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All Textbook Solutions for Introductory Chemistry: A Foundation

. For the reaction Br2(g)+5F2(g)2BrF5(g)the system at equilibrium at a particular temperature is analyzed. and the following concentrations are found: [BrF5(g)]=1.01109M,[Br2(g)]=2.41102M, and [F2(g)]=8.15102M. Calculate the value of K for the reaction at this temperature.. Consider the reaction SO2(g)+NO2(g)SO3(g)+NO(g)Suppose it is found at a particular temperature that the concent rations in the system a equilibrium are as follows: [SO3(g)]=4.99105M,[NO(g)]=6.31107M, [SO2(g)]=2.11102M, and [NO2(g)]=1.73103M. Calculate the value of K for the reaction at this temperature.. For the reaction 2CO(g)+O2(g)2CO2(g)it is found at equilibrium at a certain temperature that the concentrations are [CO(g)]=2.7104M,[O2(g)]=1.9103M, and [CO2(g)]=1.1101M. Calculate K for the reaction at this temperature.. For the reaction CO2(g)+H2(g)CO(g)+H2O(g)the equilibrium constant. K, has the value 5.21103at a particular temperature. If the system is analyzed at equilibrium at this temperature, it is found that [CO(g)]=4.73103M,[H2O(g)]=5.21103M, and [CO2(g)]=3.99102M. What is the equilibrium concentration of H2(g) in the system?. The equilibrium constant for the reaction H2(g)+F2(g)2HF(g)has the value 2.1103at a particular temperature. When the system is analyzed at equilibrium at this temperature, the concentrations of both H2(g) and F2(g) are found to be 0.0021 M. What is the concentration of HF(g) in the equilibrium system under these conditions?. For the reaction 2H2O(g)2H2(g)+O2(g)K=2.4103at a given temperature. At equilibrium ills found that [H2O(g)]=1.1101Mand [H2(g)]=1.9102M. What is the concentration of O2(g) under these conditions?. For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular temperature. a. What does the very small equilibrium constant indicate about the extent to which oxygen gas, O2(g), is converted to ozone gas, O3(g), at this temperature? b. If the equilibrium mixture is analyzed and [O2(g)]is found to be 3.04102M, what is the concentration of O3(g) in the mixture’?. For the reaction N2O4(g)2NO(g)the equilibrium constant K has the value 8.1103at a particular temperature. If the concentration of N2O4(g) is found to be 5.4104Min the equilibrium system, what is the concentration of NO2(g) under these conditions?. Explain how the dissolving of an ionic solute in water represents an equilibrium process.. What is the special name given to the equilibrium constant for the dissolving of an ionic solute in water?. Why does the amount of excess solid solute present in a solution not affect the amount of solute that ultimately dissolves in a given amount of solvent?. Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to line particles before dissolving. c. The temperature changes.. Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for K for each process. a. AgIO3(s) c. Zn3(PO4)2(s) b. Sn(OH)2(s) d. BaF2(s). Write the balanced chemical equation describing the dissolving of each of the following sparingly soluble salts in water. Write the expression for Kspfor each process. a. NiS(s) c. BaCrO4(s) b. CuCO3(s) d. Ag3PO4(s). K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.60QAP . A saturated solution of nickel(II) sulfide contains approximately 3.6104gof dissolved NiS per liter at 20°C. Calculate the solubility product K for NiS at 20 °C.. Most hydroxides are not very soluble in water. For example, for nickel(II) hydroxide. Ni(OH)2, is 2.01015at 25 °C. How many grams of nickel(ll) hydroxide dissolve per liter at 25 °C?. The solubility product constant, Ksp, for calcium carbonate at room temperature is approximately 3.0109. Calculate the solubility of CaCO3in grams per liter under these conditions.. Calcium sulfate, CaSO4, is only soluble in water to the extent of approximately 2.05 g/L at 25 °C. Calculate Kspfor calcium sulfate at 25°C.. Approximately 1.5103of iron(II) hydroxide. Fe(OH)2(s), dissolves per liter of water at 18 °C. Calculate Kspfor Fe(OH)2(s) at this temperature.. Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate Kspfor Cr(OH)3at this temperature.. Magnesium fluoride dissolves in water to the extent of 8.0102g/L at 25°C. Calculate the solubility of MgF2(s) in moles per liter, and calculate Kspfor MgF2at 25 °C.. Lead(II) chloride, PbCl2(s), dissolves in water to the extent of approximately 3.6102Mat 20 °C. Calculate Kspfor PbCl2(s), and calculate its solubility in grams per liter.. Mercury(I) chloride, Hg2Cl2, was formerly administered orally as a purgative. Although we usually think of mercury compounds as highly toxic, the K of mercury(I) chloride is small enough (1.31018)that the amount of mercury that dissolves and enters the bloodstream is tiny. Calculate the concentration of mercury(I) ion present in a saturated solution of Hg2Cl2.. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.. Before two molecules can react, chemists envision that the molecules must first collide with one another. Is collision among molecules the only consideration for the molecules to react with one another?. Why does an increase in temperature favor an increase in the speed of a reaction?. The minimum energy required for molecules to react with each other is called the _______ energy.. A(n) _______ speeds up a reaction without being consumed.. Equilibrium may be defined as the ________ of two processes, one of which is the opposite of the other.. When a chemical system has reached equilibrium, the concentrations of all reactants and products remain _________ with lime.. What does it mean to say that all chemical reactions are, to one extent or another, reversible?. What does it mean to say that chemical equilibrium is a dynamic process?. At the point of chemical equilibrium, the rate of the forward reaction _________ the rate of the reverse reaction.. Equilibria involving reactants or products in more than one state are said to be _________ .. According to Le Châtelier’s principle, when a large excess of a gaseous reactant is added to a reaction system at equilibrium, the amounts of products _____.. Addition of an inert substance (one that does not participate in the reaction) does not change the _________ of an equilibrium.. When the volume of a vessel containing a gaseous equilibrium system is decreased, the _________ of the gaseous substances present is initially increased.. Consider the following reaction at some temperature: H2O(g)+CO(g)H2(g)+CO2(g)K=2.0 Some molecules of H2O and CO are placed in a 1.0-L container as shown below. When equilibrium is reached, how many molecules of H2O, CO, H2, and CO2are present? Do this problem by trial and error—that is, if two molecules of CO react, is this equilibrium: if three molecules of CO react, is this equilibrium: and so on.. What is meant by the solubility product for a sparingly soluble salt? Choose a sparingly soluble salt and show how the salt ionizes when dissolved in water, and write the expression for its solubility product.. For a given reaction at a given temperature, the special ratio of products to reactants defined by the equilibrium constant is always equal to the same number. Explain why this is true, no matter what initial concentrations of reactants (or products) may have been taken in setting up an experiment.. Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the inter-conversion reaction?. Suppose K=4.5103at a certain temperature for the reaction PCl5(g)PCl3(g)+Cl2(g)If it is found that the concentration of PCl5is twice the concentration of PCl3, what must be the concentration of Cl2under these conditions?. For the reaction CaCO3(s)CaO(s)+CO2(g)the equilibrium constant K has the form K=[CO2]. Using a handbook to find density information about CaCO3(s) and CaO(s), show that the concentrations of the two solids (the number of moles contained in 1 L of volume) are constant.90AP . Teeth and bones are composed, to a first approximation, of calcium phosphate. Ca3(PO4)2(s). The K for this salt is 1.31032at 25 °C. Calculate the concentration of calcium ion in a saturated solution of Ca3(PO4)2.. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?. How does the collision model account for the fact that a react ion proceeds faster when the concentrations of the reactants are increased?94AP . Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?96AP 97AP . For the reaction N2(g)+3Cl2(g)2NCl3(g)an analysis of an equilibrium mixture at a particular temperature is performed. It is found that [NCl3]=1.9101M,[N2]=1.4103M, and [Cl2]=4.3105M. Calculate K for the reaction.. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.. Write the equilibrium expression for each of the following heterogeneous equilibria. a. 4Al(s)+3O2(g)2Al2O3(s)b. NH3(g)+HCl(g)NH4Cl(s)C. 2Mg(s)+O2(g)2MgO(s). Write the equilibrium expression for each of the following heterogeneous equilibria. a. P4(s)+5O2(g)P4O10(s)b. CO2(g)+2NaOH(s)Na2CO3(s)+H2O(g)c. NH4NO3(s)N2O(g)+2H2O(g). Consider the following generic reaction: 2A2B(g)2A2(g)+B2(g) Some molecules of A2B are placed in a 1.0-L container. As time passes, several snapshots of the reaction mixture are taken as illustrated below. Which illustration is the first to represent an equilibrium mixture? Explain. How many molecules of A2B reacted initially?103AP . The reaction PCl3(l)+Cl2(g)PCl5(s)liberates 124 kJ of energy per mole of PCl3reacted. Will an increase in temperature shift the equilibrium position toward products or toward reactants?105AP . For the reaction N2(g)+3H2(g)2NH3(g)K=1.3102at a given temperature. If the system at equilibrium is analyzed and the concentrations of both N2and H2are found to be 0.10 M, what is the concentration of NH3in the system?. The equilibrium constant for the reaction 2NOCl(g)2NO(g)+Cl2(g)has the value 9.2106at a particular temperature. The system is analyzed at equilibrium, and it is found that the concentrations of NOCl(g) and NO(g) are 0.44 M and 1.5103M. respectively. What is the concentration of Cl2(g) in the equilibrium system under these conditions?108AP 109AP 110AP . Mercuric sulphide, HgS, is one of the least soluble salts known, with Ksp=1.61054at 25 °C. Calculate the solubility of HgS in moles per liter and in grams per liter.112AP . For the reaction N2(g)+3H2(g)2NH3(g), list the types of bonds that must be broken and the type of bonds that must form for the chemical reaction to take place.. What does the activation energy for a reaction represent? How is the activation energy related to whether a collision between molecules is successful?115AP 116AP 117AP 118AP 119AP 120CP . Suppose that for a hypothetical reaction: A2(g)+2B(g)2AB(g)It is determined that at a certain temperature the equilibrium concentrations are: [A2]=0.0090,[B]=0.940, and [AB]=5.3104. Calculate the numerical value of K for the reaction.122CP . The reaction H2(g)+I2(g)2HI(g)has Kp=45.9at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 4.94 atm and H2at a pressure of 0.628 atm. Calculate the equilibrium pressure of I2(g) in this mixture.124CP 125CP . Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the following changes affect the number of moles of each component of the system after equilibrium is re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst 1CR 2CR 3CR How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?5CR How is the pH scale defined? What range of pH values corresponds to acidic solutions? What range corresponds to basic solutions? Why is pH = 7.00 considered neutral? When the pH of a solution changes by one unit, by what factor does the hydrogen ion concentration change in the solution? How is pOH defined? How arc pH and pOH for a given solution related? Explain.7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?8CR 9CR . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?. Describe how we write the equilibrium expression for a reaction. Give three examples of balanced chemical equations and the corresponding expressions for their equilibrium constants.12CR 13CR . In your own words, paraphrase Le Châtelier’s principle. Give an example (including a balanced chemical equation) of how each of the following changes can affect the position of equilibrium in favor of additional products for a system: the concentration of one of the reactants is increased: one of the products is selectively removed from the system: the reaction system is compressed to a smaller volume: the temperature is increased for an endothermic reaction: the temperature is decreased for an exothermic process.15CR 16CR a. Write the conjugate base for each of the following Brensted- Lowry acids. Oj, H2SOj. HC1O4. NH/. H2CO, Write the conjugate acid for each of the following Bronsted- Lowry bases. ~. hso4- nh2- nh3, co32-. Identify the Brønsted-Lowry conjugate acid-base pairs in each of the following. a. NH3(aq)+H2O(l)NH4+(aq)+OH(aq)b. H2SO4(aq)+H2O(l)HSO4(aq)+H3O+(aq)c. O2(s)+H2O(l)2OH(aq)d. NH2(aq)+H2O(l)NH3(aq)+OH(aq)e. H2PO4(aq)+OH(aq)HPO42(aq)+H2O(l)19CR 20CR 21CR 22CR 23CR . The solubility product of magnesium carbonate, MgCO3, has the value Ksp=6.82106at 25 °C. How many grams of MgCO3will dissolve in 1.00L of water?18.1SC 1CT 18.2SC 18.3SC 18.4SC 1CT Sketch a galvanic cell, and explain how it works. Look at Figs. 18.1 and 18.5. Explain what is occurring in each container and why the cell in Fig. 18.5 “works,” but the one in Fig. 18.1 does not.2ALQ Which of the following are oxidation-reduction reactions’? Explain. a.PCl3+Cl2PCl5b.Cu+2AgNO3Cu( NO3)2+2Agc.CO2+2LiOHLi2CO3+H2Od.FeCl2+2NaOHFe(OH)2+2NaCIe.MnO2+4HClCl2+2H2O+MnCl2 4ALQ 5ALQ 6ALQ In balancing oxidation-reduction equations, why is it permissible to add water to either side of the equation?What does it mean for a substance to be oxidized? The term “oxidation” originally came from substances reacting with oxygen gas. Explain why a substance that reacts with oxygen gas will always be oxidized.Label the following parts of the galvanic cell. anode cathode reducing agent oxidizing agent 1QAP 2QAP For each of the following oxidation-reduction reactions, identify which element is being oxidized and which is being reduced. a.Cl2(g)+I2(g)2ICl(g)b.Cl2(g)+2Li(s)2LiCl(s)c.2Na(s)+2H2O(l)2NaOH(aq)+H2(g)d.Cl2(g)+2NaBr(aq)2NaCl(aq)+Br2(l)For each of the following oxidation-reduction reactions, identify which element is oxidized and which is reduced. a.6Na(s)+N2(g)2Na3N(s)b.Mg(s)+Cl2(g)MgCl2(s)c.2Al(s)+3Br2(l)2AlBr3(s)d.CuSO4(aq)+Mg(s)MgSO4(aq)+Cu(s)For each of the following oxidation-reduction reactions, identify which element is being oxidized and which is being reduced. a.Ca(s)+2H2O(l)Ca(OH)2(s,aq)+H2(g) b.H2(g)+F2(g)2HF(g) c.4Fe(s)+3O2(g)2Fe2O3(s) d.2Fe(s)+3Cl2(g)2FeCl3(s)6QAP 7QAP 8QAP Explain why, although it is not an ionic compound, we still assign oxygen an oxidation state of 2 in water, H2O. Give an example of a compound in which oxygen is not in the 2 oxidation state.10QAP 11QAP 12QAP 13QAP . Assign oxidation states to all of the atoms in each of the following. a. NBr3 c. PBr5 b. SeF6 d. CH4 15QAP 16QAP . What is the oxidation state of chlorine in each of the following substances? a. CIF c. HCI b. Cl2 d. HClO . What is the oxidation state of manganese in each of the following substances? a. MnCl2 c. MnO2 b. KMnO4 d. Mn(C2H3O2)3 19QAP Assign oxidation states to all of the atoms in each of the following. CaOc. PFj AI2O3d. P2O5 21QAP 22QAP 23QAP 24QAP 25QAP 26QAP . Does an oxidizing agent donate or accept electrons? Does a reducing agent donate or accept electrons?28QAP 29QAP 30QAP 31QAP 32QAP 33QAP 34QAP 35QAP 36QAP 37QAP 38QAP 39QAP 40QAP 41QAP 42QAP 43QAP 44QAP . Balance each of the following oxidation-reduction reactions, which take place in acidic solution, by using the “half-reaction” method. a.Mg(s)+Hg2+(aq)Mg2+(aq)+Hg22+(aq)b.NO3(aq)+Br(aq)NO(g)+Br2(l)c.Ni(s)+NO(aq)Ni2+(aq)+NO2(g)d.ClO4(aq)+Cl(aq)ClO3(aq)+Cl2(g)46QAP . Iodide ion, I- , is one of the most easily oxidized species. Balance each of the following oxidation-reduction reactions, which take place in acidic solution, by using the “half-reaction” method. a.IO3(aq)+I(aq)I2(aq)b.Cr2O72-(aq)+I(aq)Cr3+(aq)+I2(aq)c.Cu2+(aq)+I(aq)CuI(s)+I2(aq)48QAP 49QAP 50QAP . In which direction do electrons flow in a galvanic cell, from anode to cathode or vice versa?52QAP . Consider the oxidation-reduction reaction Al(s)+Ni2+(aq)Al3+(aq)+Ni(s)Sketch a galvanic cell (hat makes use of this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?. Consider the oxidation—reduction reaction Zn(s)+Pb2+(aq)Zn2+(aq)+Pb(s)Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?55QAP 56QAP 57QAP 58QAP 59QAP 60QAP 61QAP 62QAP . Although aluminum is one of the most abundant metals on earth, its price until the 1890s made it a precious metal” like gold and platinum. Why?. The “Chemistry in Focus” segment Water-Powered Fireplace discusses a fireplace that uses the electrolysis of water to produce hydrogen gas. Write the balanced chemical equation for the electrolysis of water. Which element in water is oxidized? Which is reduced? Find the oxidation states to answer these questions. Also, how is heat generated by the fireplace?65AP 66AP 67AP 68AP 69AP 70AP 71AP 72AP 73AP . To obtain useful electrical energy from an oxidation-reduction process, we must set up the reaction in such a way that the Oxidation half-reaction and the reduction half-reaction are physically one _____another.75AP 76AP 77AP 78AP . The “pressure” on electrons to flow from one electrode to the other in a battery is called the _________ of the battery.80AP 81AP 82AP 83AP . For each of the following unbalanced oxidation-reduction chemical equations, balance the equation by inspection, and identify which species is the reducing agent. a.Fe(s)+O2(g)Fe2O3(s)b.Al(s)+Cl2(g)AlCl3(s)c.Mg(s)+P4(s)Mg3P2(s)85AP 86AP 87AP . Balance each of the following oxidation-reduction reactions by inspection. a.C3H8(g)+O(g)CO2(g)+H2O(g)b.CO(g)+H2(g)CH3OH(l)c.SnO2(s)+C(s)Sn(s)+CO(g)d.C2H5OH(l)+O2(g)CO2(g)+H2O(g). Balance each of the following oxidation-reduction reactions, which take place in acidic solution. a.MnO4(aq)+H2O2(aq)Mn2+(aq)+O2(g)b.BrO3(aq)+Cu+(aq)Br(aq)+Cu2+(aq)c.HNO2(aq)+I(aq)NO(g)+I2(aq). For each of the following oxidation-reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a.4Na(s)+O2(g)2Na2O(s)b.Fe(s)+H2SO4(aq)FeSO4(aq)+H2(g)c.2Al2O3(s)4Al(s)+3O2(g)d.3Mg(s)+N2(g)Mg3N2(s). For each of the following oxidation-reduction reactions of metals with nonmetals, identify which element is oxidized and which is reduced. a.3Zn(s)+N2(g)Zn3N2(s)b.Co(s)+S(s)CoS(s)c.4K(s)+O2(g)2K2O(s)d.4Ag(s)+O(g)2Ag2O(s). Assign oxidation sates to all of the atoms in each of the following: a. NH3 b.CO C. CO2 d. NF3 . Assign oxidation states to all of the atoms in each of the lot lowing: a. PBr3 b. C3H8 c. KMnO4 d. CH3COOH 94AP 95AP . Assign oxidation states to all of the atoms in each of the following: a. BiO+ b.PO43-c.NO2d.Hg22+97AP . In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a.2Br2O3(s)+6Cl2(g)4BCl3(l)+3O2(g)b.GeH4(g)+O2(g)Ge(s)+2H2O(g)c.C2H4(g)+Cl2(g)C2H4Cl2(l)d.O2(g)+2F2(g)2OF2(g). Balance each of the following half-reactions. a.I(aq)I2(s)b.O2(g)O2(s)c.P4(s)P3(s)d.Cl2(g)Cl(aq)100AP 101AP 102AP . Consider the oxidation—reduction reaction Mg(s)+Cu2+(aq)Mg2+(aq)+Cu(s)Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?104AP 105CP 1CT 19.1SC 19.2SC Exercise19.3Watches with numerals that glow in the dark” formerly were made by including radioactive radium in the paint used to letter the watch faces. Assume that to make the numeral 3 on a given watch, a sample of paint containing8.0107 mole ofR88228a was used. This watch was then put in a drawer and forgotten. Many years later someone finds the watch and wishes to know when it was made. Analyzing the paint, this person finds1.0107 moles ofR88228a in the numeral 3. Flow much time elapsed between the making of the watch and the finding of the watch? Watches and clocks with radium dials.1CT 1ALQ 2ALQ 3ALQ 4ALQ 5ALQ 6ALQ 7ALQ 8ALQ 9ALQ 10ALQ 1QAP 2QAP 3QAP 4QAP 5QAP 6QAP 7QAP 8QAP 9QAP 10QAP 11QAP 12QAP 13QAP 14QAP 15QAP 16QAP 17QAP 18QAP 19QAP 20QAP 21QAP 22QAP 23QAP 24QAP 25QAP 26QAP 27QAP 28QAP 29QAP 30QAP 31QAP 32QAP 33QAP 34QAP 35QAP 36QAP 37QAP 38QAP 39QAP 40QAP 41QAP 42QAP 43QAP 44QAP 45QAP 46QAP 47QAP 48QAP . How do the forces that hold an atomic nucleus together compare in strength with the forces between atoms in a molecule?50QAP 51QAP 52QAP 53QAP 54QAP 55QAP 56QAP 57QAP 58QAP 59QAP

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