Calculate the mass percent composition of nitrogen in each nitrogen-containing compound. c. NO₂

Most fertilizers consist of nitrogen-containing compounds such as NH₃, CO(NH₂)₂, NH₄NO₃, and (NH₄)₂SO₄. Plants use the nitrogen content in these compounds for protein synthesis. Calculate the mass percent composition of nitrogen in CO(NH₂)₂.

Iron in the earth is in the form of iron ore. Common ores include Fe₂O₃ (hematite), Fe₃O₄ (magnetite), and FeCO₃ (siderite). Calculate the mass percent composition of iron for each of these iron ores. Which ore has the highest iron content?

Copper(II) fluoride contains 37.42% F by mass. Calculate the mass of fluorine (in g) in 55.5 g of copper(II) fluoride.

Silver chloride, often used in silver plating, contains 75.27% Ag by mass. Calculate the mass of silver chloride required to plate 155 mg of pure silver.

The iodide ion is a dietary mineral essential to good nutrition. In countries where potassium iodide is added to salt, iodine deficiency (or goiter) has been almost completely eliminated. The recommended daily allowance (RDA) for iodine is 150 mg/day. How much potassium iodide (76.45% I) should you consume if you want to meet the RDA?

The American Dental Association recommends that an adult female should consume 3.0 mg of fluoride (F^-) per day to prevent tooth decay. If the fluoride is consumed in the form of sodium fluoride (45.24% F), what amount of sodium fluoride contains the recommended amount of fluoride?

Write a ratio showing the relationship between the molar amounts of each element for each compound. (See Appendix IIA for color codes.) (a)

Determine the number of moles of hydrogen atoms in each sample. a. 0.0885 mol C₄H₁₀ b. 1.3 mol CH₄

Determine the number of moles of hydrogen atoms in each sample. c. 2.4 mol C₆H₁₂

Determine the number of moles of hydrogen atoms in each sample. d. 1.87 mol C₈H₁₈

Determine the number of moles of oxygen atoms in each sample. a. 4.88 mol H₂O₂ b. 2.15 mol N₂O c. 0.0237 mol H₂CO₃ d. 24.1 mol CO₂

Calculate mass (in grams) of sodium in 8.5 g of each sodium containing food additive. a. NaCl (table salt) b. Na₃PO₄ (sodium phosphate) c. NaC₇H₅O₂ (sodium benzoate) d. Na₂C₆H₆O₇ (sodium hydrogen citrate)

Calculate the mass (in kilograms) of chlorine in 25 kg of each chlorofluorocarbon (CFC). a. CF₂Cl₂ c. C₂F₃Cl₃ d. CF₃Cl

Calculate the mass (in kilograms) of chlorine in 25 kg of each chlorofluorocarbon (CFC). b. CFCl₃

How many fluorine atoms are present in 5.85 g of C₂F₄?

How many bromine atoms are present in 35.2 g of CH₂Br₂?

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. a. 1.245 g Ni, 5.381 g I

Write a ratio showing the relationship between the molar amounts of each element for each compound. (See Appendix IIA for color codes.) (b)

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. b. 2.677 g Ba, 3.115 g Br

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. c. 2.128 g Be, 7.557 g S, 15.107 g O

Calculate the empirical formula for each stimulant based on its elemental mass percent composition.

a. nicotine (found in tobacco leaves): C 74.03%, H 8.70%, N 17.27%

b. caffeine (found in coffee beans): C 49.48%, H 5.19%, N 28.85%, O 16.48%

Calculate the empirical formula for each natural flavor based on its elemental mass percent composition. a. methyl butyrate (component of apple taste and smell): C 58.80%, H 9.87%, O 31.33%

Calculate the empirical formula for each natural flavor based on its elemental mass percent composition. b. vanillin (responsible for the taste and smell of vanilla): C 63.15%, H 5.30%, O 31.55%

The elemental mass percent composition of ibuprofen (a nonsteroidal anti-inflammatory drug [NSAID]) is 75.69% C, 8.80% H, and 15.51% O. Determine the empirical formula of ibuprofen.

The elemental mass percent composition of ascorbic acid (vitamin C) is 40.92% C, 4.58% H, and 54.50% O. Determine the empirical formula of ascorbic acid.

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.

From the given empirical formula and molar mass, find the molecular formula of each compound. a. C₆H₇N, 186.24 g/mol

From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. a. C₄H₉, 114.22 g/mol