A compound was analyzed and found to contain the following percent composition: 2.056% hydrogen, 32.69% S, and 65.26% oxygen. Calculate the empirical formula.

The empirical formula of a chemical compound is the simplest whole-number ratio of atoms present in a compound

The correct answer of the following is

The data is given as follows:-

We have to find the moles in the reaction.

The mas of the element is as follows:-

After solving the equation we get

Next, we divide each mole value by the smallest mole value (1.021)

The ratio of H to S to O is 2:1:4,

Hence, the empirical formula for H, S, and O is

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H2SO4

Explanation:

Firstly,

2.056% hydrogen = 2.056g of H

32.69% Sulphur = 32.69g of S

65.26% oxygen = 65.26g of O

Next, we convert each mass into moles by dividing by their respective molar mass:

H = 1, S = 32, O = 16

H = 2.056/1 = 2.056mol

S = 32.69/32 = 1.021mol

O = 65.26/16 = 4.078mol

Next, we divide each mole value by the smallest mole value (1.021)

H = 2.056/1.021 = 2.01

S = 1.021/1.021 = 1

O = 4.078/1.021 = 3.99

Approximately the ratio of H to S to O is 2:1:4, hence, the empirical formula for H, S and O is H2SO4.

what is the volume occupied by 40 grams of argon gas (ar) at standard conditions? what volume, in liters, is occupied by 1.5 x 1023 

explanation: