A small crystal has a mass of 7.03 mg

1. A small crystal has a mass of 7.03 mg and is shaped like a cylinder with a height of 5.17 in and a radius of 34.8 mm. What is the density of the solid in g/cm³?

 

2. If the price of gasoline is $2.03 dollars/gal, what is its price in Euros per liter, given the exchange rate is $1.20 per Euro.

 

3. Convert 316.25 K into ^o Convert 14.7 ^oC into ^oF.

 

4. Provide the names for the following compounds

 

1. NaF
2. N₂O₄
3. KNO₃
4. MgSO₄
5. NH₃
6. Cr(NO₂)

 

 

5. Provide formulas for the following compounds

 

1. Calcium iodide
2. Aluminum sulfide
3. Lithium carbonate
4. Lead (II) oxide
5. Manganese (II) dichromate

 

 

6. Name These Acids:
7. H₂S b. HF c. H₂CO₃                                                       d. HNO₂

 

7. Write formulas for the following acids:
8. Hydroiodic acid b. Hydrophosphoric acid c. Nitric acid                                    d. Chromic acid
9. How many neon atoms are there in 2.585 mol of neon?
10. What is the mass in grams of 0.2338 mol of Titanium?
11. How many moles of barium are there in 42.9g of barium?
12. Molar mass of Copper (II) Nitrate = ___________________g/mole
13. Balancing Equations
14. a) ____ Na₃PO₄ + ____ Ba(OH)₂ à ____ NaOH + ____ Ba₃(PO₄)2

    b) ____ CaF₂ + ____ Li₂CO₃ à ____ CaCO₃ + ____ LiF

    c)         ____ Ba₃N₂ + ____ PtF₂ à ____ BaF₂ + ____ Pt₃N₂

15. Write chemical equations for the following reactions.
    a) Rubidium reacts with bromine to form Rubidium bromide.
16. b) Iron (II) sulfide and water vapor are formed when hydrogen sulfide and iron (II) hydroxide react.

    c) Calcium reacts violently with water to produce calcium hydroxide and hydrogen.

 

14. Stoichiometry

15. If 2.98 moles of C are reacted with an excess of Cu₂O, what mass of CO would be produced?
16. If 43.6 g of Co(NO₃)₃ are reacted with an excess of (NH₄)₂S, how many moles of NH₄NO₃ would be produced?
17. If 19.6g of FeS is added to 44.8g of HCl and allowed to react, what is the theoretical yield of H₂S? If 6.20 g of H₂S were obtained in the lab, what is the percent yield?

 

1. 947 g of chromium (III) chloride combined with 1.13 g of copper (II) sulfate to produce 0.154 g of copper (II) chloride. What is the percent yield of this reaction?

2. Solutions and Solubility

Label the following compounds as soluble or insoluble in water:

 

1. NaCl
2. CaSO₄
3. AgNO₃
4. PbCl₂
5. Li₂S
6. MgCO₃

 

16. Calculate the molar concentration, M, of a solution of a sample with 0.271 moles in 55.0 L or solution.

 

17. Calculate the pH of a 0.543M HCl solution.

 

18. Write the net ionic equations for the following reactions. Be sure to show all physical states for reactants and products for each equation type:
19. ___KBr +    ___Pb(NO₃)₂             à     ___PbBr₂            +    ___KNO₃
    

 

1. ___Fe(C₂H₃O₂)₂ +    ___Li₂SO₄                 à     ___FeSO₄            +    ___LiC₂H₃O₂