Combustion of 28.30 g of a compound containing only carbon, hydrogen, and oxygen produces 32.75 gco2 and 13.41 gh2o. what is the empirical formula of the compound?

The empirical formula is C₂H₄O₃.

We must calculate the masses of C, H, and O from the masses given.

Mass of C = 32.75 g CO₂ × (12.01 g C/44.01 g CO₂) = 8.9372 g C

Mass of H = 13.4 g H₂O × (2.016 H/18.02 g H₂O) = 1.5067 g H

Mass of O = Mass of compound - Mass of C - Mass of H

                  = (28.30 – 8.9372 – 1.5067) g = 17.856 g

Now, we must convert these masses to moles and find their ratios. If the ratios are not integers, we multiply them by a number to make them close to integers.

From here on, I like to summarize the calculations in a table.

Element       m/g       n/mol     Ratio        ×2      Integers  

     C           8.9372   0.74415   1               2                  2

     H           1.5067    1.4948    2.0086    4.0174          4

     O        17.856       1.1160      1.4997     2.9994         3

The empirical formula is C₂H₄O₃.

answer: at room temperature (roughly 20 degrees c), you can dissolve 203.9 grams (or 200 grams) of sugar in 100 ml of water. as water temperature increases, the amount of sugar that will dissolve increases, up to about 500 grams of sugar in 100 ml water at 100 degrees c.

explanation:

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: