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What is the empirical formula of a compound that contains 4.03 g of hydrogen per mole, 64.14 g of sulfur per mole, and 128.00 g of oxygen per mole?

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Answer:

Oct 27, 2015 · CH_4 For this kind of problem, you can assume that the weight of the unknown sample is 100g ( since 75% C + 25% H = 100%). Thus, weight of C = 75g weight of H = 25g Since chemical formulas deal with number of moles rather than weight in grams, you need to convert each element by multiplying it to their respective atomic masses.

Explanation:

Ritmeks

The empirical formular i H₂SO₄

The first step is to calculate the compound by the molar mass

Hydrogen,   Sulphur,   Oxygen

4.03/1   ,   64.14/32   ,   128/16

4.03  , 2  ,   8

Divide by the lowest value

4.03/2  ,  2/2 ,  8/2

2, 1 , 4

H₂SO₄

Hence the empirical formula is H₂SO₄

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