Question

Combustion of a 0.9827 g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of H2O. What is the empirical formula of the compound?

Answer 1

The empirical formula is

C4H11O

Explanation:

Main we have to calculate the masses of

given C and H from the masses of their oxides (CO2 and H2O).

Mass of C

=1.900g CO2×12.01 g C/44.01g CO2

= 0.5185 g C

Mass of H

=1.070g H2O×2.016 g H/18.02g H2O

=0.1197 g H

Mass of C + Mass of H

=0.5185 g + 0.1197 g

= 0.6382 g

There will be less than the mass of the sample.

And will be missing mass must be caused by

Mass of O

= 0.9827 g - 0.6382 g

= 0.3445 g

Answer 2

Answer:

The empirical formula is C4H 11O2 .