Solved Examples on Mole Concept
Example 1: Calculate the molecular mass of Ammonium Sulphate (NH4)2SO4.
Solution:
Since, the relative atomic masses of N = 14, H = 1, S = 32, O =16
Therefore, the molecular mass of the given compound is,
= 2 (14 × 1 + 1 × 4) + 32 + 16 × 4
= 2(14 + 4) + 32 + 64
= 2 × 18 + 32 + 64
= 36 + 32 + 64
= 132 amu
Example 2: The molecular mass of H2SO4 is 98 a.m.u. What does it mean?
Solution:
It means that one molecule of H2SO4 is 98 times as heavy as 1/12 the mass of a C-12 atom.
Example 3: Calculate the number of atoms present in 18g of H2O.
Solution:
The 18 g of H2O ⇒ 1 mole of H2O ⇒ NA molecules
Now, 1 molecule of H2O contain 3 atoms
⇒ 1 mole H2O will contain 3*NA atoms = 3 × 6.022 × 1023 atoms = 1.8066 × 1024 atoms
Example 4: How many moles are present in 200g of NaOH?
Solution:
The mass of 1 mole of NaOH = 23 + 16 + 1= 40 g
Therefore, in 200g of NaOH the number of moles present = 200g / 40g mol-1 = 5 mol
Example 5: Calculate the mass of an atom of oxygen element.
Solution:
Mass of 1 mole of oxygen = 16g
No. of atoms in 1 mole of oxygen = NA
Therefore, mass of one atom of oxygen = 16g / NA = 16 / (6.022 × 1023) = 2.657 × 10-23 g
Example 6: Find the ratio of moles of oxygen atoms present in the compounds H2SO4, H2SO3, and SO2.
Solution:
1 mole of H2SO4 contains 4 × NA atoms of oxygen
1 mole of H2SO3 contains 3 × NA atoms of oxygen
1 mole SO2 contains 2 × NA atoms of oxygen
Therefore the required ratio is 4 × NA : 3 × NA : 2 × NA = 4 : 3 : 2
Example 7: How many moles of hydrogen and oxygen gas are required to produce 13 moles of water?
Solution:
Chemical equation of water formation:
H2 + O2 ⇢ H2O
Now the balanced equation is
2H2 + O2 ⇢ 2H2O
Thus we can deduce that 2 moles of hydrogen gas and 1 mole of oxygen gas combine together to form 2 moles of water. We can write the equation as :
H2 (1 mole) + O2 (1/2 mole)⇢ H2O (1 mole)
Hence, for production of 13 moles of water the required chemical equation would be:
H2 (13 moles) + O2 (13/2 moles) ⇢ H2O (13 moles)
Hence, for production of 13 moles of water we need 13 moles of hydrogen and 6.5 moles of oxygen gas.
Example 8: Calculate moles of electrons present in 104 g of acetylene gas.
Solution:
Now, formula for acetylene gas is C2H2. It’s structure is H—C≡C—H. Therefore, number of electrons present in 1 molecule of acetylene are 14.
Now, mass of 1 mole of acetylene is 26g ⇒ 104g of acetylene are 4 moles.
Now, 1 mole of acetylene = NA molecules
⇒ NA molecules have 14 × NA electrons
⇒ 4 moles of acetylene have 4 × 14 × NA electrons = 56 × NA electrons = 56 moles of electrons.
Mole Concept
Mole concept is the method used to express the amount of substance. This has been experimentally proving that one gram atom of any element, as well as one gram molecule of any substance, contains the same amount of entities. The experimentally decided number is found to be 6.022137 × 1023. After the discovery of the mole concept, the problem of finding absolute atomic masses of atoms was solved. It was so because the mole concept helps to count the number of atoms or molecules in a definite amount of the given substance. Let’s learn more about mole concept formulas and examples.