Advertisements
Advertisements
प्रश्न
A metal M, forms a volatile chloride containing 65.5% Chlorine. If the density of the chloride relative to hydrogen is 162.5, find the molecular formula of the chloride. [M = 56, Cl = 35.5]
Advertisements
उत्तर
Given, density of chloride relative to hydrogen = 162.5
Percentage of chlorine = 65.5‰
Percentage of Metal M = 100 - 65.5 = 34.5‰
| Element | Atomic mass | Percentage | Relative number of moles | Simplest mole ratio | Whole number ratio |
| M | 56 | 34.5 | 34.5/56 = 0.62 | 0.62/0.62 = 1 | 1 |
| Cl | 35.5 | 65.5 | 65.5/35.5 =1.85 | 1.85/0.62 = 2.98 | 3 |
Empirical formula = MCl3
Empirical formula mass = 56 + 3 x 35.5 = 162.5
Molecular mass = 2 x Vapour density = 2 x 162.5 = 325
n = Molecular mass / Empirical formula mass
= 325/162.5 = 2
Molecular formula = n x empirical formula
= 2 X MCl3 = M2Cl6
APPEARS IN
संबंधित प्रश्न
Prove the Following :
2 X V.D. = Molecular mass.
What is the mass of nitrogen in 1000Kg of urea [CO(NH2)2] ?
[H = 1, C= 12, N= 14, O = 16]
Water can split into hydrogen and oxygen under suitable conditions. The equations representing the change is: 2H2O(I) → 2H2 (g) + O2(g)
Ammonia burns in oxygen and the combustion in the presence of a catalyst may be represented as:
2NH3 (g) +21/2O2 (g) → 2NO (g) + 3H2O (I)
What mass of steam is produced when 1.5 g of nitrogen monoxide is formed?
Give one word or phrase for the following:
Formation of ions from molecules.
Give two tests of the following:
Oxygen
Calculate the number of hydrogen atoms in 0.1 mole of H2SO4.
Calculate the mass of nitrogen supplied to soil by 5 kg of urea [CO(NH2)2].
[O = 16; N = 14; C = 12; H = 1]
The atomic mass of Chlorine is 35.5. What is its vapour density?
Ammonia burns in oxygen and the combustion, in the presence of a catalyst, may be represented by;
\[\ce{2NH3 + 2 1/2O2 -> 2NO + 3H2O}\] [H = 1, N = 14, O = 16]
What mass of steam is produced when 1.5 g of nitrogen monoxide is formed?
67.2 litres of hydrogen combines with 44.8 litres of nitrogen to form ammonia under specific conditions as:
\[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\]
Calculate the volume of ammonia produced. What is the other substance, if any, that remains in the resultant mixture?
