A compound is 25.0% carbon, 8.4% hydrogen and 66.6% sulfur by mass. Put symbols in order of CHS. Enter the formula without subscripting the numbers, add no spaces. For example: C4H402. Its empirical formula is

The empirical formula of a compound is C8H5N3O5. The compound has a molar mass of 892.6 g/mol; determine the molecular formula.

An iron-containing compound is 20.1% Fe, 11.5% S, 63.3% O, and 5.1% H. What is the empirical formula for this compound? FegSO 19H25 Fe15S9O50H FeSO 11H14 FES2022H28

You are trying to determine the formula for hydrated CaSO4 and you found the following: Mass of hydrated compound (i.e. CaSO4ïXH2O) = 3.09 g Mass of product (i.e., CaSO4) = 2.43 g   What is the empirical formula of this hydrate?

a) Elemental analysis of an unknown sample shows its mass composition to be 49.45% carbon (C), 28.84% nitrogen (N), 16.46% oxygen (O) and 5.18% hydrogen (H). Using mass spectrometry, you determine that the molar mass of the compound is equal to 194.19 g/mol. What is the molecular formula of the unknown compound? b) We carry out combustion of C5H10O (molar mass = 86.13 g/mol) (its reaction with O2, to produce CO2 and H2O). What is the maximum mass of products obtained (CO2 (molar mass = 44.01 g/mol) and H2O (molar mass = 18.02g/mol)), if the reaction vessel contains 15.0 g of C5H10O and 1.00 mol of Oz.

A vial contains 4.17 x 1023 molecules of an unknown organic compound.  How many moles (3 sf) of this compound is present?  (Type "NO" in the box if you feel that you have not been given enough information to answer this question).

The composition of a compound was found to be 66.7% C, 25.9% N and 7.41% H by mass? What is the empirical formula for the compound? If the molar mass was determined to be 108.0 g, what is the molecular formula of this compound? In your answer, be sure to first state the empirical formula followed by the molecular formula.

A substance has the molecular formula C6H6O6 . What is its empirical formula? (Enter the elements in the order: C, H, 0.) Empirical formula:

A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68 mg of the compound yields 15.40 mg CO2 and 7.88 mg H2O. The molar mass of the compound is 122.1 g/mol. What are the empirical and molecular formulas of the compound?

C,d,e?