Question

An oxide of sulphur contain 66.67%sulphur what is its empirical formula.
ONLY DOO IT BY TABLE METHOD OF EMPIRICAL FORMULA )
ANSER IS S202
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Answer 1

By the end of this section, you will be able to:

Compute the percent composition of a compound

Determine the empirical formula of a compound

Determine the molecular formula of a compound

In the previous section, we discussed the relationship between the bulk mass of a substance and the number of atoms or molecules it contains (moles). Given the chemical formula of the substance, we were able to determine the amount of the substance (moles) from its mass, and vice versa. But what if the chemical formula of a substance is unknown? In this section, we will explore how to apply these very same principles in order to derive the chemical formulas of unknown substances from experimental mass measurements.

Answer 2

Given:

The percentage of sulphur = 66.67 %

To Find:

The empirical formula of the oxide.

Calculation:

- Let the mass of oxide be 100 gm.

⇒ The mass of sulphur = 66.67 gm

⇒ The mass of oxygen = 33.33 gm

- The no of moles of sulphur = 66.67/32 = 2.08

- The no of moles of oxygen = 33.33/16 = 2.08

⇒ S : O = 2.08 : 2.08

⇒ S : O = 1 : 1

- So, the empirical formula of the given oxide of sulphur is SO.

(Note: The empirical formula of SO and S2O2 is the same, i.e., SO.)