1. Write formulas for the following compounds and determine the percentage composition of each: a. nitric acid b. ammonia c. mercury(II) sulfate d. antimony(V)…

  1. Write formulas for the following compounds and determine the percentage composition of each:

a. nitric acid

b. ammonia

c. mercury(II) sulfate

d. antimony(V) fluoride

  2. Calculate the percentage composition of the following compounds:

a. lithium bromide, LiBr

b. anthracene, C₁₄H₁₀

c. ammonium nitrate, NH₄NO₃

d. nitrous acid, HNO₂

e. silver sulfide, Ag₂S

f.  iron(II) thiocyanate, Fe(SCN)₂

g. lithium acetate

h. nickel(II) formate

  3. Calculate the percentage of the given element in each of the following compounds:

a. nitrogen in urea, NH₂CONH₂

b. sulfur in sulfuryl chloride, SO₂Cl₂

c. thallium in thallium(III) oxide, Tl₂O₃

d. oxygen in potassium chlorate, KClO₃

e. bromine in calcium bromide, CaBr₂

f.  tin in tin(IV) oxide, SnO₂

  4. Calculate the mass of the given element in each of the following quantities:

a. oxygen in 4.00 g of manganese dioxide, MnO₂

b. aluminum in 50.0 metric tons of aluminum oxide, Al₂O₃

c. silver in 325 g silver cyanide, AgCN

d. gold in 0.780 g of gold(III) selenide, Au₂Se₃

e. selenium in 683 g sodium selenite, Na₂SeO₃

f.  chlorine in 5.0 ´ 10⁴ g of 1,1-dichloropropane, CHCl₂CH₂CH₃

  5. Calculate the percentage of water in each of the following hydrates:

a. strontium chloride hexahydrate, SrCl₂ × 6H₂O

b. zinc sulfate heptahydrate, ZnSO₄ × 7H₂O

c. calcium fluorophosphate dihydrate, CaFPO₃ × 2H₂O

d. beryllium nitrate trihydrate, Be(NO₃)₂ × 3H₂O

  6. Calculate the percentage of the given element in each of the following hydrates. You must first determine the formulas of the hydrates.

a. nickel in nickel(II) acetate tetrahydrate

b. chromium in sodium chromate tetrahydrate

c. cerium in cerium(IV) sulfate tetrahydrate

  7. Cinnabar is a mineral that is mined in order to produce mercury. Cinnabar is mercury(II) sulfide, HgS. What mass of mercury can be obtained from 50.0 kg of cinnabar?

  8. The minerals malachite, Cu₂(OH)₂CO₃, and chalcopyrite, CuFeS₂, can be mined to obtain copper metal. How much copper could be obtained from
1.00 ´ 10³ kg of each? Which of the two has the greater copper content?

  9. Calculate the percentage of the given element in each of the following hydrates:

a. vanadium in vanadium oxysulfate dihydrate, VOSO₄ × 2H₂O

b. tin in potassium stannate trihydrate, K₂SnO₃ × 3H₂O

c. chlorine in calcium chlorate dihydrate, CaClO₃ × 2H₂O

10. Heating copper sulfate pentahydrate will evaporate the water from the crystals, leaving anhydrous copper sulfate, a white powder. Anhydrous means “without water.” What mass of anhydrous CuSO₄ would be produced by heating
500.0 g of CuSO₄ × 5H₂O?

11. Silver metal may be precipitated from a solution of silver nitrate by placing a copper strip into the solution. What mass of AgNO₃ would you dissolve in water in order to get 1.00 g of silver?

12. A sample of Ag₂S has a mass of 62.4 g. What mass of each element could be obtained by decomposing this sample?

13. A quantity of epsom salts, magnesium sulfate heptahydrate, MgSO₄ × 7H₂O, is heated until all the water is driven off. The sample loses 11.8 g in the process. What was the mass of the original sample?

14. The process of manufacturing sulfuric acid begins with the burning of sulfur. What mass of sulfur would have to be burned in order to produce 1.00 kg of H₂SO₄? Assume that all of the sulfur ends up in the sulfuric acid.