A 1.638 Gram pure sample of a compound containing only carbon hydrogen and oxygen was burned in excess oxygen gas 3.117 g of carbon dioxide and 1.911 g of water were produced find the empirical formula of the compound

C2H6O

Explanation:

First, find the masses of C, H, and O. I used ratios.

3.117g CO2  x  1 mol CO2/44.01g CO2  x  1 mol C/1 mol CO2  x  12.01g C/1 mol C = 0.850606 g C

1.911g H2O  x  1 mol H2O/18.016g H2O  x  2 mol H2O/1 mol H2O  x  1.008g H/1 mol H = 0.213842 g H

To find the mass of oxygen, just add the masses of C and H together and subtract that from the total mass of the sample.

1.638 - (0.850606 + 0.213842) = 0.57355 g O

Second, find the moles of C, H, and O.

0.850606g C  x  1 mol C/12.01g C = 0.070825 mol C

0.213842g H  x  1 mol H/1.008g H = 0.212145 mol H

0.57355 g O  x  1 mol O/16g O = 0.035847 mol O

Finally, divide the number of moles of each element by the smallest value of moles calculated. In this case, the smallest value is 0.035847.

0.070825/0.035847 = 2

0.212145/0.035847 = 6

0.035847/0.035847 = 1

one negative thing it that it can kill water animals. another negative thing is it can cause the destruction of ecosystem. one way water pollution can be reduced is to conserve energy.

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.