2.3 Stoichiometric Chemistry
Volume - 1
Name: . . . . . . . . . . . . . . . . . . . . . . . . . . . Code: . . . . . . . . . . . . . . . . . . . . . . . . . . .
Section: . . . . . . . . . . . . . . . . . . . . . . . . . . Year: . . . . . . . . . . . . . . . . . . . . . . . . . . .
Md.Mostafizur Rahman, Lecturer of Chemistry, NASCD, Bangladesh Navy
Ex-Lecturer of Rajuk Uttara Model College, Milestone College
Mobile: 01876117734, 01913023175, E-mail:
1|Page
,Question 01: What is a mole?
Mole: A mole is used as a unit in a chemical substance.
The relative atomic mass or molecular mass expressed in the gram unit is called a mole. One mole
contains 6.023 𝑥 1023 atoms, ions or molecules. It’s denoted by n.
Mass
Volume Number,
Mole 6.023𝑥1023
22.4L
Concentration
Molarity
Question 02: What is molar volume?
Ans. Molar Volume: At STP, the volume of 1 mole of any substance in the gaseous state
occupies 22.4 L, which is called molar volume.
1 mole H2 gas = 22.4L
1 mole O2 gas = 22.4L
1 mole CO2 gas = 22.4L
Question 03: What is molar Mass?
Ans. Molar Mass: The summation of relative atomic mass in a molecule or compound is
called molar mass.
1 mole 𝐻2 gas = 2.016g
1 mole 𝐶𝑂2 gas = 44g
1 mole 𝐶 gas = 12g
Question 04: What is Avogadro's number?
Ans. Avogadro number: One mole of any substance contains 6.023 x 1023 atoms, ions, or
molecules. This number is called the Avogadro number. It's denoted by 𝑁𝐴
1 mole H2 gas = 6.023 x 1023 molecules
1 mole CO2 gas = 6.023 x 1023 molecules
1 mole C gas = 6.023 x 1023 atoms
Md.Mostafizur Rahman, Lecturer of Chemistry, NASCD, Bangladesh Navy
Ex-Lecturer of Rajuk Uttara Model College, Milestone College
Mobile: 01876117734, 01913023175, E-mail:
2|Page
, No. Topics Formula Note
𝑤 w = amount of solute(g)
1 Mole 𝑛= M = Molar Mass
𝑀
𝑉𝑜𝑙𝑢𝑚𝑒(𝐺𝑎𝑠) Volume in liters
2 Mole =
22.4
𝑎𝑡𝑜𝑚𝑠 𝑜𝑟 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠 Atoms number,
3 Mole 𝑛= Molecules number
6.023𝑥1023
𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 Empirical to the molecular
4 Mole 𝑛= formula
𝑀𝑎𝑠𝑠 𝑜𝑓 𝑒𝑚𝑝𝑖𝑟𝑖𝑐𝑎𝑙 𝑓𝑜𝑟𝑚𝑢𝑙𝑎
5 Mole = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑥 𝑉𝑜𝑙𝑢𝑚𝑒(𝐿) Molarity (Concentration)
M= Molar Mass
Amount of 𝑀𝑉𝑆 V= Volume (mL)
5 𝑤=
substance, 1000 S= Concentration
Percent 𝑎𝑡𝑜𝑚𝑖𝑐 𝑚𝑎𝑠𝑠 𝑥 𝑁𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑎𝑡𝑜𝑚𝑠 𝑥 100 Element percent=%
6 𝐸𝑙𝑒𝑚𝑒𝑛𝑡 =
Composition 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)𝑥 100
(𝑎𝑚𝑜𝑢𝑛𝑡 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡 𝑜𝑏𝑡𝑎𝑖𝑛𝑒𝑑 𝑓𝑟𝑜𝑚 𝑟𝑒𝑎𝑐𝑡𝑖𝑜𝑛)𝑥 100 =
Percentage of = 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔)
7 𝐶𝑎𝑙𝑐𝑢𝑙𝑎𝑡𝑒𝑑𝑎𝑚𝑜𝑢𝑛𝑡 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡 𝑓𝑟𝑜𝑚 𝑟𝑒𝑎𝑐𝑡𝑖𝑜𝑛 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)𝑥 100
yield =
𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑚𝐿)
𝑚𝑔
𝑠𝑜𝑙𝑢𝑡𝑒(𝑔) 𝑝𝑝𝑚 =
𝑝𝑝𝑚 = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑥 𝑀𝑟 𝑥 103 𝑝𝑚 = 𝑥 106 𝐿
𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔) 𝑚𝑔
ppm(Parts per
8 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)
𝑝𝑝𝑚 =
million) 𝑝𝑝𝑚 = 𝑥 106 𝐾𝑔
𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑚𝐿)
𝑝𝑝𝑏 = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑥 𝑀𝑟 𝑥 106
ppb(parts per 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)
9
billion) 𝑝𝑏 = 𝑥 109
𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔)
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)
𝑝𝑒𝑟𝑐𝑒𝑛𝑡 = 𝑥100
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔)
10 percent 𝑚𝑜𝑙𝑒 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑥 𝑀𝑟 𝑥 100
𝑋% =
1000
11 Dilution 𝑉1 𝑆1 = 𝑉2 𝑆2
12 limestone
Reaction Potassium Chlorate
13
Limestone + HCl
Md.Mostafizur Rahman, Lecturer of Chemistry, NASCD, Bangladesh Navy
Ex-Lecturer of Rajuk Uttara Model College, Milestone College
Mobile: 01876117734, 01913023175, E-mail:
3|Page
Volume - 1
Name: . . . . . . . . . . . . . . . . . . . . . . . . . . . Code: . . . . . . . . . . . . . . . . . . . . . . . . . . .
Section: . . . . . . . . . . . . . . . . . . . . . . . . . . Year: . . . . . . . . . . . . . . . . . . . . . . . . . . .
Md.Mostafizur Rahman, Lecturer of Chemistry, NASCD, Bangladesh Navy
Ex-Lecturer of Rajuk Uttara Model College, Milestone College
Mobile: 01876117734, 01913023175, E-mail:
1|Page
,Question 01: What is a mole?
Mole: A mole is used as a unit in a chemical substance.
The relative atomic mass or molecular mass expressed in the gram unit is called a mole. One mole
contains 6.023 𝑥 1023 atoms, ions or molecules. It’s denoted by n.
Mass
Volume Number,
Mole 6.023𝑥1023
22.4L
Concentration
Molarity
Question 02: What is molar volume?
Ans. Molar Volume: At STP, the volume of 1 mole of any substance in the gaseous state
occupies 22.4 L, which is called molar volume.
1 mole H2 gas = 22.4L
1 mole O2 gas = 22.4L
1 mole CO2 gas = 22.4L
Question 03: What is molar Mass?
Ans. Molar Mass: The summation of relative atomic mass in a molecule or compound is
called molar mass.
1 mole 𝐻2 gas = 2.016g
1 mole 𝐶𝑂2 gas = 44g
1 mole 𝐶 gas = 12g
Question 04: What is Avogadro's number?
Ans. Avogadro number: One mole of any substance contains 6.023 x 1023 atoms, ions, or
molecules. This number is called the Avogadro number. It's denoted by 𝑁𝐴
1 mole H2 gas = 6.023 x 1023 molecules
1 mole CO2 gas = 6.023 x 1023 molecules
1 mole C gas = 6.023 x 1023 atoms
Md.Mostafizur Rahman, Lecturer of Chemistry, NASCD, Bangladesh Navy
Ex-Lecturer of Rajuk Uttara Model College, Milestone College
Mobile: 01876117734, 01913023175, E-mail:
2|Page
, No. Topics Formula Note
𝑤 w = amount of solute(g)
1 Mole 𝑛= M = Molar Mass
𝑀
𝑉𝑜𝑙𝑢𝑚𝑒(𝐺𝑎𝑠) Volume in liters
2 Mole =
22.4
𝑎𝑡𝑜𝑚𝑠 𝑜𝑟 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠 Atoms number,
3 Mole 𝑛= Molecules number
6.023𝑥1023
𝑀𝑜𝑙𝑒𝑐𝑢𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 Empirical to the molecular
4 Mole 𝑛= formula
𝑀𝑎𝑠𝑠 𝑜𝑓 𝑒𝑚𝑝𝑖𝑟𝑖𝑐𝑎𝑙 𝑓𝑜𝑟𝑚𝑢𝑙𝑎
5 Mole = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑥 𝑉𝑜𝑙𝑢𝑚𝑒(𝐿) Molarity (Concentration)
M= Molar Mass
Amount of 𝑀𝑉𝑆 V= Volume (mL)
5 𝑤=
substance, 1000 S= Concentration
Percent 𝑎𝑡𝑜𝑚𝑖𝑐 𝑚𝑎𝑠𝑠 𝑥 𝑁𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑎𝑡𝑜𝑚𝑠 𝑥 100 Element percent=%
6 𝐸𝑙𝑒𝑚𝑒𝑛𝑡 =
Composition 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)𝑥 100
(𝑎𝑚𝑜𝑢𝑛𝑡 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡 𝑜𝑏𝑡𝑎𝑖𝑛𝑒𝑑 𝑓𝑟𝑜𝑚 𝑟𝑒𝑎𝑐𝑡𝑖𝑜𝑛)𝑥 100 =
Percentage of = 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔)
7 𝐶𝑎𝑙𝑐𝑢𝑙𝑎𝑡𝑒𝑑𝑎𝑚𝑜𝑢𝑛𝑡 𝑜𝑓 𝑝𝑟𝑜𝑑𝑢𝑐𝑡 𝑓𝑟𝑜𝑚 𝑟𝑒𝑎𝑐𝑡𝑖𝑜𝑛 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)𝑥 100
yield =
𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑚𝐿)
𝑚𝑔
𝑠𝑜𝑙𝑢𝑡𝑒(𝑔) 𝑝𝑝𝑚 =
𝑝𝑝𝑚 = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑥 𝑀𝑟 𝑥 103 𝑝𝑚 = 𝑥 106 𝐿
𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔) 𝑚𝑔
ppm(Parts per
8 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)
𝑝𝑝𝑚 =
million) 𝑝𝑝𝑚 = 𝑥 106 𝐾𝑔
𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑚𝐿)
𝑝𝑝𝑏 = 𝑀𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑥 𝑀𝑟 𝑥 106
ppb(parts per 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)
9
billion) 𝑝𝑏 = 𝑥 109
𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔)
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒(𝑔)
𝑝𝑒𝑟𝑐𝑒𝑛𝑡 = 𝑥100
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛(𝑔)
10 percent 𝑚𝑜𝑙𝑒 𝑛𝑢𝑚𝑏𝑒𝑟 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑥 𝑀𝑟 𝑥 100
𝑋% =
1000
11 Dilution 𝑉1 𝑆1 = 𝑉2 𝑆2
12 limestone
Reaction Potassium Chlorate
13
Limestone + HCl
Md.Mostafizur Rahman, Lecturer of Chemistry, NASCD, Bangladesh Navy
Ex-Lecturer of Rajuk Uttara Model College, Milestone College
Mobile: 01876117734, 01913023175, E-mail:
3|Page
