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General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions

Explain the important distinctions between each pair of terms: (a) Frequency and wavelength; (b) Ultraviolet and infrared light; (c) Continuous and discontinuous spectra; (d) Traveling and standing waves;(e) Quantum number and orbital; (f) Spdƒ notation and orbital diagram; (g) S block and p
Describe two ways in which the orbitals of multielectron atoms resemble hydrogen orbitals and two ways in which they differ from hydrogen orbitals.
Explain the phrase effective nuclear charge. How is this related to the shielding effect?
With the help of sketches, explain the difference between a px, py, and pz orbital.
With the help of sketches, explain the difference between a 2pz and 3pz orbital.
If traveling at equal speeds, which of the following matter waves has the longest wavelength? Explain.(a) Electron; (b) Proton; (c) Neutron; (d) α particle (He2+).
For electromagnetic radiation transmitted through a vacuum, state whether each of the following properties is directly proportional to, inversely proportional to, or independent of the frequency: (a) Velocity;(b) Wavelength; (c) Energy per mole. Explain.
Construct a concept map representing the ideas of quantum mechanics.
Construct a concept map representing the atomic orbitals of hydrogen and their properties.
Construct a concept map for the configurations of multielectron atoms.
(A) The light from red LEDs (light-emitting diodes) is commonly seen in many electronic devices. A typical LED produces 690 nm light. What is the frequency of this light?(B) An FM radio station broadcasts on a frequency of 91.5 megahertz (MHz). What is the wavelength of these radio waves in meters?
Most of the light from a sodium vapor lamp has a wavelength of 589 nm. What is the frequency of this radiation?
For radiation of wavelength 242.4 nm, the longest wavelength that will bring about the photodissociation of O2, what is the energy of (a) One photon, and (b) A mole of photons of this light?
Is there an energy level for the hydrogen atom having E = -1.00 x 10-20 J?
Determine the wavelength of the line in the Balmer series of hydrogen corresponding to the transition from n = 5 to n = 2.
Determine the kinetic energy of the electron ionized from a Li2+ ion in its ground state, using a photon of frequency 5.000 x 1016 s-1.
What is the wavelength associated with electrons traveling at one-tenth the speed of light?
A 12 eV electron can be shown to have a speed of 2.05 x 106 m/s. Assuming that the precision (uncertainty) of this value is 1.5%, with what maximum precision can we simultaneously measure the position of the electron?
What is the energy difference between the ground state and the first excited state of an electron contained in a one-dimensional box 1.00 x 102 pm long? Calculate the wavelength of the photon that could excite the electron from the ground state to the first excited state.
What is the fraction, as a percentage, of the total probability of finding, between points at 0 pm and 30 pm, an electron in the n = 5 level of a one-dimensional box 150 pm long?
Can an orbital have the quantum numbers n = 2, ℓ = 2, and mℓ = 2?
From the following sets of quantum numbers (n, ℓ, mℓ, ms), identify the set that is correct, and state the orbital designation for those quantum numbers: (2,1,0,0) (2,0,1,1) (2,2,0,1) (2,-1,0,1) (2,1,0,-1)
Write an orbital designation corresponding to the quantum numbers n = 4, ℓ = 2, mℓ = 0.
(a) Identify the element having the electron configuration(b) Write the electron configuration of arsenic. 1s²2s²2p63s²3p5
Write (a) The electron configuration of mercury, and (b) An orbital diagram for the electron configuration of tin.
Indicate the number of (a) Valence electrons in an atom of bromine; (b) 5p electrons in an atom of tellurium;(c) Unpaired electrons in an atom of indium; (d) 3d and 4d electrons in a silver atom.
Do you think the following observation is any way possible? A gas absorbs heat from its surroundings while being compressed. Explain your answer.
Balance these equations for redox reactions occurring in basic solution.(a) CrO42- + S2O42- → Cr(OH)3(s) + SO32-(b) [Fe(CN)6]3- + N2H4 → [Fe(CN)6]4- + N2(g)(c) Fe(OH)2(s) + O2(g) → Fe(OH)3(s)(d) CH3CH2OH + MnO4- → CH3COO- + MnO2(s).
A 25.00 mL sample of 0.132 M HNO3 is mixed with 10.00 mL of 0.318 M KOH. Is the resulting solution acidic, basic, or exactly neutralized?
A 7.55 g sample of Na2CO3(s) is added to 125 mL of a vinegar that is 0.762 M CH3COOH. Will the resulting solution still be acidic? Explain.
Without doing detailed calculations, determine which of the following samples occupies the largest volume:(a) 25.5 mol of sodium metal (d = 0.971 g/cm3)(b) 0.725 L of liquid bromine (d = 3.12 g/mL)(c) 1.25 x 1025 atoms of chromium metal (d = 9.4 g/cm3)(d) 2.15 kg of plumber’s solder (d = 9.4
Express P = 1 atm in pounds per square inch (psi).
Calculate the quantity of heat, in kilojoules, (a) Required to raise the temperature of 9.25 L of water from 22.0 to 29.4 °C; (b) Associated with a 33.5 °C decrease in temperature in a 5.85 kg aluminum bar (specific heat capacity of = 0.903 J g-1 °C-1).
Refer to Example 7-2. The experiment is repeated with several different metals substituting for the lead. The masses of metal and water and the initial temperatures of the metal and water are the same as in Figure 7-3. The final temperatures are (a) Zn, 38.9 °C;(b) Pt, 28.8 °C; (c) Al, 52.7
Calculate the final temperature that results when (a) A 12.6 g sample of water at 22.9 °C absorbs 875 J of heat;(b) A 1.59 kg sample of platinum at 78.2 °C gives off 1.05 kcal of heat (cp = 0.032 cal g-1 °C-1).
A 75.0 g piece of Ag metal is heated to 80.0 °C and dropped into 50.0 g of water at 23.2 °C. The final temperature of the Ag–H2O mixture is 27.6 °C. What is the specific heat capacity of silver?
A 465 g chunk of iron is removed from an oven and plunged into 375 g water in an insulated container. The temperature of the water increases from 26 to 87 °C. If the specific heat capacity of iron is 0.449 J g-1 °C-1, what must have been the original temperature of the iron?
A piece of stainless steel (cp = 0.50 J g-1 °C-1) is transferred from an oven at 201 °C into 150 mL of water at 23.2 °C. The water temperature rises to What is the mass of the steel? How precise is this method of mass determination? Explain.
A 1.00 kg sample of magnesium at 40.0 °C is added to 1.00 L of water maintained at 20.0 °C in an insulated container. What will be the final temperature of the Mg–H2O mixture (specific heat capacity of Mg = 1.024 J g-1 °C-1)?
In the form of heat, 6.052 J of energy is transferred to a 1.0 L sample of air (d = 1.204 mg/cm3) at 20.0 °C. The final temperature of the air is 25.0 °C. What is the heat capacity of air in J/K?
A 74.8 g sample of copper at 143.2 °C is added to an insulated vessel containing 165 mL of glycerol, C3H8O3(l) (d = 1.26 g/mL), at 24.8 °C. The final temperature is 31.1 °C. The specific heat capacity of copper is 0.385 J g-1 °C-1. What is the heat capacity of glycerol in J mol-1 °C-1?
A 69.0 g sample of gold at 127.1 °C is added to an insulated vessel containing 543.0 mL of water at 25.0 °C. The final temperature is 25.4 °C. What is the specific heat capacity of gold in J g-1 °C-1? The specific heat capacity of water is 4.18 J g-1 °C-1, and its density (at 25.0°C) is 0.997
Brass has a density of 8.40 g/cm3 and a specific heat capacity of 0.385 J g-1 °C-1. A 15.2 cm3 piece of brass at an initial temperature of 163 °C is dropped into an insulated container with 150.0 g water initially at 22.4 °C. What will be the final temperature of the brass–water mixture?
How much heat, in kilojoules, is associated with the production of 283 kg of slaked lime, Ca(OH)2? CaO(s) + H₂O(1) - Ca(OH)2(s) A,H° -65.2 kJ mol-1
What is the final temperature (in °C) of 1.24 g of water with an initial temperature of 20.0 °C after 6.052 J of heat is added to it?
How much heat, in kilojoules, is evolved in the complete combustion of (a) 1.325 g C4H10(g) at 25 °C and 1 atm; (b) 28.4 L C4H10(g) at STP;(c) 12.6 L C4H10(g) at 23.6 °C and 738 mmHg?Assume that the enthalpy of reaction does not change significantly with temperature or pressure. The complete
The standard enthalpy of reaction for the combustion of octane is ΔrH° = -5.48 x 103 kJ/mol C8H18(l). How much heat, in kilojoules, is liberated per gallon of octane burned? (Density of octane = 0.703 g/mL; 1 gal = 3.785 L.)
The combustion of methane gas, the principal constituent of natural gas, is represented by the equation (a) What mass of methane, in kilograms, must be burned to liberate 2.80 x 107 kJ of heat?(b) What quantity of heat, in kilojoules, is liberated in the complete combustion of 1.65 x 104 L of
Upon complete combustion, the indicated substances evolve the given quantities of heat. Write a balanced equation for the combustion of 1.00 mol of each substance, including the enthalpy of reaction, ΔrH, for the reaction.(a) 0.584 g of propane, C3H8(g), yields 29.4 kJ (b) 0.136 g of camphor,
The combustion of hydrogen–oxygen mixtures is used to produce very high temperatures (approximately 2500 °C) needed for certain types of welding operations. Consider the reaction to beWhat is the quantity of heat evolved, in kilojoules, when a 180 g mixture containing equal parts of H2 and O2 by
Refer to the Integrative Example. What volume of the synthesis gas, measured at STP and burned in an open flame (constant-pressure process), is required to heat 40.0 gal of water from 15.2 to 65.0 °C? (1 gal = 3.785 L.)Integrative ExampleWhen charcoal is burned in a limited supply of oxygen in the
Thermite mixtures are used for certain types of welding, and the thermite reaction is highly exothermic.1.00 mol of granular Fe2O3 and 2.00 mol of granular Al are mixed at room temperature (25 °C), and a reaction is initiated. The liberated heat is retained within the products, whose combined
A 0.205 g pellet of potassium hydroxide, KOH, is added to 55.9 g water in a Styrofoam coffee cup. The water temperature rises from 23.5 to 24.4 °C. [Assume that the specific heat capacity of dilute KOH(aq) is the same as that of water.](a) What is the approximate heat of solution of KOH, expressed
The heat of solution of KI(s) in water is +20.3 kJ/mol KI. If a quantity of KI is added to sufficient water at 24.3 °C in a Styrofoam cup to produce 175.0 mL of 2.50 M KI, what will be the final temperature? (Assume a density of 1.30 g/mL and a specific heat capacity of 2.7 J g-1 °C-1 for 2.50 M
You are planning a lecture demonstration to illustrate an endothermic process. You want to lower the temperature of 1400 mL water in an insulated container from 25 to 10 °C. Approximately what mass of NH4Cl(s) should you dissolve in the water to achieve this result? The heat of solution of NH4Cl
Care must be taken in preparing solutions of solutes that liberate heat on dissolving. The heat of solution of NaOH is -44.5 kJ/mol NaOH. To what maximum temperature may a sample of water, originally at 24 °C, be raised in the preparation of 500 mL of 4.0 M NaOH? Assume the solution has a density
Refer to Example 7-4. The product of the neutralization is 0.500 M NaCl. For this solution, assume a density of 1.02 g/mL and a specific heat capacity of 4.02 J g-1 °C-1. Also, assume a heat capacity for the Styrofoam cup of 10 J/°C, and recalculate the heat of neutralization.Example 7-4In the
Acetylene (C2H2) torches are used in welding. How much heat (in kJ) evolves when 5.0 L of C2H2 (d = 1.0967 kg/m3) is mixed with a stoichiometric amount of oxygen gas? The combustion reaction is 5 C₂H₂(g) + +2/202(8) 2 CO2(g) + H₂O(1) A,H° -1299.5 kJ mol-1
The heat of neutralization of HCl(aq) by NaOH(aq) is -55.84 kJ/mol H2O produced. If 50.00 mL of 1.05 M NaOH is added to 25.00 mL of 1.86 M HCl, with both solutions originally at 24.72 °C, what will be the final solution temperature? (Assume that no heat is lost to the surrounding air and that the
Propane (C3H8) gas (d = 1.83 kg/m3) is used in most gas grills. What volume (in liters) of propane is needed to generate 273.8 kJ of heat? C3H8(g) + 5O2(g) 3 CO₂(g) + 4H₂O(1) A,H° -2219.9 kJ mol-1 =
What mass of ice can be melted with the same quantity 3.50 mol H2O(l) of heat as required to raise the temperature of by 50.0 °C? [ΔfusH° = 6.01 kJ/mol H2O(s)].
What will be the final temperature of the water in an insulated container as the result of passing 5.00 g of steam, H2O(g), at 100.0 °C into 100.0 g of water at 25.0 °C? (ΔvapH° = 40.6 kJ/mol H2O).
A 125 g stainless steel ball bearing (cp = 0.50 J g -1 °C-1) at 525 °C is dropped into 75.0 mL of water at in an open Styrofoam cup. As a result, the water is brought to a boil when the temperature reaches 100.0 °C. What mass of water vaporizes while the boiling continues? (ΔvapH° = 40.6
If the ball bearing described in Exercise 31 is dropped onto a large block of ice at 0 °C, what mass of liquid water will form? (ΔfusH° = 6.01 kJ/mol H2O). Exercise 31 A 125 g stainless steel ball bearing (cp = 0.50 J g -1 °C-1) at 525 °C is dropped into 75.0 mL of water at in an open
The enthalpy of sublimation (Solid → gas) for dry ice (i.e., CO2) is ΔsubH° = 571 kJ/kg at -78.5 °C. If 125.0 J of heat is transferred to a block of dry ice that is -78.5 °C, what volume of CO2 gas (d = 1.98 g/L) will be generated?
The enthalpy of vaporization for N2(l) is 5.56 kJ/mol. How much heat (in J) is required to produce 1.0 L of N2(g) at 77.36 K and 1.0 atm?
A sample gives off 5228 cal when burned in a bomb calorimeter. The temperature of the calorimeter assembly increases by 4.39 °C. Calculate the heat capacity of the calorimeter, in kilojoules per degree Celsius.
The following substances undergo complete combustion in a bomb calorimeter. The calorimeter assembly has a heat capacity of 5.136 kJ/°C. In each case, what is the final temperature if the initial water temperature is 22.43 °C?(a) 0.3268 g caffeine, C8H10O2N4 (heat of combustion = -1014.2 kcal/mol
A coffee-cup calorimeter contains 100.0 mL of 0.300 M HCl at 20.3 °C. When 1.82 g Zn(s) is added, the temperature rises to 30.5 °C. What is the heat of reaction per mol Zn? Make the same assumptions as in Example 7-4, and also assume that there is no heat lost with the H2(g) that escapes.Example
A bomb calorimetry experiment is performed with xylose, C5H10O5(s), as the combustible substance.The data obtained areMass of xylose burned: 1.183 g Heat capacity of calorimeter: 4.728 kJ/°C Initial calorimeter temperature: 23.29 °C Final calorimeter temperature: 27.19 °C(a) What is the heat
A 0.75 g sample of KCl is added to 35.0 g H2O in a Styrofoam cup and stirred until it dissolves. The temperature of the solution drops from 24.8 to 23.6 °C.(a) Is the process endothermic or exothermic?(b) What is the heat of solution of KCl expressed in kilojoules per mole of KCl?
The heat of solution of potassium acetate in water is -15.3 kJ/mol KCH3COO. What will be the final temperature when 0.241 mol KCH3COO is dissolved in 815 mL water that is initially at 25.1 °C?
A 1.620 g sample of naphthalene, C10H8(s), is completely burned in a bomb calorimeter assembly and a temperature increase of 8.44 °C is noted. If the heat of combustion of naphthalene is -5156 kJ/mol C10H8, what is the heat capacity of the bomb calorimeter?
Salicylic acid, C7H6O3, has been suggested as a calorimetric standard. Its heat of combustion is -3.023 x 103 kJ/mol C7H6O3. From the following data determine the heat capacity of a bomb calorimeter assembly (that is, the bomb, water, stirrer, thermometer, wires, and so forth).Mass of salicylic
Refer to Example 7-3. Based on the heat of combustion of sucrose established in the example, what should be the temperature change (ΔT) produced by the combustion of 1.227 g C12H22O11 in a bomb calorimeter assembly with a heat capacity of 3.87 kJ/°C?Example 7-3The combustion of 1.010 g sucrose,
A 1.397 g sample of thymol, C10H14O(s) (a preservative and a mold and mildew preventative), is burned in a bomb calorimeter assembly. The temperature increase is 11.23 °C, and the heat capacity of the bomb calorimeter is 4.68 kJ/°C. What is the heat of combustion of thymol, expressed in
A 5.0 g sample of NaCl is added to a Styrofoam cup of water, and the change in water temperature is 5.0 °C. The heat of solution of NaCl is 3.76 kJ/mol. What is the mass (in g) of water in the Styrofoam cup?
We can determine the purity of solid materials by using calorimetry. A gold ring (for pure gold, specific heat capacity = 0.1291 J g-1 K-1) with mass of 10.5 g is heated to 78.3 °C and immersed in 50.0 g of 23.7 °C water in a constant-pressure calorimeter. The final temperature of the water is
Calculate the quantity of work associated with a 3.5 L expansion of a gas (ΔV) against a pressure of 748 mmHg in the units (a) Atm L; (b) Joules (J);(c) Calories (cal).
Calculate the quantity of work, in joules, associated with the compression of a gas from 5.62 L to 3.37 L by a constant pressure of 1.23 atm.
A 1.00 g sample of Ne(g) at 1 atm pressure and 27 °C is allowed to expand into an evacuated vessel of 2.50 L volume. Does the gas do work? Explain.
Compressed air in aerosol cans is used to free electronic equipment of dust. Does the air do any work as it escapes from the can?
In each of the following processes, is any work done when the reaction is carried out at constant pressure in a vessel open to the atmosphere? If so, is work done by the reacting system or on it? (a) Neutralization of Ba(OH)2(aq) by HCl(aq); (b) Conversion of gaseous nitrogen dioxide to gaseous
In each of the following processes, is any work done when the reaction is carried out at constant pressure in a vessel open to the atmosphere? If so, is work done by the reacting system or on it? (a) Reaction of nitrogen monoxide and oxygen gases to form gaseous nitrogen dioxide; (b)
If 325 J of work is done by a system at a pressure of 1.0 atm and 298 K, what is the change in the volume of the system?
A movable piston in a cylinder holding 5.0 L N2(g) is used to lift a 2.41 kg object to a height of 2.6 meters. How much work (in J) was done by the gas?
What is the change in internal energy of a system if the system (a) Absorbs 58 J of heat and does 58 J of work; (b) Absorbs 125 J of heat and does 687 J of work;(c) Evolves 280 cal of heat and has 1.25 kJ of work done on it?
What is the change in internal energy of a system if the surroundings (a) Transfer 235 J of heat and 128 J of work to the system; (b) Absorb 145 J of heat from the system while doing 98 J of work on the system; (c) Exchange no heat, but receive 1.07 kJ of work from the system?
The internal energy of a fixed quantity of an ideal gas depends only on its temperature. Asample of an ideal gas is allowed to expand at a constant temperature (isothermal expansion). (a) Does the gas do work?(b) Does the gas exchange heat with its surroundings?(c) What happens to the temperature
In an adiabatic process, a system is thermally insulated—there is no exchange of heat between system and surroundings. For the adiabatic expansion of an ideal gas(a) Does the gas do work? (b) Does the internal energy of the gas increase, decrease, or remain constant? (c) What happens to the
For the reaction C2H4(g) + Cl2(g) → C2H4Cl2(l), determine ΔrH°, given that 4 HCl(g) + O₂(g) →→→→ 2Cl₂(g) + 2 H₂O(1) A,H° -202.4 kJ mol-¹ 2HCl(8) + C₂H4(8) + O2(8) - = C₂H4Cl₂(1)+ H₂O(1) AH° -318.7 kJ mol-1 =
Do you think the following observation is in any way possible? An ideal gas is expanded isothermally and is observed to do twice as much work as the heat absorbed from its surroundings. Explain your answer.
There are other forms of work besides P–V work. For example, electrical work is defined as the potential x change in charge, w = ϕ Δq. If a charge in a system is changed from 10 C to 5 C in a potential of 100 V and 45 J of heat is liberated, what is the change in the internal energy? (Note: 1 V
Another form of work is extension, defined as the tension x change in length, w = ϕ Δl. A piece of DNA has an approximate tension of ƒ = 10 pN. What is the change in the internal energy of the adiabatic stretching of DNA by 10 pm?
Only one of the following quantities is equal to the heat of a chemical reaction, regardless of how the reaction is carried out. Which one and why? (a) qV; (b) qP;(c) ΔU - w;(d) ΔU; (e) ΔrH.
Determine whether ΔH is equal to, greater than, or less than ΔU for the following processes. Keep in mind that “greater than” means more positive or less negative, and “less than” means less positive or more negative. Assume that the only significant change in volume during a constant
The heat of combustion of propan-2-ol at 298.15 K, determined in a bomb calorimeter, is -33.41 kJ/g. For the combustion of one mole of propan-2-ol, determine (a) ΔU, and (b) ΔrH.
The standard enthalpy of formation of NH3(g) is -46.11 kJ/mol. What is ΔrH° for the following reaction? 2 NH3(g) -N2(g) + H₂(g) N2(8) A,Hº
Write an equation to represent the combustion of thymol referred to in Exercise 44. Include in this equation the values for ΔU and ΔH.Exercise 44A 1.397 g sample of thymol, C10H14O(s) (a preservative and a mold and mildew preventative), is burned in a bomb calorimeter assembly. The temperature
Use Hess’s law to determine ΔrH° for the reaction 1 CO(g) + O2(g) →→→→ CO₂(g), given that C(graphite) + +10₂(8) C(graphite) + O₂(g) CO(g) A,H° -110.54 kJ mol-1 CO₂(g) A,H° = -393.51 kJ mol-1 =

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