Solid aluminum hydroxide reacts with nitric acid

Chapter 3 Problems

1. If 0.274 moles of a substance weighs 62.5 g, what is the molar mass of the substance, in units of g/mol?

2. Which of these quantities does not represent 1.00 mol of the indicated substance? A. 6.02 ( 1023 C atoms

B. 26.0 g Fe

C. 12.01 g C

D. 65.4 g Zn

E. 6.02 ( 1023 Fe atoms

3. How many silicon atoms are there in 1.00 g of silicon?

4. Determine the number of moles of aluminum in 96.7 g of Al.

5. What is the molar mass of acetaminophen, C8H9NO2?

6. What is the mass of 0.0250 mol of P2O5?

7. The molecular formula of aspirin is C9H8O4. How many aspirin molecules are present in one 500-milligram tablet?

8. How many moles is 25.7 g of CaSO4?

9. What is the mass of 8.25 ( 1019 UF6 molecules?

10. Calculate the percent composition by mass of all elements in Na2CO3.

11. What is the empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine?

12. The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The molar mass of this compound is 284.5 g/mol. What is the molecular formula of the compound?

13. Balance the following equation with the smallest set of whole numbers. ___ Na + ___ H2O ( ___ NaOH + ___ H2

14. Balance the following equation with the smallest set of whole numbers. __ C2H4 + __ O2 ( __ CO2 + __ H2O

15. Balance the following equation using the smallest set of whole numbers. ___ Al + ___ H2SO4 ( ___ Al2(SO4)3 + ___ H2

16. Aluminum hydroxide reacts with nitric acid to form aluminum nitrate and water. What mass of water can be formed by the reaction of 15.0 g of aluminum hydroxide with excess nitric acid?

Al(OH)3 + 3HNO3 ( Al(NO3)3 + 3H2O

17. Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ( 4NO + 6H2O When 40.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent? How many grams of NO are produced?

18. How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following chemical equation? MnO2 + 4HCl ( MnCl2 + Cl2 + 2H2O

19. Hydrochloric acid can be prepared by the following reaction: 2NaCl(s) + H2SO4(aq) ( 2HCl(g) + Na2SO4(s) How many grams of HCl can be prepared from 2.00 mol H2SO4 and 150 g NaCl?

20. Calculate the mass of SO3 that can be produced by the reaction of 90.0 g of SO2 and 100.0 g of O2. 2SO2 + O2 ( 2SO3

21. The first step in the Ostwald process for producing nitric acid is 4NH3(g) + 5O2(g) ( 4NO(g) + 6H2O(g). If the reaction of 150. g of ammonia with 150. g of oxygen gas yields 87. g of nitric oxide (NO), what is the percent yield of this reaction?

22. What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al2O3 + 3C ( 2Al + 3CO

22b. How many grams of the excess reagent remains?

23. Calculate the mass of FeS formed when 9.42 g of Fe reacts with 8.50 g of S. Fe(s) + S(s) ( FeS(s)

23b. How many grams of the excess reagent remains?