Final exam review: second semester - Mrs. Baker's ...



Final exam review: second semester

*Make sure to study all relevant vocabulary from chapters 10-17, 22-23

The questions below are sample questions of only some of the topics we have covered. This is not a complete list of questions.

Look back at chapter problems and chapter reviews as well as old assignments, especially your chapter review worksheets. Also the on line textbook is a great resource for more practice. Be well prepared for your final.

You may have these items to aid you in the final: one large notecard 4” x 6” (HANDWRITTEN ONLY), both sides, your ion sheet, periodic table, periodic table of electronegativity values, functional group sheet, and a calculator. That’s it! Good luck!!

1. Know and be able to explain the kinetic molecular theory.

2. Know and be able to describe phase changes: between solid and liquid, liquid and gas, and solid and gas.

3. What are the properties of solid? Liquid? Gas?

4. What is the difference between an inorganic and an organic compound?

5. How many moles of ethane are present in 0.334 g?

6. A 362 g piece of silver has a heat capacity of 85.7 J/(C. What is the specific heat of silver?

7. A 6.22 kg piece of copper metal is heated from 20.5(C to 324.3(C. Calculate the heat absorbed by the metal. The specific heat of copper is 0.385J/g(C.

8. A sheet of gold weighing 10.0 g and at a temperature of 18.0(C is placed flat on a sheet of iron weighing 20.0 g and at a temperature of 55.6(C. What is the final temperature? The specific heat of gold is 0.128J/g(C and the specific heat of iron is 0.449 J/g(C.

9. A 0.1375 g sample of solid magnesium is burned in a constant volume bomb calorimeter that has a heat capacity of 1769 J/(C. The calorimeter contains exactly 300 g of water and the temperature increases by 1.126(C. Calculate the heat given off by the burning Mg in kJ/g and kJ/mol.

10. Explain why a helium weather balloon expands as it rises in the air. Assume that the temperature remains constant.

11. Convert the following temperatures to Kelvin: 0(C, 37(C, 100(C, -225(C.

12. Convert the following temperatures to (C: 77K, 4.2K, 6000K

13. A quantity of 36.4 L of methane gas is heated from 25(C to 88(C at constant pressure. What is its final volume?

14. What are standard temperature and pressure (STP)? What is the significance of STP in relation to the volume of one mole of an ideal gas?

15. A sample of nitrogen gas kept in a container of volume 2.3 L and at a temperature of 32(C exerts a pressure of 4.7 atm. Calculate the number of moles of gas present.

16. What volume would 5.6 moles of sulfur hexafluoride (SF6) gas occupy if the temperature and pressure of the gas are 128(C and 9.4 atm?

17. A gas filled balloon having a volume of 2.50 L at 1.2 atm and 25(C is allowed to rise to the stratosphere where the temperature and pressure are -23(C and 3.00 x 10-3 atm. Calculate the final volume of the balloon.

18. The temperature of 2.5 L of a gas initially at STP is increased to 250(C at constant volume. Calculate the final pressure of the gas in atm.

19. The pressure of 6.0 L of an ideal gas in a flexible container is decreased to one-third of its original pressure and its absolute temperature is decreased by one half. What is the final volume of the gas?

20. A gas evolved during the fermentation of glucose has a volume of 0.78 L when measured at 20.1(C and 1.00atm. What was the volume of this gas at the fermentation temperature of 36.5(C and 1.00 atm pressure?

21. Calculate the mass of NaOH in grams required to prepare a 5.00 x 102 ml solution of concentration 2.80M.

22. A quantity of 5.25 g of NaOH is dissolved in a sufficient amount of water to make up exactly 1 liter of solution. What is the molarity of the solution?

23. How many moles of MgCl2 are present in 60.0 ml of 0.100 M MgCl2 solution?

24. Calculate the molarity of phosphoric acid solution containing 1.5 x 102 g of the acid in 7.50 x 102 ml of solution.

25. How many grams of KOH are present in 35.0 ml of a 5.50 M solution?

26. Calculate the molarity of each of the following solutions:

a. 29 g ethanol (C2H5OH) in 545 ml of solution

b. 15.4 g sucrose in 74.0 ml of solution

c. 9.00 g sodium chloride in 86.4 ml of solution

27. Calculate the number of moles of solute present in

a. 75 ml of 1.25 M HCl

b. 100.0 ml of 0.35 M H2SO4

28. Calculate the volume in ml of a solution required to provide the following:

a. 2.14 g of sodium chloride from a 0.270 M solution

b. 4.30 g of ethanol from a 1.50 M solution

c. 0.85 g of acetic acid (CH3COOH) from a 0.30 M solution

29. Describe how to prepare 1.00 L of 0.646 M HCl solution starting with a 2.00 M HCl solution.

30. A quantity of 25.0 ml of a 0.866 M KNO3 solution is poured into a 500-ml volumetric flask and water is added until the volume of the solution is exactly 500 ml. What his the concentration of the final solution?

31. How would you prepare 60.0 ml of 0.200 M HNO3 from a stock solution of 4.00 M solution?

32. Calculate the pH for the following solutions and indicate whether the solution is acidic or basic:

a. [H+] = 1 x 10-2 mol/L

b. [OH-] = 1 x 10-2 mol / L

c. [OH-] = 1 x 10-8 mol / L

33. What are the products of a neutralization reaction?

34. Calculate the volume in ml of a 1.420 M NaOH solution required to titrate the following solution;

a. 25.00 ml of a 2.430 M HCl solution

b. 25.00 ml of a 4.500 M H2SO4 solution

c. 25.00 ml of a 1.500 M H3PO4 solution

35. Acetic acid is an important ingredient of vinegar. A sample of 50.0 ml of commercial vinegar is titrated against a 1.00 M NaOH solution. What is the concentration of acetic acid present in the vinegar if 5.75 ml of the base was required for the titration?

36. What volume of a 0.50 M KOH solution is needed to neutralize completely each of the following?

a. 10.0 ml of a 0.30 M HCl solution

b. 10.0 ml of 0.20 M H2SO4 solution

c. 15.0 ml of a 0.25 M H3PO4 solution

37. Based on intermolecular force consideration, explain what “like dissolves like” means.

38. Calculate the percent by mass of the solute in each of the following aqueous solutions:

a. 5.50 g of NaBr in 78.2 g of solution

b. 31.0 g of KCl in 152 g of water

c. 4.5 g of toluene in 29 g of benzene

39. Calculate the amount of water (in grams) that must be added to a 5.00 g of urea (H2NCONH2) in the preparation of a 16.2 % by mass solution.

40. It is estimated that 1.0 ml of seawater contains about 4.0 x 10-12 g of gold. The total volume of ocean water is 1.5 x 1021 L. Calculate the total amount of gold present in seawater. With so much gold out there, why hasn’t someone become rich by mining gold from the ocean?

41. A 3.20 g sample of a salt dissolves in 9.10 g of water to give a saturated solution at 25 degrees C. What is the solubility (g salt /100 g water) of the salt?

42. Write a balanced equation for the complete combustion of pentane.

43. Explain the difference between saturated and unsaturated hydrocarbons.

44. Draw and name the isomers of hexane.

45. Draw structures for the following compounds:

a. cyclopentane

b. cis -2-butene

c. 2,2,4-trimethylpentane

d. 1,1-diphenylhexane

e. para-dibromobenzene

f. 2-butyne

g. ethanol

h. ethylmethyl ether

i. propyl amine

j. butanone

k. pentanal

l. methanoic acid

46. Predict the products for the reactions:

a. CH3 – CH = CH2 + H2O (

b. C4H10 + Cl2 (

c. n CH2 = CH2 (

d. CH2 = CH – CH2 – CH3 + HBr (

47. Be able to identify and name functional groups

48. Know the basic properties of carbohydrates, lipids, and proteins.

49. Be able to draw the condensation reactions for any of the above.

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