Advertisements
Advertisements
प्रश्न
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]
Advertisements
उत्तर
Given: Weight of the compound: 10.47g
Weight of metal A = 6.25g
Weight of non-metal B = 10.47 – 6.25 = 4.22g
|
Element |
mass |
At. Wt. |
Relative no. of atoms |
Simplest ratio |
|
A |
6.25 |
207 |
`6.25/207` = 0.03 |
`0.03/0.03` = 1 |
|
B |
4.22 |
35.5 |
`4.26/35.5` = 0.12 |
`0.12/0.03` = 4 |
Hence, the empirical formula is AB4
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.
An organic compound contains H = 4.07%, Cl = 71.65% chlorine and remaining carbon. Its molar mass = 98.96. Find its Empirical formula.
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).
The percentage composition of sodium phosphate as determined by analysis is 42.1% sodium, 18.9% phosphorus and 39% oxygen. Find the empirical formula of the compound.
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 number of moles of carbon dioxide gas.
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.
