Citric acid was found to contain 37.51% C, 4.20% H, and 58.29% O by mass. What is the simplest formula for citric acid?

The mass percentages of H and O in a compound used for bleaching are 5.9% H and 94.1% O. The molar mass is 34g/mol. Calculate the molecular formula

A compound contains carbon and hydrogen only. A combustion analyzer collects 15.84 g of CO2 and 8.10 g of H2O.   Determine the empirical formula of the compound. What more information would you need to determine the molecular formula?

How many atoms are present in 123 g of sodium cyanide (cyanide = CN-)?     A sample contains 0.687 mol H3PO3. What is the mass of H3PO3in the sample?     A 2.000 g sample of Calcium sulfate dihydrate, CaSO42H2O (this is one molecule) contains 1.582 g CaSO4. How many moles of CaSO4 are there in this sample? Assuming that the rest of the sample is water, how many moles of H2O are there in the sample? How is the result consistent with the formula CaSO4·2H2O?

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?

A metal (M) forms an oxide with the formula M₂O. If the oxide contains 3.835% O by mass, what is the identity of the metal, M?

What volume of 1.772 M BaCl2 is needed to obtain 123 g of BaCl2?

2. What is the empirical formula for a compound containing 26.57% potassium, 35.36% chromium, and 38.07% oxygen?

Imagine you discover a substance in a forest mushroom and find through experimentation that it efficiently kills viruses but is not toxic to animal cells. You analyze its elemental composition to be: 70.08% C, 11.04% H, and remainder O by mass. What is the empirical formula of this interesting substance? Show full calculations.

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