From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. b. CCl, 284.77 g/mol

From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. c. C₃H₂N, 312.29 g/mol

Combustion analysis of a hydrocarbon produces 33.01 g CO₂ and 13.51 g H₂O. Calculate the empirical formula of the hydrocarbon.

Combustion analysis of naphthalene, a hydrocarbon used in mothballs, produces 8.80 g CO₂ and 1.44 g H₂O. Calculate the empirical formula of naphthalene.

The foul odor of rancid butter is due largely to butyric acid, a compound containing carbon, hydrogen, and oxygen. Combustion analysis of a 4.30-g sample of butyric acid produces 8.59 g CO₂ and 3.52 g H₂O. Determine the empirical formula of butyric acid.

Tartaric acid is the white, powdery substance that coats tart candies such as Sour Patch Kids. Combustion analysis of a 12.01-g sample of tartaric acid—which contains only carbon, hydrogen, and oxygen—produces 14.08 g CO₂ and 4.32 g H₂O. Determine the empirical formula of tartaric acid.

Classify each hydrocarbon as an alkane, alkene, or alkyne. a. H₂C=CH−CH₃ b. H₃C−CH₂−CH₃ c. HC≡C−CH₃ d. H₃C−CH₂−CH₂−CH₃

Classify each hydrocarbon as an alkane, alkene, or alkyne. a. HC≡CH

How many molecules of ethanol (C₂H₅OH) (the alcohol in alcoholic beverages) are present in 145 mL of ethanol? The density of ethanol is 0.789 g/cm³.

A drop of water has a volume of approximately 0.05 mL. How many water molecules does it contain? The density of water is 1.0 g/cm³.

Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. a. potassium chromate b. lead(II) phosphate

Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. c. sulfurous acid

Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. d. cobalt(II) bromide

Determine the chemical formula of each compound and then use it to calculate the mass percent composition of each constituent element. c. nitrogen triiodide

A Freon leak in the air-conditioning system of an old car releases 25 g of CF₂Cl₂ per month. What mass of chlorine does this car emit into the atmosphere each year?

A metal (M) forms a compound with the formula MCl₃. If the compound contains 65.57% Cl by mass, what is the identity of the metal?

A metal (M) forms an oxide with the formula M₂O. If the oxide contains 16.99% O by mass, what is the identity of the metal?

Fructose is a common sugar found in fruit. Elemental analysis of fructose gives the following mass percent composition: C 40.00%, H 6.72%, O 53.28%. The molar mass of fructose is 180.16 g/mol. Find the molecular formula of fructose.

Combustion analysis of a 13.42-g sample of equilin (which contains only carbon, hydrogen, and oxygen) produces 39.61 g CO₂ and 9.01 g H₂O. The molar mass of equilin is 268.34 g/mol. Find its molecular formula.

Estrone, which contains only carbon, hydrogen, and oxygen, is a female sexual hormone in the urine of pregnant women. Combustion analysis of a 1.893-g sample of estrone produces 5.545 g of CO₂ and 1.388 g H₂O. The molar mass of estrone is 270.36 g/mol. Find its molecular formula.

A hydrate of copper(II) chloride has the following formula: CuCl₂ • x H₂O. The water in a 3.41-g sample of the hydrate is driven off by heating. The remaining sample has a mass of 2.69 g. Find the number of waters of hydration (x) in the hydrate.

A compound of molar mass 177 g/mol contains only carbon, hydrogen, bromine, and oxygen. Analysis reveals that the compound contains eight times as much carbon as hydrogen by mass. Find the molecular formula.

Researchers obtained the following data from experiments to find the molecular formula of benzocaine, a local anesthetic, which contains only carbon, hydrogen, nitrogen, and oxygen. Complete combustion of a 3.54-g sample of benzocaine with excess O₂ forms 8.49 g of CO₂ and 2.14 g H₂O. Another 2.35-g sample contains 0.199 g of N. The molar mass of benzocaine is 165 g/mol. Find the molar formula of benzocaine.

Find the total number of atoms in a sample of cocaine hydrochloride, C₁₇H₂₂ClNO₄, of mass 23.5 mg.