstly the valencies of the two elements should be determined and then the sums of the valencies of the two different elements should be made equal by specifying the common lowest multiple of the two valencies. 
4. Cation is an atom with positive charge and anion is an atom with a negative charge. In case if a metal and non-metal are present, the metal should be placed first in the formula. For example NaCl, in which Na has a positive charge and Cl has a negative charge.

Let’s take an example of balanced 

Aluminium oxide:

O = 2 (belongs to group VI)

Al = 3 (belongs to group III)

Lowest common multiple of the valencies is 6,

O : 2 x 3 = 6

Al : 3x 2 = 6

The chemical formula of Aluminium oxide is Al₂O₃

Steps to Write a Chemical Reaction

It is important to note that balancing of chemical equations plays a major role in this process.  Basically, four rules are followed while writing a chemical equation. Let’s have a look below, 

1. On the left side of the equation, the right number of reactants is written.
2. On the right side of the equation, the right formulas constituting the products are written.
3. Both the reactants and the products are partitioned by an arrow which points towards the products. This arrow indicates “to produce”.
4. With the help of plus signs various products and reactants are separated. The plus sign indicates ” reacts with” on the reactants side and it means “and”  on the products side.

Let’s take an example of a balanced chemical reaction where hydrogen and chlorine will react to make HCl.

The first step involves writing the equation in terms of the formulas of both the elements, both of which are diatomic in nature.

H2 + Cl2 → HCl 

There are two hydrogen atoms and chlorine atoms on the reactants side and one atom each on the product which can be now fixed and balanced by the inclusion of the coefficient 2 on the side of the product.

H2 + Cl2 → 2HCl

Now both the sides are balanced having two hydrogen and chlorine atoms each.

Some examples of chemical reactions are listed below:

Photosynthesis: 6CO2 + 6H2O  → C6H12O6 + 6O2 + 6H2O

Calcium carbonate formation: CaCl2 + Na2CO3 → CaCO3 + 2NaCl

Iron rusting: 4Fe + 3O2 + 6H2O → 4Fe(OH)3.

Combustion of hydrogen: 2H2(g) + O2(g) → 2H2O(l ) 

Table of Chemical Formulas (Molecular)

Compound Name	Molecular Formulae
Acetic acid	CH3COOH
Hydrochloric acid	HCl
Sulfuric acid	H2SO4
Acetate	CH3COO–
Ammonia	NH3
Nitric acid	HNO3
Phosphoric acid	H3PO4
Sodium phosphate	Na3PO4
Calcium carbonate	CaCO3
Ammonium sulfate	(NH4)2SO4
Carbonic acid	H2CO3
Sodium bicarbonate	NaHCO3
Sodium hydroxide	NaOH
Calcium hydroxide	Ca(OH)2
Ethanol	C2H5OH
Hydrobromic acid	HBr
Nitrous acid	HNO2
Potassium hydroxide	KOH
Silver nitrate	AgNO3
Sodium carbonate	Na2CO3
Sodium chloride	NaCl
Cellulose	(C6H10O5)n
Magnesium hydroxide	Mg(OH)2
Methane	CH4
Nitrogen dioxide	NO2
Sodium nitrate	NaNO3
Sulfurous acid	H2SO3
Aluminium sulfate	Al2(SO4)3
Aluminium oxide	Al2O3
Ammonium nitrate	NH4NO3
Ammonium phosphate	(NH4)3PO4
Barium hydroxide	Ba(OH)2
Carbon tetrachloride	CCl4
Citric acid	C6H8O7
Hydrocyanic acid	HCN
Salicylic Acid	C7H6O3
Hydroiodic acid	HI
Hypochlorous acid	HClO
Iron iii oxide	Fe2O3
Magnesium phosphate	Mg3(PO4)2

List of Chemical Compound Formulas

Compounds are basically substances that constitute two elements or more in a definite percentage. With the help of chemical formulas, the atoms of the elements in a compound can be known. The list below shows some chemical compounds along with their chemical formulas.

Sl.No	Chemical Compound	Chemical Formula
1	Acetic acid formula	CH3COOH
2	Aluminium hydroxide	Al(OH)3
3	Acetate	CH3COO¯
4	Acetone	C3H₆O
5	Aluminium acetate	C₆H₉AlO₆
6	Aluminium bromide	AlBr3
7	Aluminium carbonate	Al2(CO3)3
8	Aluminium chloride	AlCl3
9	Aluminium fluoride	AlF3
10	Aluminium	Al
11	Aluminium iodide	AlI3
12	Aluminium oxide	Al2O3
13	Aluminium phosphate	AlPO₄
14	Amino acid	H2NCHRCOOH
15	Ammonia	NH₄
16	Ammonium dichromate	Cr2H₈N2O₇
17	Ammonium acetate	C2H3O2NH₄
18	Ammonium bicarbonate	NH₄HCO3
19	Ammonium bromide	NH₄Br
20	Ammonium carbonate	(NH₄)2CO3
21	Ammonium chloride	NH₄Cl
22	Ammonium hydroxide	NH₄OH
23	Ammonium iodide	NH₄I
24	Ammonium nitrate	NH₄NO3
25	Aluminium sulfide	Al2S3
26	Ammonium nitrite	NH₄NO2
27	Ammonium oxide	(NH₄)2O
28	Ammonium phosphate	(NH₄)3PO₄
29	Ammonium sulfate	(NH₄)2SO₄
30	Ammonium sulfide	(NH₄)2S
31	Argon gas	Ar
32	Ascorbic acid	C₆H₈O₆
33	Barium acetate	Ba(C₂H3O2)2
34	Barium bromide	BaBr2
35	Barium chloride	BaCl2
36	Barium fluoride	BaF2
37	Barium hydroxide	Ba(OH)2
38	Barium iodide	BaI2
39	Barium nitrate	Ba(NO3)2
40	Barium oxide	BaO
41	Barium phosphate	Ba3O₈P2
42	Barium sulfate	BaSO₄
43	Benzene	C₆H₆
44	Benzoic acid	C₇H₆O2
45	Bicarbonate	CHO3¯
46	Bleach	NaClO
47	Boric acid	H3BO3
48	Potassium Bromate	KBrO3
49	Bromic acid	HBrO3
50	Bromine	Br
51	Butane	C₄H₁₀
52	Butanoic acid	C₄H₈O2
53	Calcium acetate	C₄H₆CaO₄
54	Calcium bromide	CaBr2
55	Calcium carbonate	CaCO3
56	Calcium hydride	CaH2
57	Calcium hydroxide	Ca(OH)2
58	Calcium iodide	CaI2
59	Calcium nitrate	Ca(NO3)2
60	Calcium oxide	CaO
61	Carbon monoxide	CO
62	Carbon tetrachloride	CCl₄
63	Carbonic acid	H2CO3
64	Calcium phosphate	Ca3(PO₄)2
65	Carbonic acid	H2CO3
66	Citric acid	C₆H₈O₇
67	Chlorate	ClO3¯
68	Chlorine	Cl
69	Chlorine gas	Cl2
70	Chlorous acid	HClO2
71	Chromate	CrO₄²¯
72	Chromic acid	H2CrO₄
73	Citric acid	C₆H₈O₇
74	Copper ii carbonate	CuCO3
75	Copper ii nitrate	Cu(NO3)2
76	Cyanide	CN¯
77	Dichromate	K2Cr2O₇
78	Dihydrogen monoxide	OH2
79	Dinitrogen monoxide	N2O
80	Dinitrogen pentoxide	N2O₅
81	Dinitrogen trioxide	N2O3
82	Ethanol	C2H₅OH
83	Iron oxide	Fe2O3
84	Ethylene glycol	C2H₆O2
85	Fluorine gas	F2
86	Aluminium bromide	AlBr3
87	Aluminium sulphide	Al2S3
88	Ammonium carbonate	(NH₄)2CO3
89	Ammonium nitrate	(NH₄)(NO3)
90	Ammonium phosphate	(NH₄)3PO₄
91	Barium chloride	BaCl2
92	Barium sulphate	BaSO₄
93	Calcium nitrate	Ca(NO3)2
94	Carbon monoxide	CO
95	Carbon tetrachloride	CCl₄
96	Carbonic acid	H2CO3
97	Hydrofluoric acid	HF
98	Hydroiodic acid	HI
99	Hypochlorous acid	HClO
100	Lithium phosphate	Li3PO₄
101	Magnesium nitrate	MgNO3
102	Magnesium phosphate	Mg3(PO₄)2
103	Nitrogen monoxide	NO
104	Nitrous acid	HNO2
105	Potassium carbonate	K2CO3
106	Potassium iodide	KI
107	Potassium nitrate	KNO3
108	Potassium phosphate	KH2PO₄
109	Sodium carbonate	Na2CO₄
110	Sodium oxide	Na2O
111	Fructose chemical	C₆H₁2O₆
112	Glycerol	C3H₈O3
113	Helium gas	He
114	Hexane	C₆H₁₄
115	Hydrobromic acid	HBr
116	Hydrochloric acid	HCl
117	Hydrocyanic acid	HCN
118	Hydrofluoric acid	HF
119	Hydrogen carbonate	CHO3¯
120	Hydrogen gas	H2
121	Hydrogen peroxide	H2O2
122	Hydrogen phosphate	H3PO₄
123	Hydrogen sulphate	HSO₄¯
124	Hydroiodic acid	HI
125	Hydrosulfuric acid	H2SO₄
126	Hydroxide	OH¯
127	Hypobromous acid	HBrO
128	Hypochlorite	NaClO
129	Hypochlorous acid	HClO
130	Hypoiodous acid	HIO
131	Iodic acid	HIO3
132	Iodide	I¯
133	Iodine	I₂
134	Iron iii nitrate	Fe(NO3)3
135	Iron ii oxide	FeO
136	Iron iii carbonate	Fe2(CO3)3
137	Iron iii hydroxide	Fe(OH)3
138	Iron iii oxide	Fe2O3
139	Iron iii chloride	FeCl3
140	Lactic acid	C3H6O3
141	Lead acetate	Pb(C2H3O2)2
142	Lead ii acetate	Pb(C2H3O2)2
143	Lead iodide	PbI2
144	Lead iv oxide	PbO2
145	Lead nitrate	Pb(NO3)2
146	Lithium bromide	LiBr
147	Lithium chloride	LiCl2
148	Lithium hydroxide	LiOH
149	Lithium iodide	LiI
150	Lithium oxide	Li2O
151	Lithium phosphate	Li3PO4
152	Magnesium acetate	Mg(CH3COO)2
153	Magnesium bicarbonate	C2H2MgO6
154	Magnesium carbonate	MgCO3
155	Magnesium chloride	MgCl2
156	Magnesium hydroxide	Mg(OH)2
157	Magnesium iodide	MgI2
158	Magnesium nitrate	Mg(NO3)2
159	Magnesium nitride	Mg3N2
160	Magnesium carbonate	MgCO3
161	Magnesium bromide	MgBr2
162	Magnesium oxide	MgO
163	Magnesium phosphate	Mg3(PO4)2
164	Magnesium sulphate	MgSO4
165	Magnesium sulphide	MgS
166	Methane	CH4
167	Methanol	CH3OH
168	Nickel acetate	Ni(C2H3O2)2
169	Nickel nitrate	Ni(NO3)2
170	Nitric acid	HNO3
171	Nitride	N3–
172	Nitrite	NO2−
173	Nitrogen dioxide	NO2
174	Nitrogen monoxide	NO
175	Nitrous acid	HNO2
176	Oxalate	C2O42¯
177	Oxalic acid	H2C2O4
178	Oxygen	O2
179	Ozone	O3
180	Perbromic acid	HBrO4
181	Potassium Permanganate	KMnO4
182	Permanganate ion	MnO4–
183	Phosphate	PO43-
184	Sodium hydrogen phosphate	Na2HPO4
185	Sodium formate	CHNaO2
186	Phosphoric acid	H3PO4
187	Phosphorus pentachloride	PCl5
188	Phosphorus trichloride	PCl3
189	Potassium acetate	CH3CO2K
190	Potassium bicarbonate	KHCO3
191	Potassium carbonate	K2CO3
192	Potassium chlorate	KClO3
193	Potassium hydrogen phosphate	K2HPO4
194	Potassium chloride	KCl
195	Potassium chromate	CrK2O4
196	Potassium cyanide	KCN
197	Potassium dichromate	K2Cr2O7
198	Potassium fluoride	KF
199	Potassium hydroxide	KOH
200	Potassium hypochlorite	KClO

Physics Formulas and Chemistry Formulas (FAQs)