Glencoe Semester II Review Problems 2015
1. If 42.7 g of carbon monoxide reacts completely with nitrogen monoxide at STP, what volume of
nitrogen gas will be produced? Carbon dioxide is the only other product of this reaction.
2. If 5.50 moles of CaC2 react with excess water. How many moles of C2H2 will be produced?
product of this reaction is calcium hydroxide.
The other
3. What ions form when sulfuric acid dissolves in water?
4. A substance is composed of 51.37% oxygen, 47.70% chromium and 0.9265% hydrogen. If the molar
mass is 218 grams, what is the molecular formula of this substance?
5. Give the pH of a solution with a [OH-] of 3.75 x 10-8 M. Is this an acid or a base?
6. When 10.2 g of canola oil at 25.0°C is placed in a wok, 3.34 kJ of heat is required to heat it to a
temperature of 196.4°C. What is the specific heat of canola oil?
7. What acid must have reacted with calcium hydroxide in order to form the calcium nitrate salt?
8. Give the percent composition for the oxygen present in a sample of ammonium acetate.
9. What is the molarity of a 1.5 L solution containing 40.0 g of C6H12O6?
10. Calculate the missing value:
a. V1 = 2.0 L, P1 = 0.82 atm, V2 = 5.0 L, P2 = ?
b. V1 = 250 ml, T1 = ?, V2 = 400. Ml, T2 = 75°C
c. P1 = 14.952 psi, T1 = -10°C, P2 = ?, T2 = 45°C
d. P1 = 450 torr, V1 = 4.00 L, T1 = ?, P2 = 32.55 in. Hg, V2 = 425 ml, T2 = 873 K
11. What is the difference between a solute and a solvent?
12. Perform the following conversions:
a. 3.25 x 1020 atoms of silicon to moles
b. 4.25 x 10-2 moles of sulfuric acid to molecules
c. 5.90 grams of carbon tetrachloride to molecules
d. 4.44 x 1023 atoms of lead to grams
e. 78 grams of silicon to atoms
13. Calculate the pressure inside an old-time TV tube with a volume of 3.50 L that contains 2.300 x 10-5
grams of nitrogen gas at 22.0°C.
14. Write the balanced equation for the reaction between hydrobromic acid and aluminum hydroxide.
15. How much energy is lost by 3580 g of granite as it cools from 41.2°C to -12.9°C? Granite has a specific
heat 0.803 J/g°C.
16. The empirical formula for the indicator, congo red, is NaC15H11N3SO3. Congo red’s molar mass is about 673
g/mole. What is the molecular formula for congo red?
17. What mass of ammonium thiosulfate is required to produce 1.5 L of 0.25 M solution?
18. Calculate [OH-] in an aqueous solution where [H3O+] is 5.40 x 10-3M. Is this an acid or a base?
19. Determine the theoretical yield and the percent yield of C2H5OH if 684 g of C12H22O11 reacts and 349 g
of C2H5OH is obtained in the following reaction: C12H22O11 + H2O  C2H5OH + CO2
20. What mass of argon is in a sealed, 2.00 L tank at 3.50 atm and 25.0°C?
21. Write the equation showing what happens when chromic acid dissolves in water.
22. What volume of a 3.00 M solution can be made from 122 g LiF?
23. Sketch a rough graph illustrating an endothermic reaction with low activation energy.
24. What is the empirical formula for a compound that is 85.63% carbon and 14.37% hydrogen?
25. What mass of C2H5OH can be made from 750 g of C6H12O6?
C6H12O6  C2H5OH + CO2
26. What is the volume of 42 g of carbon monoxide gas at STP?
27. Car batteries use lead, lead (IV) oxide and sulfuric acid to produce an electric current. The products of
this reaction are lead (II) sulfate and water. What mass of lead (II) sulfate will form when 25.0 g of lead
reacts with excess amounts of the other reactants?
28. Bond breaking (releases/absorbs) energy.
29. What is the pH of a base with a molarity of 0.875 M?
30. Calculate the change in enthalpy for the synthesis of dichlorine monoxide. Is this reaction exothermic or
endothermic?
31. What volume of 0.250 M lead (II) chloride solution is required to react completely with 75.00 g of
aluminum acetate?
32. Dihydrogen monosulfide reacts with oxygen gas to form water and sulfur atoms. What mass of sulfur
will form if 6.5 L of oxygen gas is completely used up at 2.0 atm and 290 K?
33. In lab, a student oxidizes a 0.280 g sample of nickel in a crucible. The final mass of the nickel oxide in
the crucible after oxidation is complete is 0.433 g. Write the formula and name for the nickel oxide in
the crucible.
34. How many grams of sodium metal will react with 3.00 L of 0.500 M calcium nitrate solution?
35. Name the salt that will form from a reaction between phosphoric acid and magnesium hydroxide.
36. Calculate ΔH for the reaction P4 + O2  P4O6. P4 contains six P – P bonds and P4O6 contains twelve
P – O bonds. Is the activation energy for this reaction more or less than the energy released as the P4O6
bonds form?
37. Upon heating, calcium carbonate decomposes to calcium oxide and carbon dioxide. What is the
theoretical yield of carbon dioxide if 235.0 g of reactant is heated? What is the percent yield of carbon
dioxide if 197.5 g of carbon dioxide is collected?
38. What is the pH of a solution in which [H3O+] = 7.9 x 10-3M. Is this solution an acid or a base?
39. Write a balanced equation for the neutralization of acetic acid with magnesium hydroxide.
40. Find the percent composition of metal in a sample of titanium (II) phosphide.
41. What is the molarity of hydrocyanic acid if 0.0275 liters of 3.025 M nickel (III) hydroxide are required
to neutralize 0.0148 liters of the acid?
42. What is the final pH of a mixture of 12.48 ml of 0.150 M phosphoric acid and 14.75 ml of 0.280 M
magnesium hydroxide?
43. Calculate the enthalpy change for the reaction CH4 + Cl2  CCl4 + H2. Is this reaction going to get hot
or cold as it proceeds?