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Questions and Answers of Chemical Principles

What do we mean when we say that a liquid is volatile? Do volatile liquids have large or small vapor pressures at room temperature? What strengths of intermolecular forces occur in highly volatile
A substance has the following properties:Sketch a heating curve for the substance, starting at \(-50^{\circ} \mathrm{C}\). AHvap AHfus bp mp 20 kJ/mol 5.0 kJ/mol 75C -15C C(s) Specific Heat
Given the data in Exercise 87 on substance X, calculate the energy that must be removed to convert 250 . g of substance \(\mathrm{X}\) from a gas at \(100 .{ }^{\circ} \mathrm{C}\) to a solid at
How much energy does it take to convert \(0.500 \mathrm{~kg}\) of ice at \(-20 .{ }^{\circ} \mathrm{C}\) to steam at \(250 .{ }^{\circ} \mathrm{C}\) ? Specific heat capacities: ice, \(2.1 \mathrm{~J}
A \(20.0 \mathrm{~g}\) sample of ice at \(-10.0^{\circ} \mathrm{C}\) is mixed with \(100.0 \mathrm{~g}\) of water at \(80.0^{\circ} \mathrm{C}\). Calculate the final temperature of the mixture
Silver crystallizes in a cubic closest packed structure. The radius of a silver atom is 1.44 Å (144 pm). Calculate the density of solid silver.
Using the plots in Fig. 16.48(b), determine whether water or diethyl ether has the smaller enthalpy of vaporization.Figure 16.48(b) In (Pvap) (b) Water 1/T (K) -Diethyl ether -Ethanol
A solution was prepared by adding 20.0 g of urea to 125 g of water at 25°C, a temperature at which pure water has a vapor pressure of 23.76 torr. The observed vapor pressure of the solution was
A solution was prepared by dissolving 18.00 g of glucose in 150.0 g of water. The resulting solution was found to have a boiling point of 100.34°C at 1 atm. Calculate the molar mass of glucose.
What mass of ethylene glycol (C2H6O2), the main component of antifreeze, must be added to 10.0 L of water to produce a solution for use in a car’s radiator that freezes at –10.0°F (–23.3°C)?
To determine the molar mass of a certain protein, 1.00 × 10–3 g of the protein was dissolved in enough water to make 1.00 mL of solution. The osmotic pressure of this solution was found to be 1.12
What concentration of sodium chloride in water is needed to produce an aqueous solution isotonic with blood (π = 7.70 atm at 25°C)?
The observed osmotic pressure for a 0.10 M solution of Fe(NH4)2(SO4)2 at 25°C is 10.8 atm. Compare the expected and experimental values for i.
In a lab you need at least \(100 \mathrm{~mL}\) of each of the following solutions. Explain how you would proceed by using the given information.a. \(2.0 \mathrm{~m} \mathrm{KCl}\) in water (density
a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide.b. Based on your answers to part a, which ion, \(\mathrm{Cl}^{-}\)or \(\mathrm{I}^{-}\), is
What factors cause one solute to be more strongly hydrated than another? For each of the following pairs, predict which substance would be more soluble in water.a. \(\mathrm{CH}_{3} \mathrm{CH}_{2}
Glycerin \(\left(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{3}ight)\) is a nonvolatile liquid. What is the vapor pressure of a solution made by adding \(164 \mathrm{~g}\) of glycerin to \(338
Which of the following will have the lowest total vapor pressure at \(25^{\circ} \mathrm{C}\) ?a. pure waterb. a solution of glucose in water with \(\chi_{\text {glucose }}=0.01\)c. a solution of
Which of the choices in Exercise 40 has the highest vapor pressure?Data from Exercises 40Which of the following will have the lowest total vapor pressure at \(25^{\circ} \mathrm{C}\) ?pure waterA
A solution is made by mixing \(50.0 \mathrm{~g}\) of acetone \(\left(\mathrm{CH}_{3} \mathrm{COCH}_{3}ight)\) and \(50.0 \mathrm{~g}\) of methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}ight)\). What is
What is osmotic pressure? How is osmotic pressure calculated? Molarity units are used in the osmotic pressure equation. When does the molarity of a solution approximately equal the molality of the
Calculate the freezing-point depression and osmotic pressure in torr at \(25^{\circ} \mathrm{C}\) for an aqueous solution of \(1.0 \mathrm{~g} / \mathrm{L}\) of a protein (molar mass \(\left.=9.0
Before refrigeration became common, many foods were preserved by salting them heavily. Fruits were preserved by mixing them with a large amount of sugar (fruit preserves). How do salt and sugar act
Distinguish between a strong electrolyte and a weak electrolyte. How can colligative properties be used to distinguish between strong and weak electrolytes?
Consider an aqueous solution containing sodium chloride that has a density of \(1.01 \mathrm{~g} / \mathrm{mL}\). Assume that the solution behaves ideally. The freezing point of this solution at 1.00
What is the van't Hoff factor? Why is the observed freezing-point depression for electrolyte solutions sometimes less than the calculated value? Is the discrepancy greater for concentrated or dilute
Consider the following:What would happen to the level of liquid in the two arms if the semipermeable membrane separating the two liquids was permeable to the following?a. \(\mathrm{H}_{2}
Use the data in the following table for three different aqueous solutions of \(\mathrm{CaCl}_{2}\) to calculate the apparent value of the van't Hoff factor. Molality 0.0225 0.0910 0.278
The Tyndall effect is often used to distinguish between a colloidal suspension and a true solution. Explain.
The solubility of benzoic acid,is \(0.34 \mathrm{~g} / 100 \mathrm{~mL}\) in water at \(25^{\circ} \mathrm{C}\) and \(10.0 \mathrm{~g} / 100 \mathrm{~mL}\) in benzene \(\left(\mathrm{C}_{6}
A sample containing \(0.0500 \mathrm{~mol}\) of \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}ight)_{3}\) is dissolved in enough water to make \(1.00 \mathrm{~L}\) of solution. This solution contains
The compound \(\mathrm{VCl}_{4}\) undergoes dimerization in solution:\[2 \mathrm{VCl}_{4} ightleftharpoons \mathrm{V}_{2} \mathrm{Cl}_{8}\]When \(6.6834 \mathrm{~g}\) of \(\mathrm{VCl}_{4}\) is
Liquid A has vapor pressure \(x\), and liquid \(\mathrm{B}\) has vapor pressure \(y\). What is the mole fraction of the liquid mixture if the vapor above the solution is \(30 . \% \mathrm{~A}\) by
Using the following information, identify the strong electrolyte whose general formula is\[\mathrm{M}_{x}(\mathrm{~A})_{y} \cdot z \mathrm{H}_{2} \mathrm{O}\]Ignore the effect of interionic
What are the three types of hydrides? How do they differ?
Slaked lime \(\left[\mathrm{Ca}(\mathrm{OH})_{2}ight]\) is used to soften hard water by removing calcium ions from hard water through the reaction\[\mathrm{Ca}(\mathrm{OH})_{2}(a
What are three-centered bonds?
Use bond energies to estimate the maximum wavelength of light that will cause the reaction\[\mathrm{O}_{3} \xrightarrow{h v} \mathrm{O}_{2}+\mathrm{O}\]
Sulfur forms a wide variety of compounds in which it has \(+6,+4,+2,0\), and -2 oxidation states. Give examples of sulfur compounds having each of these oxidation states.
Give two reasons why \(\mathrm{F}_{2}\) is the most reactive of the halogens.
Calculate the \(\mathrm{pH}\) of a \(0.050 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}ight)_{3}\) solution. The \(K_{\text {a }}\) value for \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}ight)_{6}{
The inert pair effect is sometimes used to explain the tendency of heavier members of Group 3A to exhibit +1 and +3 oxidation states. What does the inert pair effect reference? (Consider the valence
Sodium tripolyphosphate \(\left(\mathrm{Na}_{5} \mathrm{P}_{3} \mathrm{O}_{10}ight)\) is used in many synthetic detergents. Its major effect is to soften the water by complexing \(\mathrm{Mg}^{2+}\)
A balloon is inflated to its full extent by heating the air inside it. In the final stages of this process the volume of the balloon changes from 4.00 × 106 L to 4.50 × 106 L by addition of 1.3 ×
Consider 2.00 mol of a monatomic ideal gas that is taken from state A (PA × 2.00 atm, VA = 10.0 L) to state B (PB = 1.00 atm, VB = 30.0 L) by two different pathways:Calculate q, w, ΔE, and ΔH for
When 1.00 L of 1.00 M Ba(NO3)2 at 25.0°C is mixed with 1.00 L of 1.00 M Na2SO4 at 25°C in a calorimeter, the white solid BaSO4 forms, and the temperature of the mixture increases to 28.1°C.
When 2.00 mol of SO2(g) reacts completely with 1.00 mol of O2(g) to form 2.00 mol of SO3(g) at 25°C and a constant pressure of 1.00 atm, 198 kJ of energy is released as heat. Calculate ΔH and ΔE
It has been suggested that hydrogen gas obtained from the decomposition of water might be a substitute for natural gas (principally methane). To compare the energies of combustion of these fuels, the
Diborane (B2H6) is a highly reactive boron hydride that was once considered as a possible rocket fuel for the U.S. space program. Calculate ΔH for the synthesis of diborane from its elements,
Using the standard enthalpies of formation listed in Table 9.4, calculate the standard enthalpy change for the overall reaction that occurs when ammonia is burned in air to form nitrogen dioxide and
Methanol (CH3OH) is sometimes used as a fuel in high-performance engines. Using the data in Table 9.4, compare the standard enthalpy of combustion per gram of methanol with that of gasoline. Gasoline
Assuming that the combustion of hydrogen gas provides three times as much energy per gram as gasoline, calculate the volume of liquid H2 (density = 0.0710 g/mL) required to furnish the energy
A friend tells you "Free energy \(G\) and pressure \(P\) are directly related by the equation \(G=G^{\circ}+R T \ln (P)\). Also, \(G\) is related to the equilibrium constant \(K\) in that when
You remember that \(\Delta G^{\circ}\) is related to \(R T \ln (K)\) but can't remember if it is \(R T \ln (K)\) or \(-R T \ln (K)\). Realizing what \(\Delta G^{\circ}\) and \(K\) mean, how can you
Which is larger: \(\Delta S\) at constant pressure or \(\Delta S\) at constant volume? Provide a conceptual rationale.
At 1 atm, liquid water is heated above \(100^{\circ} \mathrm{C}\). For this process which of the following choices (i-iv) is correct for \(\Delta S_{\text {surr }}\) ? \(\Delta S\) ? \(\Delta
Which of the following processes require energy as they occur?a. Salt dissolves in \(\mathrm{H}_{2} \mathrm{O}\).b. A clear solution becomes a uniform color after a few drops of dye are added.c. A
Choose the compound with the greatest positional probability in each case.a. \(1 \mathrm{~mol}_{\text {of }} \mathrm{H}_{2}\) at STP or \(1 \mathrm{~mol}_{\text {of }} \mathrm{H}_{2}\) at
Calculate \(\Delta S_{\text {surr }}\) for the following reactions at \(25^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm}\). a. C3H8(g) + 5O(g) 3CO2(g) + 4HO(l) b. 2NO2(g) 2NO(g) + O(g) AH = -2221 kJ AH
Given the following data:calculate \(\Delta G^{\circ}\) for the reaction\[6 \mathrm{C}(s)+3 \mathrm{H}_{2}(g) \longrightarrow \mathrm{C}_{6} \mathrm{H}_{6}(l)\] 2C6H6(l) +150(g) 12CO(g) + 6HO(l)
For each of the following pairs, choose the substance with the higher positional probability (per mole) at a given temperature.a. solid CO2 and gaseous CO2b. N2 gas at 1 atm and N2 gas at 1.0 ×
Predict the sign of the change in positional probability for each of the following processes.a. Solid sugar is added to water to form a solution.b. Iodine vapor condenses on a cold surface to form
Calculate the change in entropy that occurs when a sample containing 2.00 mol of water is heated from 50.°C to 150.°C at 1 atm pressure. The molar heat capacities for H2O(l) and H2O(g) are 75.3 J
In the metallurgy of antimony, the pure metal is recovered by different reactions, depending on the composition of the ore. For example, iron is used to reduce antimony in sulfide ores:Carbon is used
At what temperatures is the following process spontaneous at 1 atm?What is the normal boiling point of liquid Br2? Br(1) Br(g) where AH 31.0 kJ/mol and AS= 93.0 J K mol-
Predict the sign of ΔS° for each of the following reactions.a. the thermal decomposition of solid calcium carbonate:b. the oxidation of SO2 in air: CaCO3(s) CaO(s) + CO,(g)
Calculate ΔS° for the reduction of aluminum oxide by hydrogen gasusing the following standard entropy values. AlO3(s) + 3H(g) 2Al(s) + 3HO(g)
Consider the reactioncarried out at 25°C and 1 atm. Calculate ΔH° ΔS°, and ΔG° using the following data: 2SO2(g) + O2(g) 2SO3(g)
Using the following data (at 25°C),calculate ΔG° for the reaction Cdiamond "(s) + O(g) Cgraphite + O(g) - '(s) CO(g) CO(g) AG = -397 kJ AG = -394 kJ (10.5) (10.6)
Methanol is a high-octane fuel used in high-performance racing engines. Calculate ΔG° for the reactiongiven the following free energies of formation: 2CHOH(g) + 30(g) 2CO(g) + 4HO(g)
A chemical engineer wants to determine the feasibility of making ethanol (C2H5OH) by reacting water with ethylene (C2H4) according to the equationIs this reaction spontaneous under standard
One method for synthesizing methanol (CH3OH) involves reacting gaseouscarbon monoxide and hydrogen:Calculate ΔG at 25°C for this reaction, in which carbon monoxide gas at 5.0 atm and hydrogen gas
Consider the ammonia synthesis reactionwhere ΔG =–33.3 kJ per mole of N2 consumed at 25°C. For each of thefollowing mixtures of reactants and products at 25°C, predict the direction inwhich the
The overall reaction for the corrosion (rusting) of iron by oxygen isUsing the following data, calculate the equilibrium constant for this reaction at 25°C. 4Fe(s) + 30(g) 2FeO3(s)
The value of Kp is 3.7 × 10–6 at 900. K for the ammonia synthesis reaction. Assuming the value of ΔH° for this reaction is –92 kJ, calculate the value of Kp at 550. K.
Consider a sample containing 5.00 mol of a monatomic ideal gas at 25.0°C and an initial pressure of 10.0 atm. Suppose the external pressure is lowered to 1.00 atm in a reversible manner. Calculate
What is the difference between \(\mathscr{E}\) and \(\mathscr{E}^{\circ}\) ? When is \(\mathscr{E}\) equal to zero? When is \(\mathscr{E}^{\circ}\) equal to zero? (Consider "regular" galvanic cells
Consider the following galvanic cell:What happens to \(\mathscr{E}\) as the concentration of \(\mathrm{Zn}^{2+}\) is increased? as the concentration of \(\mathrm{Ag}^{+}\)is increased? What happens
The saturated calomel electrode, abbreviated SCE, is often used as a reference electrode in making electrochemical measurements. The SCE is composed of mercury in contact with a saturated solution of
Consider only the species (at standard conditions)\[\mathrm{Na}^{+}, \mathrm{Cl}^{-}, \mathrm{Ag}^{+}, \mathrm{Ag}, \mathrm{Zn}^{2+}, \mathrm{Zn} \text {, and } \mathrm{Pb}\]in answering the
Use the table of standard reduction potentials (Table 11.1) to pick a reagent that is capable of each of the following oxidations (under standard conditions in acidic solution).a. oxidizes
Use the table of standard reduction potentials (Table 11.1) to pick a reagent that is capable of each of the following reductions (under standard conditions in acidic solution).a. reduces
The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing \(\mathrm{Mn}^{2+}\) ions. These ions are then oxidized to
For the following half-reaction, \(\mathscr{E}^{\circ}=-2.07 \mathrm{~V}\) :\[\mathrm{AlF}_{6}{ }^{3-}+3 \mathrm{e}^{-} \longrightarrow \mathrm{Al}+6 \mathrm{~F}^{-}\]Using data from Table 11.1,
The solubility product for \(\mathrm{CuI}(s)\) is \(1.1 \times 10^{-12}\). Calculate the value of \(\mathscr{E}^{\circ}\) for the half-reaction\[\mathrm{CuI}+\mathrm{e}^{-} \longrightarrow
Calculate the \(\mathrm{pH}\) of the cathode compartment for the following reaction given \(\mathscr{E}_{\text {cell }}=3.01 \mathrm{~V}\) when \(\left[\mathrm{Cr}^{3+}ight]=\) \(0.15
The overall reaction in the lead storage battery isa. Calculate \(\mathscr{E}\) at \(25^{\circ} \mathrm{C}\) for this battery when \(\left[\mathrm{H}_{2} \mathrm{SO}_{4}ight]=4.5 \mathrm{M}\); that
Concentration cells are commonly used to calculate the value of equilibrium constants for various reactions. For example, the silver concentration cell illustrated in Fig. 11.11 can be used to
In the electrolysis of a sodium chloride solution, what volume of \(\mathrm{Cl}_{2}(\mathrm{~g})\) is produced in the same time it takes to produce \(6.00 \mathrm{~L}\) of
The black silver sulfide discoloration of silverware can easily be removed by heating the silver article in a sodium carbonate solution in an aluminum pan. The reaction is\[3 \mathrm{Ag}_{2}
Consider a cell based on the following half-reactions:a. Draw this cell under standard conditions, labeling the anode, the cathode, the direction of electron flow, and the concentrations, as
A zinc-copper battery is constructed as follows:\[\mathrm{Zn}\left|\mathrm{Zn}^{2+}(0.10 M)ight|\left|\mathrm{Cu}^{2+}(2.50 M)ight| \mathrm{Cu}\]The mass of each electrode is 200 . \(\mathrm{g}\).a.
The measurement of \(\mathrm{F}^{-}\)ion concentration by ionselective electrodes at \(25.00^{\circ} \mathrm{C}\) obeys the equation\[\mathscr{E}_{\text {meas }}=\mathscr{E}_{\text {ref }}-0.05916
You make a galvanic cell with a piece of nickel, \(1.0 \mathrm{M}\) \(\mathrm{Ni}^{2+}(a q)\), a piece of silver, and \(1.0 \mathrm{M} \mathrm{Ag}^{+}(a q)\). Calculate the concentrations of
Consider the following galvanic cell:A 15.0-mol sample of \(\mathrm{NH}_{3}\) is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia
Describe completely the galvanic cell based on the following half-reactions under standard conditions: Ag + e Fe+ + e Ag Fe2+ 8 = 0.80 V 8 = 0.77 V (1) (2)
Using the data in Table 11.1, calculate ΔG° for the reactionIs this reaction spontaneous? Cu+ (aq) + Fe(s) Cu(s) + Fe+ (aq)
Using the data from Table 11.1, predict whether 1 M HNO3 will dissolve gold metal to form a 1 M Au3+ solution. TABLE II.I Standard Reduction Potentials at 25C (298 K) for Many Common Half-reactions
For the cell reactionpredict whether ξcell will be larger or smaller than ξ°cell for the following cases. 2Al(s) + 3Mn+ (aq) 2A1+ (aq) + 3Mn(s) Ecell = 0.48 V
Describe the cell based on the following half-reactions:where VO+ + 2H+ + e Zn+ +2e= VO+ + HO 2+ Zn 8 = 1.00 V 8 = -0.76 V (1) (2)

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