Question: Consider Fig. 14.10. Imagine you are
Consider Fig. 14.10. Imagine you are talking to a friend who has not taken any science courses, and explain how the figure demonstrates the concept of vapor pressure and enables it to be measured. From figure 14.10 
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Diethyl ather vapor -Vacuum -H;O vapor 24 mm Hg -Liquid H,O Original Hg leved 545 mm Hg Patm= 760 mm Hg 736 mm Hg Diethyl ether liquid 215 mm Hg- It is easy to measure the vapor pressure of a liquid by using a simple barometer of the type shown here. The water vapor pushed the mercury down 24 mm (760 - 736), so the vapor pressure of water is 24 mm Hg at this temperature. Diethyl ether is much more volatile than water and thus shows a higher vapor pressure. In this case, the mercury level has been pushed down 545 mm (760 – 215), so the vapor pressure of diethyl ether is 545 mm Hg at this temperature. Figure 14.10
> What is the total number of valence electrons in each of the following molecules? a. HNO3 b. H2SO4 c. H3PO4 d. HClO4
> When a person has a severe fever, one therapy to reduce the fever is an “alcohol rub.” Explain how the evaporation of alcohol from the person’s skin removes heat energy from the body.
> Consider the flasks in the following diagrams. Assuming the connecting tube has negligible volume, draw what each diagram will look like after the stopcock between the two flasks is opened. Also, solve for the final pressure in each case, in terms of t
> Which of the following statements is(are) true? a. At constant temperature, the lighter the gas molecules, the faster the average velocity of the gas molecules. b. At constant temperature, the heavier the gas molecules, the larger the average kinetic e
> 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. a. sodium, Na, and selenium, Se b. rubidium, Rb, and fluorine, F c. potas
> What is an alloy? Explain the differences in structure between substitutional and interstitial alloys. Give an example of each type.
> What is a network solid? Give an example of a network solid and describe the bonding in such a solid. How does a network solid differ from a molecular solid?
> During the making of steel, iron(II) oxide is reduced to metallic iron by treatment with carbon monoxide gas. FeO(s) + CO(g) / Fe(s) + CO2(g) Suppose 1.45 kg of Fe reacts. What volume of CO(g) is required, and what volume of CO2(g) is produced, each mea
> Explain the overall trend in the following melting points in terms of the forces among particles in the solids indicated. Hydrogen, H2………………….-259 °C Ethyl alcohol, C2H5OH………-114 °C Water, H2O……………………….…0 °C Sucrose, C12H22O11…………...186 °C Calcium chlo
> Describe in detail the microscopic processes that take place when a solid melts and when a liquid boils. What kind of forces must be overcome? Are any chemical bonds broken during these processes?
> In general terms, what is a chemical bond?
> 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. a. N-P or N-O b. N-C or N-O c. N-S or N-C d. N-F or N-S
> Dinitrogen monoxide, N2O, reacts with propane, C3H8, to form nitrogen, N2; carbon dioxide, CO2; and water, H2O. a. Write a balanced chemical equation for this reaction, treating all substances as gases. Include phases in your equation. b. Two reservoir
> A mixture contains 5.00 g each of O2, N2, CO2, and Ne gas. Calculate the volume of this mixture at STP. Calculate the partial pressure of each gas in the mixture at STP.
> The forces holding together a molecular solid are much (stronger/ weaker) than the forces between particles in an ionic solid.
> A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their prope
> Consider the following unbalanced chemical equation in which element X is unknown: X(s) + F2(g) ( XF3(s) If 9.15 g of element X(s) is completely reacted with 4.00 L of fluorine gas at 250 °C and 2.50 atm, what is the identity of X?
> Two molecules that contain the same number of each kind of atom but that have different molecular structures are said to be isomers of each other. For example, both ethyl alcohol and dimethyl ether (shown below) have the formula C2H6O and are isomers. Ba
> If water is added to magnesium nitride, ammonia gas is produced when the mixture is heated. Mg3N2(s) + 3H2O(l) 3MgO(s) + 2NH3(g) If 10.3 g of magnesium nitride is treated with water, what volume of ammonia gas would be co
> 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 ch
> Calcium carbide, CaC2, reacts with water to produce acetylene gas, C2H2. CaC2(s) + 2H2O(l) C2H2(g) + Ca(OH)2(s) What volume of acetylene at 25 °C and 1.01 atm is generated by the complete reaction of 2.49 g of calcium carbide? What
> Explain the difference between intramolecular and intermolecular forces.
> Ammonia and gaseous hydrogen chloride combine to form ammonium chloride. NH3(g) + HCl(g) NH4Cl(s) If 4.21 L of NH3(g) at 27 °C and 1.02 atm is combined with 5.35 L of HCl(g) at 26 °C and 0.998 atm, what mass of NH4Cl(s) will be produced
> For each of the following molecules, predict both the molecular structure and bond angles around the central atom. a. SeS2 b. SeS3 c. SO2 d. CS2
> Consider the following reaction for the combustion of octane, C8H18: 2C8H18(l) + 25O2(g) / 16CO2(g) + 18H20(l) What volume of oxygen gas at STP would be needed for the complete combustion of 10.0 g of octane?
> Which substance in each pair would be expected to be more volatile at a particular temperature? Explain your reasoning. a. H2O(l) or H2S(l) b. H2O(l) or CH3OH(l) c. CH3OH(l) or CH3CH2OH(l)
> Calcium oxide can be used to “scrub” carbon dioxide from air. CaO(s) + CO2(g) CaCO3(s) What mass of CO2 could be absorbed by 1.25 g of CaO? What volume would this CO2 occupy at STP?
> Using the VSEPR theory, predict the molecular structure of each of the following polyatomic ions. a. dihydrogen phosphate ion, H2PO4- b. perchlorate ion, ClO4- c. sulfite ion, SO32-
> Which substance in each pair would be expected to have a lower boiling point? Explain your reasoning. a. CH3OH or CH3CH2CH2OH b. CH3CH3 or CH3CH2OH c. H2O or CH4
> Explain, in terms of the kinetic molecular theory, how an increase in the temperature of a gas confined to a rigid container causes an increase in the pressure of the gas.
> How is the phenomenon of temperature explained on the basis of the kinetic molecular theory? What microscopic property of gas molecules is reflected in the temperature measured?
> Consider the following molecules: CH3OH, CH4, H2O, C2H6. a. Draw the Lewis structure for each molecule, and indicate whether each is polar or nonpolar. b. At room temperature, two of these compounds exist as a liquid, and two of these compounds exist a
> What 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.
> For the indicated atom in each of the following molecules or ions, give the number and arrangement of the electron pairs around that atom. a. As in AsO43- b. Se in SeO42- c. S in H2S
> Small quantities of hydrogen gas can be prepared in the laboratory by the addition of aqueous hydrochloric acid to metallic zinc. Zn(s) + 2HCl(aq) ZnCl2(aq) + H2(g) Typically, the hydrogen gas is bubbled through water for collection and
> Although the valence electron pairs in ammonia have a tetrahedral arrangement, the overall geometric structure of the ammonia molecule is not described as being tetrahedral. Explain.
> Suppose that 1.28 g of neon gas and 2.49 g of argon gas are confined in a 9.87-L container at 27 °C. What would be the pressure in the container?
> If a gaseous mixture is made of 2.41 g of He and 2.79 g of Ne in an evacuated 1.04-L container at 25 °C, what will be the partial pressure of each gas and the total pressure in the container?
> What general principles determine the molecular structure (shape) of a molecule?
> We often collect small samples of gases in the laboratory by bubbling the gas into a bottle or flask containing water. Explain why the gas becomes saturated with water vapor and how we must take the presence of water vapor into account when calculating t
> Determine the partial pressure of each gas as shown in this figure. Note: The relative numbers of each type of gas are depicted in the figure. 1.00 atm о Не Ne Ar
> Explain why the measured properties of a mixture of gases depend only on the total number of moles of particles, not on the identity of the individual gas particles. How is this observation summarized as a law?
> What mass of neon gas would be required to fill a 3.00-L flask to a pressure of 925 mm Hg at 26 °C? What mass of argon gas would be required to fill a similar flask to the same pressure at the same temperature?
> What evidence do we have that the solid form of water is less dense than the liquid form of water at its freezing/melting point?
> A tank contains a mixture of 52.5 g of oxygen gas and 65.1 g of carbon dioxide gas at 27 °C. The total pressure in the tank is 9.21 atm. Calculate the partial pressure (in atm) of each gas in the mixture.
> 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. a. c
> 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. a. c
> 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. a. c
> 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. a. s
> What do we mean by a dynamic equilibrium? Describe how the development of a vapor pressure above a liquid represents such an equilibrium.
> In carbon compounds a given group of atoms can often be arranged in more than one way. This means that more than one structure may be possible for the same atoms. For example, both the molecules diethyl ether and 1-butanol have the same number of each ty
> 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. a. C2H6 b. NF3 c. C4H10 d. SiCl4
> 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. a. H2S b. SiF4 c. C2H4 d. C3H8
> Compare and contrast the bonding found in the H2 (g) and HF(g) molecules with that found in NaF(s).
> 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. a. NBr3 b. HF c. CBr4 d. C2H2
> Give the total number of valence electrons in each of the following molecules. a. B2O3 b. CO2 c. C2H6O d. NO2
> Give the total number of valence electrons in each of the following molecules. a. N2O b. B2H6 c. C3H8 d. NCl3
> If you’ve ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopic basis how a vapor pressure builds up in a closed con
> What mass of helium gas is needed to pressurize a 100.0-L tank to 255 atm at 25 °C? What mass of oxygen gas would be needed to pressurize a similar tank to the same specifications?
> Given each of the following sets of values for an ideal gas, calculate the unknown quantity. a. P = 782 mm Hg; V =? n = 0.210 mol; T = 27 °C b. P =? mm Hg; V = 644 mL; n = 0.0921 mol; T = 303 K c. P = 745 mm Hg; V = 11.2 L; n = 0.401 mol; T =? K
> Show how Charles’s gas law can be derived from the ideal gas law.
> Show how Boyle’s gas law can be derived from the ideal gas law.
> What do we mean by an ideal gas?
> Explain what the “duet” and “octet” rules are and how they are used to describe the arrangement of electrons in a molecule.
> Consider a sample of ice being heated from -5 °C to +5 °C. Describe on both a macroscopic and a microscopic basis what happens to the ice as the temperature reaches 0 °C.
> Given the following sets of values for three of the gas variables, calculate the unknown quantity. a. P = 782.4 mm Hg; V = ?; n = 0.1021 mol; T = 26.2 °C b. P = ? mm Hg; V = 27.5 mL; n = 0.007812 mol; T = 16.6 °C c. P = 1.045 atm; V = 45.2 mL; n = 0.00
> For each of the following pairs, indicate which is larger. a. I or F b. F or F- c. Na+ or F-
> For each of the following pairs, indicate which is smaller. a. Fe or Fe3+ b. Cl or Cl- c. Al3+ or Na+
> For each of the following pairs, indicate which species is larger. Explain your reasoning in terms of the electron structure of each species. a. Mg2+ or Mg b. Ca2+ or K+ c. Rb+ or Br- d. Se2- or Se
> For each of the following pairs, indicate which species is smaller. Explain your reasoning in terms of the electron structure of each species. a. H or H- b. N or N3- c. Al or Al3+ d. F or Cl
> When dry ammonia gas (NH3) is bubbled into a 125-mL sample of water, the volume of the sample (initially, at least) decreases slightly. Suggest a reason for this.
> Ionic solids are generally considerably harder than most molecular solids. Explain.
> Describe in general terms the structure of ionic solids such as NaCl. How are the ions packed in the crystal?
> How do ionic solids differ in structure from molecular solids? What are the fundamental particles in each? Give two examples of each type of solid and indicate the individual particles that make up the solids in each of your examples.
> On the basis of the smaller units that make up the crystals, cite three types of crystalline solids. For each type of crystalline solid, give an example of a substance that forms that type of solid.
> Describe a simple mercury barometer. How is such a barometer used to measure the pressure of the atmosphere?
> Why are the dipole–dipole interactions between polar molecules not important in the vapor phase?
> What mass of neon gas is required to fill a 5.00-L container to a pressure of 1.02 atm at 25 °C?
> If two gases that do not react with each other are placed in the same container, they will completely with each other.
> If 2.71 g of argon gas occupies a volume of 4.21 L, what volume will 1.29 moles of argon occupy under the same conditions?
> If 3.25 moles of argon gas occupies a volume of 100. L at a particular temperature and pressure, what volume does 14.15 moles of argon occupy under the same conditions?
> 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. a. aluminum and bromine b. aluminum and oxygen c. aluminum and phosphorus
> If 0.00901 mole of neon gas at a particular temperature and pressure occupies a volume of 242 mL, what volume would 0.00703 mole of neon occupy under the same conditions?
> If 5.12 g of oxygen gas occupies a volume of 6.21 L at a certain temperature and pressure, what volume will 25.0 g of oxygen gas occupy under the same conditions?
> If a 0.475-L sample of neon gas is heated from 27 °C to 82 °C at constant pressure, what will be the volume of the sample at the higher temperature?
> If a gaseous mixture is made of 3.50 g of He and 5.75 g of Ar in an evacuated 2.05-L container at 25 °C, what will be the partial pressure of Ar in the container?
> An expandable vessel contains 729 mL of gas at 22 °C. What volume will the gas sample in the vessel have if it is placed in a boiling water bath (100. °C)?
> A sample of a gas at 0.780 atm occupies a volume of 0.501 L. If the temperature remains constant, what will be the new pressure if the volume increases to 0.794 L?
> If the pressure on a 2.10 * 104 mL sample of gas is doubled at constant temperature, what will be the new volume of the gas?
> Convert the following pressures into mm Hg. a. 0.903 atm b. 2.1240 * 106 Pa c. 445 kPa d. 342 torr
> If 0.214 mole of argon gas occupies a volume of 652 mL at a particular temperature and pressure, what volume would 0.375 mole of argon occupy under the same conditions?
> If 10.0 g of liquid helium at 1.7 K is completely vaporized, what volume does the helium occupy at STP?
> 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. a. aluminum, Al, and sulfur, S b. radium, Ra, and oxygen, O c. calcium,
> At what temperature does 4.00 g of helium gas have a pressure of 1.00 atm in a 22.4-L vessel?
> Suppose two separate 100.0-L tanks are to be filled, one with helium and one with hydrogen. What mass of each gas is needed to produce a pressure of 2.70 atm in its respective tank at 24 °C?
> What is the pressure inside a 10.0-L flask containing 14.2 g of N2 at 26 °C?
> You have 1 mole of an ideal gas in a balloon. How must the volume change so that the pressure in the balloon doubles and the temperature in °C is halved (assume the temperature is a positive value)? a. The volume must decrease by more than half the orig
> Carbon dioxide gas, in the dry state, may be produced by heating calcium carbonate. CaCO3(s) / CaO(s) + CO2(g) What volume of CO2, collected dry at 55 °C and a pressure of 774 torr, is produced by complete thermal decomposition of 10.0 g of CaCO3?
> The 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. Formula Compound Name Molecular Structure CO, NH3 SO3 H,0 ClO,-
> Which of the following compounds or ions exhibit resonance? a. O3 b. CNO- c. AsI3 d. CO32- e. AsF3
