Copper Odyssey Conversion I
Conversion I - Changing elemental copper to copper (II) nitrate.
Pre-lab Questions: (page one of your lab report)
1. Balance the following reaction.
____ Cu(s) + ____ HNO3(aq) ____ Cu(NO3)2(aq) + ____ NO2(g) + ____ H2O(l)
2. In Table format:
a. Correctly name all of the above compounds.
b. List at least ten physical and/or chemical propertiesfor each of the above compounds.
c. Draw the structural formulas for each of the above compounds.
Analysis Questions: (Day 1 Homework, page seven of your lab report)
1. What type of chemical reaction is Conversion I?
2. Define the following bond types: ionic, nonpolar covalent, and polar covalent.
3. Identify each Conversion I reactant and product as a formula unit, a nonpolar molecule, or a polar molecule.
4. Why does HNO3 contain one nitrate andCu(NO3)2 contain two nitrates?
5. What does the 6M signify in the expression 6M HNO3?
6. Calculate the molar mass of each reactant. Be sure your work in clearly labeled!
7. Using the initial measured mass of copper used in Conversion I, determine the moles of copper.
8. Calculate the number of atoms of copper in your sample.
9. Using the initial measured mass of copper used in Conversion I, determine the mass of NO2 produced.
10. Using the Ideal Gas Law formula, calculate the volume of NO2 produced at 27°C and 1.0atm.
11. Calculate the moles of 6M nitric acid used in Conversion I.
12. Why could you assume the density of nitric acid is the same as water?
13. Using the amount of nitric acid used in Conversion I,calculate the mass of NO2 produced.
14. Based on your answers in problem nine and thirteen, which reactant would you expect to be limiting? Why?
15. Write the compound formula of the brown gas formed.
16. Write the compound formula of the blue product.
17. Why did the bottle have to be put in the fume hood?
18. The copper metal disappeared during this reaction. What became of the copper atoms?
19. Make a list of everything in the liquid in the bottle at the end of reaction one.
20. Give the old-fashioned, Latin name for nitric acid.
21. Why did we bother to measure the initial mass of the copper wire?
22. Write the equilibrium expression, k, for ConversionI.Remember only gases and aqueous substances are written in the expression!
23. In which direction would the equilibrium shift, if more copper was added to the reaction?
24. What would have happened to the concentration of the Cu(NO3)2if more copper was added to the reaction?
25. What happens to the volume of the NO2 as it moves higher in the atmosphere?
26. Calculate thisnew volume of NO2if the pressure drops to 0.70atm and the temperature drops to -15°C (use the original temperature and pressure given in problem ten and the original volume calculated in problem ten).
27. Why did we use nitric acid rather than some other acid, like hydrochloric acid?
28. Fill in the blanks: In Conversion I, elemental copper was changed to copper (II) ______by the action of ______acid. The Roman numeral (II) stands for the ______on the copper. This value is ______because all metals ______electrons to become stable ______with ______valence electrons like the ______gases. In Conversion I, water and a toxic gas, called ______, were formed. This gas was brown in color and is the same gas that gives the brownish look to Los Angeles smog. Nitric acid is the only strong acid that will react with copper. The acid we used was not full strength, but had been diluted with water to a concentration of______. In this reaction, four ______of nitric acid were used for every one copper atom. A single nitric acid formula unit has ______atoms in it. The formula unit of copper (II) nitrate had ______atoms in it. While the nitrogen dioxide and the water molecules each have ______atoms in them.