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A compound is 2. 00% H by mass, 32. 7% S by mass, and 65. 3% O by mass. What is its empirical formula? The final step is to use the mole ratios of the elements to write the empirical formula. The mole ratios of the elements are: mole ratio of H:S:O = 2:1:4 The mole ratios show the ratios of the elements in the compound. Use these ratios to identify the subscripts on each element in the empirical formula. Remember that the subscript 1 is not shown. What is the correct empirical formula for this compound? HSO H2S1O4 H2SO4.

Sagot :

Lanuel

The empirical formula of this compound is [tex]H_2SO_4[/tex]

Given the following data:

  • Percentage of H = 2.00%
  • Percentage of S = 32.7%
  • Percentage of O = 65.3%

Scientific data:

  • Molar mass of hydrogen (H) = 1.0 g/mol.
  • Molar mass of sulfur (S) = 32 g/mol.
  • Molar mass of oxygen (O) = 16 g/mol.

To determine the empirical formula of this compound:

Note: We would assume that the mass of the compound is 100 grams.

Hence, the mass of its constituent elements are:

  • Mass of hydrogen (H) = 2.00 grams
  • Mass of sulfur (S) = 32.7 grams
  • Mass of oxygen (O) = 65.3 grams

Next, we would determine the number of moles of each element by using this formula:

[tex]Number\;of\;moles = \frac{mass}{molar\;mass}[/tex]

For hydrogen (H):

[tex]Number\;of\;moles = \frac{2.00}{1}[/tex]

Number of moles = 2.0 moles

For sulfur (S):

[tex]Number\;of\;moles = \frac{32.7}{32}[/tex]

Number of moles = 1.0 moles

For oxygen (O):

[tex]Number\;of\;moles = \frac{65.3}{16}[/tex]

Number of moles = 4.0 moles

Empirical formula = [tex]H_2SO_4[/tex]

Read more: https://brainly.com/question/21280037

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