CHM 130
Instructor: ________________________ Name: ______________________________
Spring 2017
Homework III
Ch. 10-15
Due no later than Noon on Friday April 28th, 2017.
Show all your work, each step with units, for full credit for calculations.
1. Balance these reactions and indicate the type of reaction: Combination (C), Decomposition (D),
Combustion (CB), Acid Base (AB), Single Replacement (SR), or Double Replacement (DR).
a. Type=____
___ Zn(s) + ____Ag2SO4(aq)  ____Ag(s) + ____ZnSO4(aq)
b. Type=____
___Al(OH)3(aq) + ___HBr(aq)  ___H2O(l) + ___AlBr3(aq)
c. Type=____
___Fe2O3(s)  ___Fe(s) + ___O2(g)
d. Type=____
___Co(s) + __Cl2(g)  ___CoCl3(s)
2. Predict the products for the following reactions, indicate all states and balance.
a. ___NaCl(s) + ___Zn(s)  _____________________________________________
b. ___Cd(NO3)2(aq) + ___Al(s)  _________________________________________
c. ___H3PO4(aq) + ___Sr(OH)2(aq)  ________________________________________
d. ___Zn(C2H3O2)2(aq) + ___Na3PO4(aq)  _______________________________________
e. ___C6H6(l) + ___O2(g)  __________________________________________________
f.
___BaS(aq) + ___CaSO4(aq)  _____________________________________________
3. Write this aqueous reaction and balance: manganese(II) nitrate plus sodium chromate produces
manganese(II) chromate and sodium nitrate.
______________________________________________________________________________
4. Consider this reaction:
Mn(s) + SnCl2(aq)  MnCl2(aq) + Sn(s)
a. What is oxidized? _____________________ What is reduced? __________________
b. What is the reducing agent? ___________ What is the oxidizing agent? ______________
5. What is the Law of Conservation of Matter? __________________________________________
______________________________________________________________________________
6. Circle the following if they are soluble: CaCO3
Na3PO4
AgI
SrS
PbSO4
7. Describe three ways to increase the rate of a reaction:
a. _________________________________________________________________
b. __________________________________________________________________
c. __________________________________________________________________
8. True or False? You can stop a reaction at the transition state. ________________
9. True or False? Molecules must collide with each other in order to react. _____________
10. True or False? Molecules can be in any orientation to react. ________________
11. If I have 24.31 grams of magnesium, how many moles is this? ___________________
12. If I have 24.31 grams of magnesium, how many atoms is this? ____________________
13. What is the molar mass of barium phosphate? _____________________________g/mol
14. Draw an exothermic profile in this box:
Label TS, H, Ea,
15. If I have 2.45 x 1026 atoms of sulfur, how many moles is this?
16. If I have 45.2 moles of sodium nitride, how many grams is this?
17. If I have 26.9 grams of NaCl, how many moles is this?
18. How many atoms are in 78.3 grams of carbon?
19. How many liters at STP is 44.44 moles of carbon dioxide?
20. How many grams is 24.3 L of carbon dioxide at STP?
21. How many atoms are in 14.5 liters of nitrogen gas at STP? Be careful – think about nitrogen gas.
22. Calculate the percent composition for every element in barium nitrate.
23. Use this balanced reaction to answer these problems.
2 Al(s) + 6 HCl(aq)  2 AlCl3(aq) + 3 H2(g)
a. How many molecules of HCl are needed to react with 2 atoms of aluminum? _______
b. How many moles of hydrogen gas could be made from 6 moles of HCl? ________
c. How many moles of hydrogen gas would be produced from 5.55 moles of aluminum?
d. How many grams of HCl would be needed to produce 15.35 grams of AlCl3?
e. If 70.5 liters of hydrogen gas are produced, how many grams of Al reacted?
24. Calculate the mass of mercury produced when 3.45 grams of mercury(II) oxide decomposes?
Given: 2 HgO(s)  2 Hg(l) + O2(g)
25. Name the four intermolecular forces we studied:
a. __________________________________ c. ___________________________
b. __________________________________ d. ____________________________
26. Which IMF goes with nonpolar compounds in general? _____________________
27. Which IMF goes with polar compounds in general? ______________________
28. What is the strongest IMF you can find in these samples:
a. CO gas _____________________
b. NaBr in water ____________________________
c. C6H12_____________________________
d. NH3 ________________________________
29. What holds the following together? Choices include the four IMF’s and polar covalent, nonpolar
covalent bonds or ionic bonds.
a. The Na ion to the Cl ion in NaCl(s) ________________________
b. The H atom to O atom in liquid water _________________________
c. An H2O molecule to another H2O molecule ____________________________
d. A CO2 molecule to another CO2 molecule _______________________
e. A PCl3 molecule to another PCl3 molecule ___________________________
30. Consider two liquids: PBr3 and C6H6. Answer the following questions based solely on IMF.
a. Which has the higher vapor pressure? _________________
b. Which has the higher boiling point? ________________
c. Which has the lower surface tention? _______________
d. Which has higher viscosity? __________________
31. Define vapor pressure in your own words.
32. Give three properties of water:
33. Draw a typical heating cooling curve in this box. Label solid, liquid gas, boiling point and melting
point.
34. A solution is defined as a _____________ dissolved in a ___________________.
35. Fill in the following table with yes or no as to whether the chemicals would mix based on like
dissolves like.
NH3 solute
C6H14 solute
SiF4 solute
PBr3 liquid solvent
36. What is the mass percent of 45.7 grams of NaCl dissolved in 255 grams of water?
37. If a normal IV glucose solution is 5.00 % glucose, what is the mass of the solvent if it contains 25.0 g
of glucose?
38. What is the molarity of 33.56 grams of potassium bromide dissolved to make a 2.200 L solution?
39. What is the molarity of 14.5 grams of magnesium chloride dissolved to make 1450 mL of solution?