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# Module 1 Chapter 1 (5 questions)

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Module 1 Chapter 1 (5 questions)

Preston University

Chemistry (CH 1010)

Module 1 Chapter 1 (5 questions) 24. Which of the following are exact numbers?

A. There are 100 cm in 1 m.

B. One meter equals 1.094 yards.

C. We can use the equation F = (9/5)C + 32 to convert from Celsius to Fahrenheit temperature.

Are the numbers (9/5) and 32 exact or inexact?

D. = 3.1415927

a. exact

b. inexact; 0.9144 m/yd is exact (see Exercise 1.23c) Thus, there are 1/0.9144= 1.093613 ...yd/m.

c. exact

d. inexact (it has an infinite number of decimal places.)

34. a. How many kilograms are in one teragram? 2b. How many nanometers are in 6.50 X 10 terameters?

c. How many kilograms are in 25 femtograms?

d. How many liters are in 8.0 cubic decimeters?

e. How many microliters are in one milliliter?

f. How many picograms are in one microgram?

52. A thermometer gives a reading of 96.1 F + 0.2F What is the temperature in C? What is the uncertainty?

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3 at 20C. If 5.25 of pure silver pellets is added to a graduated 60.The density of pure silver is 10.5 g/cm

cylinder containing 11.2 mL of water, to what volume level will the in the cylinder rise?

64. What is the difference between homogeneous and heterogeneous matter? Classify each of the

following as homogeneous or heterogeneous.

a. soil

b. the atmosphere

c. a carbonated soft drink

d. gasoline

e. gold

f. a solution of ethanol and water

Module 2 Chapter 2 (4 questions)

28. The mass of beryllium that combines with 1.000g of oxygen to form beryllium oxide is 0.5633g.

When atomic masses were first being measured, it was thought that the formula of beryllium oxide was

BeO. What would be the atomic mass of beryllium is this were the case? Assume that oxygen has an 23

atomic mass of 16.00.

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34. What are the symbols of the following metals: sodium, beryllium, manganese, chromium, uranium?

52. Complete the following table:

Symbol # protons in nucleus # neutrons in nucleus # electrons Net charge

238 U92

20 20 2+

23 28 20

89 Y39

35 44 36

15 26 3-

72. Write the formula for each of the following compounds:

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a. sulfer diflouride

b. sulfur hexaflouride

c. sodium dihydrogen phosphate

d. lithium nitride

e. chromium (III) carbonate

f. time (II) flouride

g. ammonium acetate

h. ammonium hydrogen sulfate

i. cobalt(III) nitrate

j. mercury(I) chloride

k. potassium chlorate

l. sodium hydride

Module 3 Chapter 3 (5 questions)

24. An element consists of 1.40% of an isotope with mass 203.973 amu, 24.10% of an isotope with mass

205.9745 amu, 22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with mass

207.9766 amu. Calculate the average atomic mass and identify the element. 30. How many Fe atoms and how many moles of Fe atoms are in 500.og of iron?

58. There are several important compounds that contain only nitrogen and oxygen. Calculate the mass

percent of nitrogen in each of the following:

a. NO, a gas formed by the reaction of N2 with O2 in internal combustion engines.

b. NO2, a brown gas mainly responsible for the brownish color of photochemical smog.

c. N2O4, a colorless liquid used as a fuel for the space shuttle.

d. N2O, a colorless gas sometimes used as an anesthetic by dentists (known as laughing gas).

68. The compound adrenaline contains 56.79% C, 6.56% H, 28.37% O, and 8.28% N by mass. What is the empirical formula for adrenaline?

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82. Balance the following equations:

(aq) + HPO(aq) HO(l) + Ca(PO)(s) a. Ca(OH)2342342

b. Al(OH)(s) + HCl(aq) AlCl(aq) + HO(l) 332

c. AgNO(aq) + HSO(aq) AgSO(s) + HNO(aq) 324243

Module 4 Chapter 4 (4 questions)

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

a. A 16.45 g sample of NaCl is dissolved in enough water to make 1.000 L of solution.

b. An 853.5 mg sample of KIO3 is dissolved in enough water to make 250.0 mL of solution.

c. A 0.4508 g sample of iron is dissolved in a small amount of concentrated nitric acid forming Fe3+

ions in solution and is diluted to a total volume of 500.0 mL. (Calculate the molarity of Fe3+.)

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30. When the following solutions are mixed together, what precipitate (if any) will form?

(aq) + KCl(aq) a. FeSO4b. Al(NO)(aq) + Ba(OH)(aq) 332

c. CaCl(aq) + NaSO(aq) 224

d. KS(aq) + Ni(NO)(aq) 232

48. Write the balanced molecular, complete ionic, and net ionic equations for the reactions that occur when

the following are mixed.

a. solid silver hydroxide and hydrobromic acid

b. aqueous strontium hydroxide and hydroiodic acid

c. solide iron(III) hydroxide and nitric acid

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64. Balance the following oxidation-reduction reactions that occur in acidic solution using the half-reaction method. -2+(aq) Cu(aq) + NO(g) a. Cu(s) + NO3-3+2-b. CrO(aq) + Cl(aq) Cr(aq) + Cl(g) 272

c. Pb(s) + PbO(s) + HSO(aq) PbSO(s) 22442+3+-d. Mn(aq) + NaBiO(s) Bi(aq) + MnO(aq) 34

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2+AsO(aq) + Zn(s) AsH(g) + Zn(aq) e. H343

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Module 5 Chapter 5 (4 questions) 24. A gauge on a compressed gas cylinder reads 2200 psi (pounds per square inch; 1 atm = 14.7 psi).

Express this pressure in each of the following units.

a. standard atmospheres

b. megapascals (Mpa)

c. torr

32. Consider the following chemical equation. 2NO(g) NO(g) If 25.0 mL of NO gas is completely 2242converted to NO gas under the same conditions, what volume will the NO occupy? 2424

50. The method used by Joseph Priestley to obtain oxygen made use of the thermal decomposition of mercuric oxide: heat 2HgO(s) 2Hg(l) + O(g) 2

What volume of oxygen gas, measured at 30.0C and 725 torr, can be produced from the complete decomposition of 4.10 g mercuric oxide?

62. A mixture of 1.00 g H and 1.00 g He is placed in a 1.00 L container at 27C. Calculate the partial 2pressure of each gas and the total pressure.

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Module 6 Chapter 6 (5 questions)

-5518. Calculate the kinetic energy of a 1.0 X 10 g object with a velocity of 2.0 X 10 cm/s.

22. Calculate E for each of the following.

a. q = -47 kJ, w = +88 kJ

b. q = +82 kJ, w = +47 kJ

c. q = +47 kJ, w = 0

d. In which of these cases do the surroundings do work on the system?

32. Are the following processes exothermic or endothermic? a. the combustion of gasoline in a car engine

b. water condensing of a cold pipe

c. CO(s) CO(g) 22

d. F(g) 2F(g) 2

52. Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon

and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of

combustion for CH (-2341 kJ/mol), CH (-2755 kJ/mol), and H (-286 kJ.mol), calculate H for the 44482reaction

CH(g) + 2H(g) CH(g) 44248

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