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 |
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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 |
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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 |
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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 |
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