3. Chemical Reactions

What is the empirical formula of the compound given the combustion data: 2.08 g CO₂, 1.28 g H₂O, and 4.77 g SO₃?

A 45.2 mg sample of phosphorus reacts with selenium to form 131.6 mg of the selenide. Determine the empirical formula of phosphorus selenide.

A compound consists of 36.33% carbon, 6.11% hydrogen, 21.20% nitrogen, and 36.31% oxygen. What is the empirical formula for this compound?

A compound containing nitrogen and oxygen is decomposed in the laboratory and produces 1.78 g of nitrogen and 4.05 g of oxygen. Calculate the empirical formula of the compound.

A compound contains 15.94% boron, with the remainder being fluorine. What is the empirical formula of the compound?

A hydrocarbon produced 0.0100 mol of carbon and 0.0150 mol of hydrogen during combustion. What is the empirical formula of the hydrocarbon?

A metal (M) forms an oxide with the formula M2O. Identify the metal if the oxide is 16.99% O by mass.

A sample of an unknown compound was decomposed and found to be composed of 1.36 mol of oxygen, 4.10 mol of hydrogen, and 2.05 mol of carbon. What is the empirical formula of the unknown compound?

An unknown compound contains only carbon, hydrogen, and chlorine. Using combustion analysis, you burned 22.56 mg of the sample and collected 7.11 mg of H2O and 52.93 mg of CO2. What is the empirical formula of this compound?

An unknown compound contains only carbon, hydrogen, and oxygen. Using combustion analysis, you burned 19.31 mg of the sample and collected 17.96 mg of H2O and 43.89 mg of CO2. What is the empirical formula of this compound?

Determine the empirical formula of a compound that is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen.

Which of the following methods can be used to determine the empirical formula of zinc oxide?

If 0.500 mol of copper combines with 0.250 mol of sulfur, what is the empirical formula of the copper sulfide product?

In an experiment, 10.0 g of sulfur and 10.0 g of oxygen react completely to form an oxide of sulfur. What is its empirical formula?

Upon combustion, a 0.8009 g sample of a compound containing only carbon, hydrogen, and oxygen produces 1.6004 g CO2 and 0.6551 g H2O. What is the empirical formula of the compound?