A compound is found to be 30.45% nitrogen (N) and 69.55% oxygen (O) by mass. If 1.63 g of this compound occupy 389 mL at 0.00°C and 775 mm Hg, what is the empirical formula of the compound?

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?