Skip to main content

Bartleby Sitemap - Textbook Solutions

All Textbook Solutions for Introductory Chemistry: A Foundation

n general terms, what is a covalent bond?escribe the type of bonding that exists in the Cl2(g)molecule. How does this type of bonding differ from that found in the HCl(g)molecule? How is it similar?6QAP he relative ability of an atom in a molecule to attract electrons to itself is called the atom’s .hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.9QAP What factor determines the relative level of polarity of a polar covalent bond?In each of the following groups, which element is the most electronegative? Which is the least electronegative? msp;a.K,Na,Hb.F,Br,Nac.B,N,F In each of the following groups. which element is the most electronegative? Which is the least electronegative? msp;a.Cs,Ba.Atb.Ba,Sr,Rac.O,Rb,Mg On the basis. of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic. covalent, or polar covalent. O—O Al—O B—0 On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be covalent, polar covalent, or ionic. msp;a.SSb.SHc.SK Which of the following molecules contain polar covalent hands? msp;a.water,H20c.fluorine,F2b.carbonmonoxide,COd.nitrogen,N2 Which of the following molecules contain polar covalent bonds? msp;a.phosphorus,P4c.ozone,O3b.oxygen,O2d.hydrogenfluoride,HF On the basis of the electronegativity values given in Fig. 12.3, indicate which is the more polar bond in each of the following pairs. msp;a.HForHClc.HBrorHClb.HClorHId.HIorHBr On the basis of the electronegativity values given in Fig. 12.3. indicate which is the more polar bond in each of the following pairs. msp;a.OClorOBrc.PSorPOb.NOorNFd.HOorHN Which brand in each of the following pairs has the greater ionic character? msp;a.NaForNaIb.LiClorCsClc.CaSorC0d.MgNorMgP Which hand in each of the following pairs has less ionic character? msp;a.NaOorNaNc.NaClorKClb.KS0rKPd.NaClorMgCl What is a dipole moment? Give four examples of molecules that possess dipole moments, and draw the direction of the dipole as shown in Section 12.3.Why is the presence of a dipole moment in the water molecule so important? What are some properties of water that are determined by its polarity?In each of the following diatomic molecules, which end of the molecule is negative relative to the other end? msp;a.hydrogenchloride,HClb.carbonmonoxide,COc.brominemonofluoride.BrF In each of the following diatomic molecules. which end of the molecule is positive relative to the other end? msp;a.hydrogenfluoride,HFb.chlorinemonofluorideClFc.iodinemonofluorideICl For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which and of the bond is positive and which is negative. msp;a.CFc.COb.SiCd.BC For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. msp;a.SPc.SClb.SFd.SBr For each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. msp;a.SiHc.SHb.PHd.ClH For each of the following bonds, draw a figure indicating the direction of the bond dipole. including which end of the bond is positive and which is negative. msp;a.HCc.NSb.NOd.NC What does it mean when we say that in forming bonds, atoms try to achieve an electron configuration analogous to a noble gas?30QAP Nonmetals form negative ions by (losing/gaining) enough electrons to achieve the electron configuration of the next noble gas.Explain how the atoms in covalent molecules achieve electron configurations similar to those of the noble gases. How does this differ from the situation in ionic compounds?Which simple ion would each of the following elements he expected to form? What noble gas has an analogous electron configuration to each of the inns? msp;a.chlorine,Z=17b.strontium,Z=38c.oxygen,Z=8d.rubidium,Z=37 Which simple ion would each of the following elements be expected to form? Which noble gas has an analogous electron configuration to each of the ions? msp;a.bromine,Z=35b.cesium,Z=55c.phosphorus,Z=15d.sulfur,Z=16 For each of the following numbers of electrons, give the formula of a positive ion that would have that number of electros, and write the complete electros configuration for each ion. msp;a.10electronsc.18electronsb.2electronsd.36electrons What is the expected ground—state electron configuration for Te2-?On the basis of their electron configurations, predict the formula of the simple binary ionic compounds likely to form when the following pairs of elements react with each other. aluminum, Al, and sulfur, S radium, Ra, and oxygen, O calcium, Ca, and fluorine, F cesium, Cs, and nitrogen, N rubidium. Rb, and phosphorus. P On the basis of their electron configurations, predict the formula of the simple binary ionic compound likely to form when the following pairs of elements react with each other. aluminum and bromine aluminum and oxygen aluminum and phosphorus aluminum and hydrogen Name the noble gas atom that has the same electron configuration as each of the ions in the following compounds. msp;a.bariumsulfide,BaSb.strontiumfluoride,SrF2c.magnesiumoxide,MgOd.aluminumsulfide,Al2S3 Atoms form ions so as to achieve electron configurations similar to those of the noble gases. For the following pairs of noble gas configurations, give the formulas of two simple ionic compounds that would have comparable electron configurations. msp;a.[He]and[Ne]c.[He]and[Ar]b.[Ne]and[Ne]d.[Ne]and[Ar]41QAP Describe in general terms the structure of ionic solids such as NaCl. How are the ions packed in the crystal?Why are cations always smaller than the atoms from which they are formed?Why are anions always larger than the atoms from which they are formed?For each of the following pairs, indicate which species is smaller. Explain your reasoning in terms of the electron structure of each species. msp;a.HorHc.AlorAl3+b.NorN3d.ForCl 46QAP 47QAP For each of the following pairs, indicate which is larger. msp;a.IorFb.ForFc.Na+orF Why are the valence electrons of an atom the only electrons likely to be involved in bonding to other moms?Explain what the “duet" and “octet” rules are and how they are used to describe the arrangement of electrons in a molecule.What type of structure must each atom in a compound usually exhibit for the compound to be stable?When elements in the second and third periods occur in compounds, what number of electrons in the valence shell represents. the mast stable electron arrangement? Why?How many electrons are involved when two atoms in a molecule are connected by a “double bond”? Write the Lewis structure of a molecule containing a double bond.54QAP Write the simple Lewis structure for each of the following atoms. msp;a.I(Z=53)c.Xe(Z=54)b.Al(Z=13)d.Sr(Z=38)Write the simple Lewis structure for each of the following atoms. msp;a.Mg(Z=12)c.S(Z=16)b.Br(Z=35)d.Si(Z=14)Give the total number of valence electrons in each of the following molecules. msp;a.N2Oc.C3H8b.B2H6d.NC13 Give the total number of valence electrons in each of the following molecules. msp;a.B2O3c.C2H6Ob.CO2d.NO2 Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. msp;a.NBr3c.CBr4b.HFd.C2H2 Write a Lewis structure for each of the following simple molecules. Show all bonding valence electrons pairs as lines and all nonbonding valence electron pairs as dots. msp;a.H3Sc.C2H4b.SiF4d.C3H8 Write a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. msp;a.C2H6d.C4H10b.NF3d.SiCl4 Which of the following species exhibits resonance? msp;CH4,OCl2,NO2,HCN(C is the central atom)The “Chemistry in Focus“ segment Broccoli—Miracle Food? discusses the health benefits of eating broccoli and gives a Lewis structure for sulforaphane, a chemical in broccoli. Draw possible resonance structures for sulforaphane.The “Chemistry in Focus" segment Hiding Carbon Dioxide- discusses attempts at sequestering (storing) underground CO2produced at power plants so as to diminish the: greenhouse effect. Draw all resonance structures of the CO2molecule.Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the: various possible resonance forms. msp;a.sulfateion,SO42b.phosphateion,PO43c.sulfiteion,SO32 Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. msp;a.chlorateion,ClO3b.peroxideion,O22c.acetateion,C3H3O2 Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. msp;a.chlorineion,C1O2b.perbromateion,BrO4c.cyanideion,CN Write a Lewis structure for each of the following polyatomic ions. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those ions that exhibit resonance, draw the various possible resonance forms. msp;a.carbonateion,CO32b.ammoniumion,NH4+c.hypochloriteion,ClO What is the geometric structure of the water molecule? How many pairs of valence electrons are there on the oxygen atom in the water molecule? What is the approximate HOHbond angle in water?What is the geometric sanctum of the ammonia molecule? How many pairs of electrons surround the nitrogen atom in NH3? What is the approximate HNHbond angle in ammonia?What is the geometric structure of the boron trifluoride moleCule, BF3? How many pairs of valence electrons are present on the boron atom in BF3? What are the approximate FBFbond angles in BF3?What is the geometric structure of the SiF4molecule? How many pairs of valence electrons are present on The silicon atom of SiF4? What are the approximate FSiFbond angles in SiF4?Why is the geometric structure of a molecule important, especially for biological molecules?74QAP How is the structure around a given atom related to repulsion between valence electron pairs on the atom?Why are all diatomic molecules linear, regardless of the number of valence electron pairs on the atoms involved?Although the valence electron pairs in ammonia have a tetrahedral arrangement me overall geometric structure of the ammonia molecule is not described as being tetrahedral. Explain.Although both the BF3and NF3molecules contain the same number of atoms, the BF3molecule is flat, whereas the NF3molecule is trigonal pyramidal. Explain.For the indicated atom in each of the following molecules or ions. give the number and arrangement of the electron pairs around that atom. msp;a.AsinA3O43b.SeinSeO42c.SinH2S 80QAP Using the VSEPR theory, predict the molecular structure of each of the following molecules. :math>a.NCl3b.H2Sec.SiCl4 82QAP Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions. msp;a.sulfateion,SO42b.phosphateion,PO43c.ammoniumion,NH4+Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions. msp;a.dihydrogenphosphateion,H2PO4b.perchlorateion,ClO4c.sulfiteion.SO32 For each of the following molecules or ions, indicate the bond angle expected between the central atom and any two adjacent hydrogen atoms. msp;a.H2Ob.NH3c.NH4+d.CH4 For each of the following molecules or ion. indicate the bond angle expected between the central atom and any two adjacent chlorine atoms. msp;a.Cl2Ob.NC13c.CCl4d.C2Cl4 The “Chemistry in Focus" segment Taste—It's the Structure That Counts discusses artificial sweeteners. What are the expected bond angles around the nitrogen atom in aspartame?88QAP 89AP In ionic bonding, the electrons are shared between the atoms. the process of fanning an ionic bond is highly endothermic overall. the bonding that occurs is usually between two nonmetal atoms. a noble gas configuration is fanned far each element or ion. At least two of the above statements are correct.The geometric arrangement of electron pairs around a given atom is determined principal by the tendency to minimize between the electron pairs.92AP 93AP Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. In an N—O bond. electron density is greater near the O atom. An N—O bond is an example of a polar covalent band. In general, chemical bonds form to minimize energy. The bond in KBr is formed by sharing electrons.95AP For each of the following pairs of elements, identify which element would be expected to be more electronegative. It should not be necessary to look at a table of actual electronegativity values. msp;a.BeorBab.NorPc.ForCl On the basis of the electronegativity values given in Fig. 12.3, indicate whether each of the following bonds would be expected to be ionic, covalent, or polar covalent. msp;a.HOc.HHb.OOd.HCl Which of the following molecules contain polar covalent hands? carbon monoxide, CO chlorine, Cl2 iodine monochloride, ICl phosphorus, P4 99AP 100AP or each of the following bonds, draw a figure indicating the direction of the bond dipole, including which end of the bond is positive and which is negative. msp;a.NClc.NSb.NPd.NC 102AP 103AP 104AP hich noble gas has the same electron configuration as each of the ions in the following compounds? msp;a.calciumbromide,CaBr2b.aluminumselenide,Al2Se3c.strontiumoxide,SrOd.potassiumsulfide,K2S 106AP rite the Lewis structure for each of the following atoms. msp;a.He(Z=2)d.Ne(Z=10)b.Br(Z=35)e.I(Z=53)c.Sr(Z=38)f.Ra(Z=88)108AP rite a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. msp;a.GeH4c.NI3b.ICld.PF3 110AP rite a Lewis structure for each of the following simple molecules. Show all bonding valence electron pairs as lines and all nonbonding valence electron pairs as dots. For those molecules that exhibit resonance, draw the various possible resonance forms. msp;a.SO2b.N2O(Nincenter)c.O3 112AP hy is the molecular structure of H2Ononlinear, whereas that of BeF2is linear, even though both molecules consist of three atoms?114AP sing the VSEPR theory, predict the molecular structure of each of the following molecules. msp;a.C12Ob.OF2c.SiCl4 116AP or each of the following molecules, indicate the bond angle expected between the central atom and any two adjacent chlorine atoms. msp;a.C12Oc.BeCl2b.CCl4d.BCl3 118AP 119AP 120AP 121AP Classify the bonding in each of the following molecules as ionic, polar covalent, or nonpolar covalent. a.H2d.SO2g.CF4b.K3Pe.HFh.K2Sc.NaIf.CCl4 ompare the electronegativities of each pair of atoms. State the element of each pair that has the greater electronegativily. l> Pair Symbol for Element with Greater Electronegativity msp;PandCl msp;CaandN msp;NandAs 124CP rrange the atoms and/or ions in the following groups in order of decreasing size. msp;a.O,O,O2b.Fe2+,Ni2+,Zn2+c.Ca+,K+,Cl 126CP 127CP he formulas of several chemical substances are given in the table below. For each substance in the table, give its chemical name and predict its molecular structure. l> Formula Compound Name Molecular Structure msp;CO2 msp;NH3 msp;SO3 msp;H2O msp;ClO4 1CR hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?3CR 4CR 5CR hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?7CR 8CR 9CR What is a driving force? Name two common and important driving forces, and give an example of each. What is entropy? Although the total energy of the universe is constant, is the entropy of the universe constant? What is a spontaneous process?11CR Methane, CH4, is the major component of natural gas. Methane burns in air, releasing approximately 890kJof heat energy per mole. msp;CH4(g)+2O2(g)CO2(g)+2H2(g) What quantity of heat is released if 0.521moleof methane is burned? What quantity of heat is released if 1.25gof methane is burned? What quantity of methane must have reacted if 1250kJof heat energy was released?What is electronegative radiation? Give some examples of such radiation. Explain what the wavelength ( ) and frequency (v) of electronegative radiation represent. Sketch a representation of a wave and indicate on your drawing one wavelength of the wave. At what speed does electromagnetic radiation move through space? How is this speed related to and v?14CR Do atoms in excited states emit radiation randomly, at any wavelength? Why? What does it mean to say that the hydrogen atom has only certain discrete energy levels available? How do we know this? Why was the quantization of energy levels surprising to scientists when it was first discovered?16CR Schrodinger and de Broglie suggested a ‘Wave—particle duality" for small particles—that is, if electromagnetic radiation showed some particle-like properties, then perhaps small punicles might exhibit same wave-like properties. Explain. How does the wave mechanical picture of the atom fundamentally differ from the Bohr model? How do wave mechanical arbitals differ from Bohr’s orbits? What does it mean to say that an orbital represents a probability map for an electron?Describe the general characteristics of the first (lowest-energy) hydrogen atomic orbital. How is this orbital designated symbolically? Does this orbital have a sharp “edge"? Does the orbital represent a surface upon which the electron travels at all times?19CR Describe the sublevels and orbitals that constitute the third and fourth principal energy levels of hydrogen. How is each of the orbitals designated and what! are the general shapes of their probability maps?Describe electron spin. How does electron spin affect the total number of electrons that can be accommodated in a given orbital? What does the Pauli exclusion principle tell us about electrons and their spins?22CR List the order in which the orbitals are filled as the atoms beyond hydrogen are built up. How many electrons overall can be accommodated in the first and second principal energy levels? How many electrons can be placed in a given s subshell? In a given p subshell? In a specific p orbital? Why do we assign unpaired electrons in the 2p orbitals of carbon, nitrogen, and oxygen?24CR 25CR 26CR What are the representative elements? In what region(s) of the periodic table are these elements found? In what general area of the periodic table are the metallic elements found? In what general area of the table are the nonmetals found? When in the table are the metalloids located?28CR 29CR 30CR 31CR 32CR 33CR 34CR Give evidence that ionic bonds are very strong. Does an ionic substance contain discrete molecules? With what general type of structure do ionic compounds occur? Sketch a representation of a general structure for an ionic compound. Why is a cation always smaller and an anion always larger than the respective parent atom? Describe the bonding in an ionic compound containing polyatomic ions.36CR 37CR For three simple molecules of your own choice, apply the rules for writing Lewis structures. Write your discussion as if you are explaining the method to someone who is not familiar with Lewis structures.39CR 40CR 41CR 42CR 43CR 44CR 45CR 46CR Which of the following statements is correct and provides the best explanation when removing the first two electrons from calcium? Energy is released when either electron comes off because calcium is a metal and not very electronegative. It takes less energy to remove the second electron from calcium compared with the first because calcium wants to have eight electrons in its outer shell (and thus have a noble gas configuration. It takes less energy to remove the first electron compared with the second because it is in a higher energy level than the second electron. Electrons cannot be removed from calcium because it is a metal and only wants to gain electrons to become more stable. It takes more energy to remove the second electron compared with the first because the nucleus binds the electrons more tightly as each electron is removed.Hydrogen gas and oxygen gas react violently to form water. When this occurs, a very loud noise is heard. Draw the Lewis structures for hydrogen gas, oxygen gas, and water. State whether each molecule is polar or nonpolar and why. Explain how the polarity of these molecules is related to hydrogen and oxygen existing in the gas phase at room temperature and water existing in the liquid phase at room temperature. Which is lower in energy for this reaction a mixture of hydrogen and oxygen gases or water? How do you know this is true?13.1SC 13.2SC 1CT trong>Exercise 13.3 A child blows a bubble that contains air at 28Cand has a volume of 23cm3at I atm. As the bubble rises, it encounters a pocket of cold air (temperature 18C). If there is: no change in pressure, will the bubble get larger or smaller as the air inside cools to 18C? Calculate the new volume of the bubble.13.4SC trong>Exercise 13.5 A weather balloon contains 1.10105molesof He and has a volume of 2.70106Lat 1.00atmpressure. Calculate the temperature of the helium in the balloon in kelvins and in Celsius degrees.13.6SC 13.7SC trong>Exercise 13.8 A sample of argon gas with a volume of 11.0Lat a temperature of 13Cand a pressure of 0.747atm is heated to 56Cand a pressure of 1.18atm. Ca1culate the final volume.13.9SC 13.10SC 1CT trong>Exercise 13.11 Calculate the volume of hydrogen produced at 1.50atmand 19Cby the reaction of 26.5gof zinc with excess hydrochloric acid according to the balanced equation msp;Zn(s)+2HCl(aq)ZnCl2(aq)+H2(g)at if STP was defined as normal room temperature (22C)and 1atm? How would this affect the molar volume of an ideal gas? Include an explanation and a number.13.12SC 1ALQ 2ALQ 3ALQ 4ALQ 5ALQ 6ALQ 7ALQ 8ALQ 9ALQ 10ALQ 11ALQ 12ALQ 13ALQ Draw molecular—level views than show the differences among solids, liquids, and gases.15ALQ 16ALQ 17ALQ 18ALQ 19ALQ 20ALQ You are holding two balloons of the same volume. One balloon contains 1.0gof helium. The other balloon contains neon. Calculate the mass of neon in the balloon?22ALQ 23ALQ The introduction to this chapter says that "we live immersed in a gaseous solution.” What dues. that mean?2QAP 3QAP 4QAP 5QAP 6QAP 7QAP 8QAP 9QAP 10QAP Make the indicated pressure conversions. msp;a.1.54105Patoatmospheresb.1.21atmtopascalsc.97,345PatommHgd.1.32kPatopascals 12QAP 13QAP 14QAP 15QAP 16QAP 17QAP 18QAP 19QAP 20QAP 21QAP 22QAP 3. A sample of helium gas with a volume of :math>29.2mLat 735mmHgis compressed at constant temperature until its volume is 15.1mL. What will be the new pressure in the sample?24QAP 25QAP 26QAP 27QAP 28QAP A sample of gas in a balloon has an initial temperature of 13Cand a volume at 1340L. If the temperature changes to 87Cand there is no overall change of pressure or amount of gas, what is the new volume of the gas?Suppose a 375mLsample of neon gas at 78Cis cooled to 22Cat constant pressure. What will be the new volume of the neon sample?For each of the following sets of volume/temperature data, calculate the missing quantity after the change is made. Assume that the pressure and the amount of gas remain the same. V=2.03Lat24C;V=3.0lLat?C V=l27mLat273K;V=?mLat373K V=49.7mLat34C;V=?at350K For each of the following sets of volume/temperature data, calculate the missing quantity. Assume that the pressure and the mass of gas remain constant. V=25.0Lat0C;V=50.0Lat?C V=247mLat25C;V=255mLat?C V=l.00mLat2272C;V=?at25C 33QAP 34QAP Suppose 1.25Lof argon is cooled from 291Kto 78K. What will be the new 1mlumfs 0f the argon sample?Suppose a 125mLsample of argon is cooled from 450Kto 250Kat constant pressure. What will be the volume of the sample at the lower temperature?37QAP 38QAP 39QAP 40QAP 41QAP If :math>1.04gof chlorine gas occupies a volume of 872mLat a particular temperature and pressure, what volume will 2.08gof chlorine gas occupy under the same conditions?If 3.25moles of argon gas occupies a volume of 100.Lat a particular temperature and pressure, what volume does 14.15moles of argon occupy under the same conditions?44QAP 45QAP 46QAP 47QAP 48QAP 49QAP 50QAP 51QAP Determine the pressure in a 125Ltank containing 56.2kgof oxygen gas at 21C.53QAP 54QAP 55QAP Suppose that a 1.25gsample of neon gas is confined in a 10.1Lcontainer at 25C. What will be the pressure in the container? Suppose the temperature is then raised 50C. What will me new pressure he after the temperature is increased?At what temperature will a 1.0gsample of neon gas exert a pressure of 500torr in a 5.0Lcontainer?58QAP What pressure exists in a 200Ltank containing 5.0kgof neon gas. at 300.K?60QAP Suppose a 24.3mLsample of helium gas at 25Cand 1.01atm is heated to :math>50.Cand compressed to a volume of 15.2mL. What will be the pressure of the sample?62QAP 63QAP 64QAP 65QAP 66QAP 67QAP Suppose than 1.28gof neon gas and 2.49gof argon gas. Are confined in a 9.87Lcontainer at 27C. What would be the pressure in the container?A tank contains a mixture of 52.5gof oxygen gas and 65.1gof carbon dioxide gas at 27C. The total pressure in the tank is 9.21 am. Calculate the partial pressure (in arm) of each gas in the mixture.What mass of new gas would but required to fill a 3.00Lflask to a pressure of 925mmHgat 26C? What mass of argon gas would be required to fill a similar flask to the same pressure at the same temperature?71QAP 72QAP A 500mLsample of O2gas at 24Cwas prepared by decomposing a 3aqueous solution of hydrogen peroxide, H3O2, in the presence of a small amount of manganese catalyst by the reaction msp;2H2O2(aq)2H2O(g)+O2(g) e oxygen mus. prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2in the mixture? How many moles of O2are in the mixture? (The vapor pressure of water at 24Cis 23mmHg.)74QAP 75QAP 76QAP 77QAP 78QAP 79QAP 80QAP 81QAP 82QAP 83QAP 84QAP Calcium oxide can be used to “scrub" carbon dioxide from air. msp;CaO(s)+CO2(g)CaCO3(s) at mass of CO2could he absorbed by 1.25gof CaO? What volume would this CO2occupy an STP?Consider the following reaction: msp;C(s)+O2(g)CO2(g) at volume of oxygen gas at 25 °C and 1.02atm would be required to react completely with 1.25gof carbon?Consider the following reaction for the combustion of octane, C8H18: msp;2C8H18(l)+25O2(g)16CO2(g)+18H2O(l) at volume of oxygen gas at STP would be needed for the complete combustion of 10.0gof octane?Although we: generally think of combustion reactions as involving oxygen gas, other rapid oxidation reactions are also referred to as combustions. For example, if magnesium metal is placed into chlorine gas, a rapid oxidation takes place, and magnesium chloride is produced. msp;Mg(s)+Cl2(g)MgCl2(s) at Volume of chlorine gas, measured at STP, is required to react completely with 1.02gof magnesium?m>89. Ammonia and gaseous hydrogen chloride combine to form ammonium chloride. em> msp;NH3(g)+HCl(g)NH4Cl(s) 4.2lLof NH3(g)at 27Cand 1.02mmis combined with 5.35Lof HCl(g)at 26Cand 0.998arm, what mass of NH4Cl(s)will be produced? Which gas is the limiting reactant? Which gas is present in excess?

Page: [1][2][3][4][5][6][7][8][9][10][11]