Molar Mass and Empirical Formulas

The video tutorial explains how to calculate the empirical and molecular formulas of a compound based on its percent composition by mass. It covers converting mass to moles, determining mole ratios, and using these ratios to find the empirical formula. The tutorial then shows how to calculate the molecular formula using the molar mass. The video concludes with additional resources for further learning.

What is the percent composition of sulfur in the compound?

• 6.21%

• 39.5%

• 44.4%

• 9.86%

Which element has the highest percent composition by mass in the compound?

• Carbon

• Hydrogen

• Sulfur

• Oxygen

What is the molar mass of carbon used in the conversion to moles?

• 16.00 g/mol

• 32.07 g/mol

• 12.01 g/mol

• 1.01 g/mol

How many moles of hydrogen are present in the compound?

• 0.616 moles

• 1.232 moles

• 6.149 moles

• 3.697 moles

What is the smallest mole ratio used to calculate the empirical formula?

• 3.697

• 6.149

• 1.232

• 0.616

What is the empirical formula of the compound?

• C6H12O6

• C6H10S2O

• CH4

• C2H5OH

What is the molar mass of the empirical formula C6H10S2O?

• 58.4 g/mol

• 98.1 g/mol

• 180.2 g/mol

• 162.3 g/mol

How does the molar mass of the empirical formula compare to the given molar mass of the molecular formula?

• It is higher

• It is double

• It is approximately the same

• It is lower

What is the molecular formula of the compound?

• C2H4O2

• C6H10S2O

• C12H20S4O2

• C3H5SO

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