The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C₁₄H₁₈N₂O₅. (a) What is the molar mass of aspartame?

The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C₁₄H₁₈N₂O₅. (c) How many molecules of aspartame are present in 1.00 mg of aspartame?

The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet®, is C₁₄H₁₈N₂O₅. (d) How many hydrogen atoms are present in 1.00 mg of aspartame?

A sample of glucose, C₆H₁₂O₆, contains 1.250×10²¹ carbon atoms. (c) How many moles of glucose does it contain?

A sample of the male sex hormone testosterone, C₁₉H₂₈O₂, contains 3.88×10²¹ hydrogen atoms. (b) How many molecules of testosterone does it contain?

The allowable concentration level of vinyl chloride, C₂H₃Cl, in the atmosphere in a chemical plant is 2.0×10⁻⁶ g/L. How many moles of vinyl chloride in each liter does this represent?

At least 25 mg of tetrahydrocannabinol (THC), the active ingredient in marijuana, is required to produce intoxication. The molecular formula of THC is C₂₁H₃₀O₂. How many molecules?

Give the empirical formula of each of the following compounds if a sample contains a.0.0130 mol C, 0.0390 mol H, and 0.0065 mol O

Give the empirical formula of each of the following compounds if a sample contains b.11.66 g iron and 5.01 g oxygen

Determine the empirical formula of each of the following compounds if a sample contains b. 5.28 g Sn and 3.37 g F;

Determine the empirical formula of each of the following compounds if a sample contains c. 87.5% N and 12.5% H by mass.

Determine the empirical formulas of the compounds with the following compositions by mass: a. 55.3% K, 14.6% P, and 30.1% O

Determine the empirical formulas of the compounds with the following compositions by mass: c. 62.1% C, 5.21% H, 12.1% N, and the remainder O

A compound whose empirical formula is XF3 consists of 65% F by mass. What is the atomic mass of X?

The compound XCl4 contains 75.0% Cl by mass. What is the element X?

What is the molecular formula of each of the following compounds? (a) empirical formula CH, molar mass 5 78.0 g/mol (b) empirical formula NH₂Cl, molar mass = 51.5 g/mol

What is the molecular formula of each of the following compounds? (b) empirical formula C₂H₄O, molar mass = 88.0 g/mol

Determine the empirical and molecular formulas of each of the following substances: (a) Styrene, a compound used to make Styrofoam® cups and insulation, contains 92.3% C and 7.7% H by mass and has a molar mass of 104 g/mol.

Determine the empirical and molecular formulas of each of the following substances: (b) Caffeine, a stimulant found in coffee, contains 49.5% C, 5.15% H, 28.9% N, and 16.5% O by mass and has a molar mass of 195 g/mol.

Determine the empirical and molecular formulas of each of the following substances: (c) Monosodium glutamate (MSG), a flavor enhancer in certain foods, contains 35.51% C, 4.77% H, 37.85% O, 8.29% N, and 13.60% Na, and has a molar mass of 169 g/mol.

Determine the empirical and molecular formulas of each of the following substances: (a) Ibuprofen, a headache remedy, contains 75.69% C, 8.80% H, and 15.51% O by mass and has a molar mass of 206 g/mol.

Determine the empirical and molecular formulas of each of the following substances: (b) Cadaverine, a foul-smelling substance produced by the action of bacteria on meat, contains 58.55% C, 13.81% H, and 27.40% N by mass; its molar mass is 102.2 g/mol.

(a) Combustion analysis of toluene, a common organic solvent, gives 5.86 mg of CO₂ and 1.37 mg of H₂O. If the compound contains only carbon and hydrogen, what is its empirical formula?

(b) Menthol, the substance we can smell in mentholated cough drops, is composed of C, H, and O. A 0.1005-g sample of menthol is combusted, producing 0.2829 g of CO₂ and 0.1159 g of H₂O. What is the empirical formula for menthol? If menthol has a molar mass of 156 g/mol, what is its molecular formula?

(a) The characteristic odor of pineapple is due to ethyl butyrate, a compound containing carbon, hydrogen, and oxygen. Combustion of 2.78 mg of ethyl butyrate produces 6.32 mg of CO₂ and 2.58 mg of H₂O. What is the empirical formula of the compound?

Valproic acid, used to treat seizures and bipolar disorder, is composed of C, H, and O. A 0.165-g sample is combusted to produce 0.166 g of water and 0.403 g of carbon dioxide. What is the empirical formula for valproic acid?

Propenoic acid, C₃H₄O₂, is a reactive organic liquid that is used in the manufacturing of plastics, coatings, and adhesives. An unlabeled container is thought to contain this liquid. A 0.275-g sample of the liquid is combusted to produce 0.102 g of water and 0.374 g carbon dioxide. Is the unknown liquid propenoic acid? Support your reasoning with calculations.

Washing soda, a compound used to prepare hard water for washing laundry, is a hydrate, which means that a certain number of water molecules are included in the solid structure. Its formula can be written as Na2CO3 # xH2O, where x is the number of moles of H2O per mole of Na2CO3. When a 2.558-g sample of washing soda is heated at 125 C, all the water of hydration is lost, leaving 0.948 g of Na2CO3. What is the value of x?

Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as MgSO4 # xH2O, where x indicates the number of moles of H2O per mole of MgSO4. When 5.061 g of this hydrate is heated to 250 C, all the water of hydration is lost, leaving 2.472 g of MgSO4. What is the value of x?

Hydrofluoric acid, HF(aq), cannot be stored in glass bottles because compounds called silicates in the glass are attacked by the HF(aq). Sodium silicate (Na₂SiO₃), for example, reacts as follows: Na₂SiO₃(s) + 8 HF(aq) → H₂SiF₆(aq) + 2 NaF(aq) + 3 H₂O(l) (a) How many moles of HF are needed to react with 0.300 mol of Na₂SiO₃? (b) How many grams of NaF form when 0.500 mol of HF reacts with excess Na₂SiO₃? (c) How many grams of Na₂SiO₃ can react with 0.800 g of HF?