Advertisements
Advertisements
प्रश्न
A compound is formed by 24 g of X and 64 g of oxygen. If the atomic mass of X = 12 and O = 16, calculate the simplest formula of the compound.
Advertisements
उत्तर
Mass of X in the given compound =24 g
Mass of oxygen in the given compound =64 g
So total mass of the compound =24 + 64 = 88 g
% of X in the compound = `24/88 xx100` = 27.3%
% of oxygen in the compound = `64/88 xx100` =72.7%
| Element | %age | Atomic weight | Atomic ratio | Simplest ratio |
| X | 27.3 | 12 | `27.3/12` = 2.27 | `2.27/2.27` = 1 |
| O | 72.7 | 16 | `72.7/16` = 4.54 | `4.54/2.27` = 2 |
So, simplest formula of the compound = XO2
APPEARS IN
संबंधित प्रश्न
Ethane burns in oxygen to form CO2 and H2O according to the equation:
\[\ce{2C2H6 + 7O2 -> 4CO2 + 6H2O}\]
If 1250 cc of oxygen is burnt with 300 cc of ethane, calculate:
- the volume of CO2 formed.
- the volume of unused O2.
Give the appropriate term defined by the statements given below :
The formula that represents the simplest ratio of the various elements present in one molecule of the compound.
Give the empirical formula of: C6H12O6
The empirical formula of a compound is C2H5. Its vapour density is 29. Determine the relative molecular mass of the compound and hence its molecular formula.
Calculate the percentage of water of crystallization in CuSO4. 5H2O
(H = 1, O = 16, S = 32, Cu = 64)
A compound of X and Y has the empirical formula XY2. Its vapour density is equal to its empirical formula weight. Determine its molecular formula.
Explain the term empirical formula.
0.2 g atom of silicon combine with 21.3 g of chlorine. Find the empirical formula of the compound formed.
Silicon (Si = 28) forms a compound with chlorine (Cl = 35.5) in which 5.6 g of silicon combines with 21.3 g of chlorine. Calculate the empirical formula of the compound.
- A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correctly to 1 decimal place. (H = 1; C = 12; Cl = 35.5)
- The relative molecular mass of this compound is 168, so what is its molecular formula?
- By what type of reaction could this compound be obtained from ethyne?
