5.6g of organic compound on burning with exess oxygen gave 17.6g of CO2 and 7.2g of H2O .the organic compound

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To determine the organic compound, we need to calculate the empirical formula. The empirical formula represents the simplest whole-number ratio of the elements in a compound.

First, let's calculate the number of moles of carbon dioxide (CO2) and water (H2O) produced.

For CO2:
- Mass of CO2 produced = 17.6g
- Molar mass of CO2 = 12.01g/mol (carbon) + 2 * 16.00g/mol (oxygen) = 44.01g/mol

Number of moles of CO2 = Mass of CO2 produced / Molar mass of CO2
Number of moles of CO2 = 17.6g / 44.01g/mol

Next, let's calculate the number of moles of water (H2O):
- Mass of H2O produced = 7.2g
- Molar mass of H2O = 1.01g/mol (hydrogen) + 16.00g/mol (oxygen) = 18.01g/mol

Number of moles of H2O = Mass of H2O produced / Molar mass of H2O
Number of moles of H2O = 7.2g / 18.01g/mol

Now, let's determine the number of moles of carbon (C) and hydrogen (H) in the organic compound:

Number of moles of C = Number of moles of CO2 (since there is 1 carbon atom in 1 molecule of CO2)
Number of moles of H = Number of moles of H2O (since there are 2 hydrogen atoms in 1 molecule of H2O)

Finally, let's express the moles of C and H in the simplest whole-number ratio:

Divide the number of moles of C and H by the smaller value to get the empirical formula.

For example, if there are 2 moles of C and 4 moles of H:
Empirical formula = (2 moles of C / 2) : (4 moles of H / 2) = C1H2 = CH2

So, based on the given information, the empirical formula of the organic compound is CH2.