Advertisements
Advertisements
प्रश्न
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.
Advertisements
उत्तर
| Element | Percentage | Atomic Weight | Ratio | Simplest Ratio |
| C | 54.54 | 12 | `54.54/12` = 4.54 | `4.54/2.27` = 2 |
| H | 9.09 | 1 | `9.09/1` = 9.09 | `9.09/2.27` = 4 |
| O | 36.36 | 16 | `36.36/16` = 2.27 | `2.27/2.27` = 1 |
So, its empirical formula = C2H4O
APPEARS IN
संबंधित प्रश्न
The equation for the burning of octane is:
\[\ce{2C8H18 + 25O2 -> 16CO2 + 18H2O}\]
What is the empirical formula of octane?
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.
A hydrocarbon contains 4.8g of carbon per gram of hydrogen. Calculate:
find the 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.
10.47 g of a compound contained 6.25 g of metal A and rest non-metal B. Calculate the empirical formula of the compound [At. wt of A = 207, B = 35.5]
A hydride of nitrogen contains 87.5% percent by mass of nitrogen. Determine the empirical formula of this compound.
Find the empirical formula of a compound containing 17.64% hydrogen and 82.35% of nitrogen.
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.
