Question

Combustion of a 0.9827-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.878 g of CO2 and 1.153 g of H2O. What is the empirical formula of the compound ?

Answer 1

Answer:

The correct answer is , The empirical formula  of the compound is C4H11O

Explanation:

Given: Combustion of a 0.9827-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.878 g of CO2 and 1.153 g of H2O.

To find: What is the empirical formula of the compound

Calculation:

we have to calculate the masses of

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

Mass of Carbon,

=1.900g CO2×12.01 g C/44.01g$C_{2}O$

= 0.5185 g C

Mass of Hydrogen,

=1.070g $H_{2}O$×2.016 g H/18.02g $H_{2}O$

=0.1197 g H

Mass of Carbon + Mass of Hydrogen

=0.5185 g + 0.1197 g

= 0.6382 g

There will be fewer than the sample's mass.

And the lost mass must be the result of

Mass of Oxygen,

= 0.9827 g - 0.6382 g

= 0.3445 g

Therefore, the empirical formula of the compound is 0.3445g.

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