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Published on: 13/05/2022
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Questions + Answers key
Take MCQ Science Test1.
Calculate the number of molecules in 11g of CO2
2.
Write the applications of Avogadro's law.
3.
Relative molecular mass of water (H2O) is calculated as follows: A water molecule is made of 2 atoms of hydrogen and one atom of oxygen.
4.
Relative molecular mass of sulphuric acid (H2SO4) is calculated as follows: Sulphuric acid contains 2 atoms of hydrogen, 1 atom of sulphur and 4 atoms of oxygen.
5.
Boron naturally occurs as a mixture of boron-10 (5 protons + 5 neutrons) and boron-11 (5 protons + 6 neutrons) isotopes. The percentage abundance of B-10 is 20 and that of B-11 is 80. Then, the atomic mass of boron is calculated as follows :
1.
Gram molecular of CO2 = 44g
Number of molecules present in 44g of CO2
= 6.023 X 1023
∴ Number of molecules present in 11g of CO2
= \(\frac{6.023\times{10}^{23}}{44}\)x 11
= 1.53 x 1023 molecules.
2.
i) Avogadro's law explains Gay-Lussac's law.
ii) It helps in the determination of atomicity of gases.
iii) Molecular formula of gases can be derived from Avogadro's law.
iv) It determines the relation between molecular mass and vapour density.
v) It helps to determine gram molar volume of all gases. (i.e., 22.4 litre at STP).
3.
So, the relative molecular mass of water
= (2 x mass of hydrogen) + (1 x mass of oxygen)
= (2 x 1) + (1 x 16 )
= 18.
i.e. one molecule of H2O is 18 times as heavy as \(\frac{1}{12^{th}}\) of the mass of a carbon -12.
4.
Therefore, Relative molecular mass of sulphuric acid
= (2 x mass of hydrogen) + (1 x mass of sulphur) + (4 x mass of oxygen)
= (2 x 1) + (1 x 32) + (4 x 16)
= 98.
i.e. one molecule of H2SO4 is 98 times as heavy as \(\frac{1}{12^{th}}\) of the mass of a carbon - 12.
5.
Atomic mass of Boron =\(\left(10 \times \frac{20}{100}\right)+\left(11 \times \frac{80}{100}\right)\)\(\)
= (10 x 0.20) + (11 x 0.80)
= 2+ 8.8
= 10.8 amu.
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Tamilnadu Stateboard 10th Standard Subjects
Tamilnadu Stateboard Standards
