Advertisements
Advertisements
प्रश्न
Find the empirical formula of a compound containing 17.64% hydrogen and 82.35% of nitrogen.
Advertisements
उत्तर १
Given is the % of H n N
So atomic weight of H is 1
the atomic weight of N is 14
Divide % of H with its atomic weight. weight and similarly N % with its atomic weight I.e. 14
You will get the relative no of atoms.
to get the simplest ratio. Divide the smaller value of relative no of atoms with the two. you will get the simplest ratio
NH3
उत्तर २
| Element | Percentage | Atomic Weight | Ratio | Simplest Ratio |
| Hydrogen | 82.35% | 14 | `82.35/14` = 5.88 | `5.88/5.88` = 1 |
| Nitrogen | 17.64% | 1 | `17.46/1` = 17.46 | `17.46/5.88` = 3 |
∴ Empirical Formula= N1H3 = NH3
संबंधित प्रश्न
The equation for the burning of octane is:
\[\ce{2C8H18 + 25O2 -> 16CO2 + 18H2O}\]
What is the empirical formula of octane?
On analysis, a substance was found to contain:
C = 54.54%, H = 9.09%, O = 36.36%
The vapour density of the substance is 44, calculate its empirical formula.
An organic compound, whose vapour density is 45, has the following percentage composition,
H = 2.22%, O = 71.19% and remaining carbon. Calculate its empirical formula.
An organic compound contains H = 4.07%, Cl = 71.65% chlorine and remaining carbon. Its molar mass = 98.96. Find its Empirical formula.
Determine the formula of the organic compound if its molecule contains 12 atoms of carbon. The percentage compositions of hydrogen and oxygen are 6.48 and 51.42 respectively.
A compound X consists of 4.8% carbon and 95.2% bromine by mass. Determine the empirical formula of this compound working correctly to one decimal place (C = 12; Br = 80).
An experiment showed that in a lead chloride solution, 6.21 g of lead is combined with 4.26 g of chlorine. What is the empirical formula of this chlorine? (Pb = 207; Cl = 35.5)
The following experiment was performed in order to determine the formula of a hydrocarbon. The hydrocarbon X is purified by fractional distillation.
0.145 g of X was heated with dry copper (II) oxide and 224 cm3 of carbon dioxide was collected at S.T.P.
Calculate the empirical formula of X by the following step:
Calculate the mass of carbon contained in this quantity of carbon dioxide and thus the mass of carbon in sample X.
The following experiment was performed in order to determine the formula of a hydrocarbon. The hydrocarbon X is purified by fractional distillation.
0.145 g of X was heated with dry copper (II) oxide and 224 cm3 of carbon dioxide was collected at S.T.P.
Calculate the empirical formula of X by the following step:
Calculate the mass of hydrogen in sample X.
The following experiment was performed in order to determine the formula of a hydrocarbon. The hydrocarbon X is purified by fractional distillation.
0.145 g of X was heated with dry copper (II) oxide and 224 cm3 of carbon dioxide was collected at S.T.P.
Calculate the empirical formula of X by the following step:
Deduce the ratio of atoms of each element in X (empirical formula).
