Chemistry Final Exam Review. Study quizlet for cpt 7, 8/9, 11, 12/14/15, and 22

Concepts and Problem review:

1. In the reaction 2NaCl 2Na + Cl2, chlorine is a ___. 2. Explain how you can tell the difference between synthesis, decomposition, single displacement, and double displacement reactions. Give an example of each.3. In a chemical equation what is the difference between coefficients and subscripts?4. What is the differences between reactants and products?5. What are the symbols used in chemical equations to show the states of matter of the reactants and product?6. What is stoichiometry?7. What are the 5 types of chemical reactions and how can you tell them apart?8. Balance the following: Cu + Fe2O3 Fe + CuO9. What are the products resulting from a reaction between aluminum sulfate and lithium oxide?10. How does a real gas differ from an ideal gas?11. What is Boyles law? 12. What is Charles law13. What is Avogadros law14. What is the ideal gas law15. At high pressures which of the following may cause real gas to deviate from the behavior predicted for an ideal gas?16. What does water vapor pressure depends on ?17. What is molar volume? 18. How are the pressure and volume of a gas related?19. What is an electrolyte?20. What is Arrheniuss theory on acids and bases? Give an example21. What is the Bronsted-Lowry theory on acids and bases? Give an example22. What is the Lewis theory on acids and bases? Give an example23. What is the formula for a hydronium ion? Why is it important?24. Label the acid, base, conjugate acid, and conjugate base in the reaction:HCl + KOH KCl + H2O 25. What are conjugate acids and conjugate bases?26. What are the products that would be expected in the neutralization reaction involving nitric acid and lithium hydroxide . Write and balance the equation27. Which of the following oxide will form an acid when you add water to it? MgO or SO228. What is an amphoteric substance29. What are the characteristics of a strong acid? A strong base?30. What is an indicator? What are some advantages and disadvantages to them?31. Write the net ionic equation for the reaction of MgCl2 and LiOH in water?32. What is hydrolysis? What might be formed in a hydrolysis reaction33. What is a spectator ion? How can you tell if an ion is a spectator ion?34. What is a buffer system and what does it do?35. What is the difference between aliphatic and aromatic hydrocarbons? Give examples36. What is a homologous series? Give an example37. What are the formulas and names for the first 10 alkanes?38. What is the difference among alkanes, alkenes and alkynes?39. What type of substituted hydrocarbons can you make with C=O ?40. How do you name halogen compounds? Give an example41. How do you name branched hydrocarbons? Give and example42. Are hydrocarbons ionic compounds or molecules (ionic bonds or covalent bonds)?43. What is percentage yield?44. What are the conditions of STP?45. Write the parent acid and parent base of the following salt and decide if its acidic, basic, or neutral: Al(NO3)346. Name the following compound: CH3 - CH2 - CH2 CH2 - CH2 - CH347. Explain the differences that you would see in a structural formula between aliphatic and aromatic compounds.48. What is the difference between a monatomic and polyatomic ion? Give examples49. What is the difference between a binary and ternary compound? Give examples50. What is the difference between an anion and a cation? Give examples51. What is the oxidation number of Copper II? Show the ion symbol52. What ions are in Li2SO4?53. What are the rules for naming ionic compounds. Give an example and explain how to do it54. How many atoms of O are shown In Mg(NO3)255. Name the 7 diatomic gases.56. Name this compound Mg(NO3)2 and Li2O57. Write the formula for the compound made from iron II and Phosphate58. For the formula of a compound to be correct, the algebraic addition of the charges on the atoms or ions in the compound must add up to __________.59. What is the charge of each ion in CuO?60. What is the atomic mass unit? What isotope was it based on?61. What is the difference between empirical formulas and molecular formulas?62. What is the empirical formula for H2O263. What is the formula mass of copper II sulfate (write the formula first)64. If one molecule of CO2 has a mass of 44 u, what is the mass of 6.02 X 10^23 molecules of CO265. Use the Stock method to name this compound: Fe2O3

66. Write the formula for the compound you would get if you combined aluminum and sulfate.

CALCULATIONS:

Stoichiometry:1. Ammonia is produced according to the following equation: N2 + 3H2 2NH3. How many grams of nitrogen would be required to produce 21 grams of ammonia?

Percentage yield2. In the reaction between calcium hydride and water the theoretical yield of hydrogen is 7.18 grams. In running this reaction the actual amount of hydrogen produced was 5.8 grams. What was the percentage yield of this reaction?

Gas Laws:3. 0.0840 l of a gas is collected by water displacement at 22.0 C and 102 kPa. What volume would the dry gas occupy at 101.3kPa and 27.0C? (water vapor pressure at 22.0C = 2.6 kPa)

4. You have 2.3 dm3 of oxygen at a pressure of 98.0 kPa and a temperature of 21 C. What is the volume under standard conditions?

5. Correct the volume of the gas to what it would be at standard temperature, the initial conditions where212 mL at 22 degrees Celcius.

6. 0.5 mole of a gas was collected in a lab at a temperature of 20.0 C and a pressure of 105.0 kPa. What volume will the gas occupy under these conditions?

ACID BASE TITRATIONS:7. 70.0 mL of 2.00M KOH are used in titrating 25 mL of HCl. What is the concentration of the HCl?

Mole Calculations8. How many molecules of sulfur dioxide are present in .87 moles of sulfur dioxide?

9. How many moles are represented by 112.0 grams of NO2

10. 1.50 X 10^23 molecules of salt, NaCl, would have a mass of ___.

11. What is the percent of Li in Li2SO4?

12. What is the molecular formula for hydrogen peroxide if its empirical formula is HO and its molecular mass is 34.

13. If a compound containing only magnesium and oxygen consists of 0.564 g Mg and 0.376 g O, what is the compound's empirical formula..