- 1(current)
Q. No.
In an iron oxide, the mass percent of iron and oxygen are 69.9 and 30.1, respectively. The empirical formula of the oxide of iron will be:
1. Fe3O2
2. Fe2O2
3. Fe2O3
4. Fe3O4
Subtopic: Empirical & Molecular Formula |
70%
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The average atomic mass of chlorine using the following data would be:
| Isotope |
% Natural Abundance |
Molar Mass |
| 35Cl | 75.77 | 34.9689 |
| 37Cl | 24.23 | 36.9659 |
1. 38.4527 u
2. 37.4527 u
3. 36.4527 u
4. 35.4527 u
Subtopic: Empirical & Molecular Formula |
77%
From NCERT
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The molar mass of naturally occurring Argon isotopes is:
| Isotope | Isotopic molar mass | Abundance |
| 36-Ar | 35.96755 g mol–1 | 0.337% |
| 38-Ar | 37.96272 g mol–1 | 0.063% |
| 40-Ar | 39.9624 g mol–1 | 99.600% |
| 1. | 49.99947 g mol-1 | 2. | 39.99947 g mol-1 |
| 3. | 35.59947 g mol-1 | 4. | 45.59947 g mol-1 |
Subtopic: Empirical & Molecular Formula |
81%
From NCERT
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Burning a small sample of welding gas (constituted of C and H only) in oxygen gives 3.38 g carbon dioxide, 0.690 g of water, and no other products. A volume of 10.0 L (measured at STP) of this welding gas is found to weigh 11.6 g. Molecular formula of welding gas would be:
1. C2H2
2. C2H6
3. CH
4. C2H4
Subtopic: Empirical & Molecular Formula |
57%
From NCERT
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Q. No.
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