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We can do similar analyses of the molecules Li2 and Bez. Figure 9 .16(b) shows the locations of the molecular orbitals resulting from the combination of P Y ' and p z orbitals relative to the two atomic nuclei. To understand better the relative energy levels of the molecular orbitals resulting from p-orbital combinations, consider the fluorine molecule (F z)....
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11.7(a) 11.7(b) 11.7(c). If, for example, as s hown in Figure 11.7(b), we double the pressure on the confined gas by adding enough mercury to make the difference in mercury levels on the left and right 760 mm (the height of a mercury column that exerts a pressure equal to 1 atm), the volume of the gas i s reduced...
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Sample Problem 11.12]. 11.2 PYI = P z V 2 (at constant temperature). 11.3 (a ) V = k2T (at constant pre ss ure) 11.3 (b). 11.10. 11.15. 11.16. Section 11.1: Properties of Gases. 11.2 11.3. 11.11 Why is it that if the barometer reading falls in one part of the world, it mu s t ri se so mewhere...
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Figure 12.15 Arrangement of identical spheres in a simple cubic cell. Figure 12.16 Three types of cubic cells. The other types of cubic cells, shown in Figure 12.16, are the body-centered cubic cell (bcc) and the face-centered cubic cell (fcc). SECTION 12.3 Crystal Structure 475. Figure 12.18 (a) A comer atom in any cell is shared by eight unit cells....
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12.99 Which of the following properties indicates ve ry s tron g. 12.103 Which of the following sub s tances h as the highest polarizability:. 12.105. 12.106. 12.107. 12.108. 12.109. 12.110. 12.111. 12.115. 12.116. 12.117. 12 .11 8. 12.119. 12.120. effect on the vapor pre ssu re of the water w he n (a) it s temperature is lowere d,...
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Checkpoint 13.5 Colligative Properties. SECTION 13.6 Calculations Using Colligative Properties 527. Sample Problems 13.10 and 13.11 illustrate this technique.. Sample Problem 13.10. Strategy Use Equation 13.7 to determine the molal concentration of the solution. Solution Solving Equation 13.7 for molal concentration,. Strategy Use Equation 13.8 to calculate the molarity of the solution. Solution Rearranging Equation 13.8 to solve for molarity,...
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[F, I doubles 0.10 0.20. Rate doubles 4.8 X X 10 - 3. rate 3 2.4 X 10 - 3 Mis = 2. rate I 1.2 X 10 - 3 Mis. 4.8 X 10 - 2.4 X 10 - 3. Thus, we can write the rate law as follow s. k = rate 1.2 X 10 - 3 Mis =...
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e) Calculate t ll2 of the reaction. 14.1 14. 14.4 14.5. 14.10. 14.11. Section 14.1: Reaction Rates Review Questions. 14.1 What is meant by the rate of a chemical reaction ? What are the units of the rate of a reaction. 14.3 What are the advantages of measuring the initial rate of a reaction?. 14.7 Consider the reaction. 14.8 Consider...
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which has an equilibrium constant (Ke) of 3 .0 X 10 - 6 at ns o c.. a) 3.0 X 10 - 6 c ) 2.0 X 10- 2 b) 2.5 X 10 - 4 d ) 3 . it) 3.0 X 10 - 6 atm b) 3.3 X 10 5 atm. lS.4A (a) 2.3 X 10 24 , (b)...
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Sample Problem 16.16. Checkpoint 16.7 Conjugate Acid-Base Pairs. Checkpoint 16.8 Diprotic and Polyprotic Acids. Figure 16.3 Lewis structures of the oxoacids of chlorine. SECTION 16.10 Acid-Base Properties of Salt Solutions 663. Sample Problem 16.20. 16.7 to determine Ka for NH t. SECTION 16.10 Acid-Base Properties of Salt Solutions 665. Figure 16.4 The six H 2 0. Checkpoint 16.10 Acid-Base Properties...
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Consider a liter of solution containing 0.10 mole of acetic acid. Using the Kafor acetic acid (1.8 X 10- 5 ) and an equilibrium table. Initial co ncentration (M): 0.10 0 0. Equilibrium concentration (M): 0.10 - x x x. Assuming that (0.10 - x) M = 0.10 M and solving for x, we get 1.34 X 10 - 3...
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Sample Problem 17.11. (Figur e 17.10):. Figure 17.9 (Left)Anaqueous cobalt(II) chloride solution. Checkpoint 17.5 Factors Affecting Soubility. Sample Problem 17.12. Fig u re 17.11 Flame tests for. Checkpoint 17.6 Separation of Ions Using Differences in Solubility. 17.6.1 A solution is 0.10 M in Br. 17.6.2 Barium nitrate is added slowly to a solution that is 0 . Figure 17.12 A...
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Sample Problem 18.2 demonstrates this approach.. SECTION 18.3 The Second and Third Laws of Thermodynamics 735. 92.6 kJ/mol) into Equation 18.9 , we get. From Equation 18.2, we write. Checkpoint 18.3 The Second and Third Laws of Thermodynamics. SECTION 18.4 Gibbs Free Energy 737. G = H- TS Equation 18.10. Each of the term s in Equation 18.10 pertain s...
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A half-reaction is an oxidation or a reduction that occurs as part of the overall redox reaction.. We adjust the coefficient of the chromium(III) ion to balance the reduction half-reaction.. SECTION 19.1 Balancing Redox Reactions 76. In the case of the reduction, there is a total charge of [(14. Sample Problem 19.1 shows how to use the half-reaction method to...
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19.1 19. 2 19.3 19.4. 19 5 E o = 0.0592 V I ct K. Section 19 .1: Balancing Redox Equations Problems. Section 19 .2: Galvanic Cells. 19.3 Define the following terms: anode, cathode, cell voltage, electromotive jorce, standard reduction potential.. Section 19.3: Standard Reduction Potentials. 19.11. 19.13 Which of the following reagent s can oxidize H 2 0 to...
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Figure 20.9 If a critical mass is present, many of the neutrons emitted during the fission process will be. Figure 20.10 Schematic. Figure 20.9 s how s two types of fission reactions. SECTION 20.5 Nuclear Fission 8- 3. The nuclear fuel consists of uranium , usually in the form of its oxide, U 3 0 S (Figure 20.13).. Figure 20.11...
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Having di scussed the chemi s try in the outer region s of Earth's atmosphere, we will focus in Sections 21.4 through 2 1. Figure 21.11 shows the carbon cycle in our global ecosystem. SECTION 21.5 The Greenhouse Effect 839. Fig u re 21.11 The carbon cycle.. Figure 21.12 The incomin g. Figure 21.13 Vibration motion of a diatomic molecule....
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Checkpoint 22.1 Coordination Compounds. Figure 22.5 s how s four different geometric arrangements for metal atoms with monodentate ligands. SECTION 22.2 Structure of Coordination Compounds 865. Figure 22.6 shows the cis and trans isomers of diamrninedichloroplatinum(II). Figure 22.9 shows the cis and trans isomers of dichlorobis(ethylenediamine)cobalt(III) ion and the mirror image of each. Figure 22 .6 The (a) cis and...
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Figure 23.11 (a) Silicon crystal doped with phosphorus. Figure 23.12 Main group metal s (gree n) and Group 2B metal s (b lue) according to their positions in the periodic table.. Phos- phorus ([Ne]3/3p 3 ) has one more va lence electron than si licon ([Ne ]3 s 2 3 p 2), so there is a valence electro n left...
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Figure 24.11 Structures of some common pho sphorus-containing. SECTION 24.5 Oxygen and Sulfur. The structure of hydrogen peroxide is s hown in Figure 24.12. Figure 24 .12 The structure of. SECTION 24.5 Oxygen and Sulfur 919. 2H20) and various sulfide minerals such as pyrite (FeS2) (Figure 24.14). Sulfur is extracted from underground deposits by the Frasch l process, shown in...