A2.20 g sample of a compound gave 5.63 g co2 and 2.30 g h2o on combustion in air. the compound is known to contain only c, h, o. what is its simplest formula?

The simplest formula is C₅H₁₀O.

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

Mass of C =5.63 g CO₂ × (12.01 g C/44.01 g CO₂) = 1.536 g C

Mass of H = 2.30 g H₂O × (2.016 g H/18.02 g H₂O) = 0.2573 g H

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

= (2.20 – 1.536 – 0.2573) g = 0.406 g

Now, we must convert these masses to moles and find their ratios.

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

Element  Mass/g    Moles     Ratio    Integers

     C         1.536     0.1279     5.038        5

     H       0.2573    0.2553  10.05         10

     O       0.406      0.0254    1                 1

The empirical formula is C₅H₁₀O.

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.