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chemistry a molecular approach

Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions

Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 5.00 * 102 kJ of heat. C(s) + O₂(8) CO₂(8) AHxn=-393.5 kJ
A silver block, initially at 58.5 °C, is submerged into 100.0 g of water at 24.8 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.2 °C. What is the mass of the silver block?
A 32.5-g iron rod, initially at 22.7 °C, is submerged into an unknown mass of water at 63.2 °C, in an insulated container.The final temperature of the mixture upon reaching thermal equilibrium is 59.5 °C. What is the mass of the water?
A 2.74-g sample of a substance suspected of being pure gold is warmed to 72.1 °C and submerged into 15.2 g of water initially at 24.7 °C. The final temperature of the mixture is 26.3 °C. What is the heat capacity of the unknown substance? Could the substance be pure gold?
Exactly 1.5 g of a fuel burns under conditions of constant pressure and then again under conditions of constant volume. In measurement A the reaction produces 25.9 kJ of heat, and in measurement B the reaction produces 23.3 kJ of heat. Which measurement (A or B) corresponds to conditions of
In order to obtain the largest possible amount of heat from a chemical reaction in which there is a large increase in the number of moles of gas, should you carry out the reaction under conditions of constant volume or constant pressure? Explain.
When 0.514 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8 °C to 29.4 °C.Find ΔErxn for the combustion of biphenyl in kJ/mol biphenyl.The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/°C.
Zinc metal reacts with hydrochloric acid according to the balanced equation:When 0.103 g of Zn(s) is combined with enough HCl to make 50.0 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.5 °C to 23.7 °C. Find ΔHrxn for this
Mothballs are composed primarily of the hydrocarbon naphthalene (C10H8). When 1.025 g of naphthalene burns in a bomb calorimeter, the temperature rises from 24.25 °C to 32.33 °C.Find ΔErxn for the combustion of naphthalene. The heat capacity of the bomb calorimeter, determined in a separate
Instant cold packs used to ice athletic injuries on the field contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the endothermic reaction:In order to measure the enthalpy change for this reaction, 1.25 g of
For each generic reaction, determine the value of ΔH2 in terms of ΔH1. a. A + B -2C 2C — A + B b. A + 12B — C 2 A + B - 2C c. A → B + 2 C 1/2B + C - → • 1/2A ΔΗ, ΔΗ, = ? ΔΗ ΔΗ, = ? ΔΗ ΔΗ, = ?
Consider the generic reaction:Determine the value of ΔH for each related reaction. A + 2B C + 3D → AH = 155 kJ
Calculate ΔHrxn for the reaction:Use the following reactions and given ΔH’s: 5 C(s) + 6 H₂(8) C5H12(1)
Calculate ΔHrxn for the reaction:Use the following reactions and given ΔH’s: Fe₂O3(s) + 3 CO(g) 2 Fe(s) + 3 CO2(8)
Calculate ΔHrxn for the reaction:Use the following reactions and given ΔH’s: CaO(s) + CO2(g) CaCO3(s)
Calculate ΔHrxn for the reaction:Use the following reactions and given ΔH’s: CH4(g) + 4 Cl2(g) CC14(g) + 4 HCl(g)
Write an equation for the formation of each compound from its elements in their standard states, and find ΔH°f for each in Appendix IIB.a. NH3(g) b. CO2(g) c. Fe2O3(s) d. CH4(g)
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. a. C₂H4(g) + H₂(g) C₂H6(8) b. CO(g) + H₂O(g) →→→ H₂(g) + CO₂(g) c. 3 NO₂(g) + H₂O(1) d. Cr₂O3(s) + 3 CO(g) 2 HNO3(aq) + NO(g) 2 Cr(s) + 3 CO₂(8)
Write an equation for the formation of each compound from its elements in their standard states, and find ΔH °rxn for each.a. NO2(g) b. MgCO3(s) c. C2H4(g) d. CH3OH(l)
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. 2 H₂O(l) +2 SO₂(8) SO3(8) a. 2 H₂S(g) + 3 O₂(g) b. SO2(g) + ¹/2O2(8) c. C(s) + H₂O(g) →→→ CO(g) + H₂(g) d. N₂O4(g) + 4 H₂(g) N₂(g) + 4H₂O(g)
Top fuel dragsters and funny cars burn nitromethane as fuel according to the balanced combustion equation:Calculate the standard enthalpy of formation (ΔH°f) for nitromethane. 2 CH3NO₂(1) + ³/2O₂(g) 2 CO₂(g) + 3 H₂O(1) + N₂(g) AHxn = -1418 kJ
During photosynthesis, plants use energy from sunlight to form glucose (C6H12O6) and oxygen from carbon dioxide and water. Write a balanced equation for photosynthesis and calculate ΔH°rxn.
Ethanol (C2H5OH) can be made from the fermentation of crops and has been used as a fuel additive to gasoline. Write a balanced equation for the combustion of ethanol and calculate ΔH°rxn.
The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the balanced equation:Calculate the standard enthalpy of formation (ΔH°f) for nitroglycerin. 4 C3H5N3O9 (1) 12 CO₂(g) + 10 H₂O(g) + 6 N₂(g) + O₂(g) AHixn -5678 kJ =
Determine the mass of CO2 produced by burning enough of each fuel to produce 1.00 * 102 kJ of heat. Which fuel contributes least to global warming per kJ of heat produced? a. CH.(g) + 2 O2(g) b. C3Hg(g) + 5 O2(g) c. CgHg(I) + 25/2 O2(g) CO2(g) + 2H2O(g) ΔΗxn - 3 CO2(g) + 4H,O(g) ΔHxn = -2043
Methanol (CH3OH) has been suggested as a fuel to replace gasoline.Write a balanced equation for the combustion of methanol, find ΔH°rxn, and determine the mass of carbon dioxide emitted per kJ of heat produced. Use the information from the previous exercise to calculate the same quantity for
The citizens of the world burn the fossil fuel equivalent of 7 * 1012 kg of petroleum per year. Assume that all of this petroleum is in the form of octane (C8H18) and calculate how much CO2 (in kg) the world produces from fossil fuel combustion per year. (Begin by writing a balanced equation for
In a sunny location, sunlight has a power density of about 1 kW/m2. Photovoltaic solar cells can convert this power into electricity with 15% efficiency. If a typical home uses 385 kWh of electricity per month, how many square meters of solar cells are required to meet its energy requirements?
The kinetic energy of a rolling billiard ball is given by KE = 1/2 mv2. Suppose a 0.17-kg billiard ball is rolling down a pool table with an initial speed of 4.5 m/s. As it travels, it loses some of its energy as heat. The ball slows down to 3.8 m/s and then collides head-on with a second billiard
Evaporating sweat cools the body because evaporation is an endothermic process:Estimate the mass of water that must evaporate from the skin to cool the body by 0.50 °C. Assume a body mass of 95 kg and assume that the specific heat capacity of the body is 4.0 J/g · °C. H₂O(1)→ H₂O(g) AHxn =
A 100-W lightbulb is placed in a cylinder equipped with a moveable piston. The lightbulb is turned on for 0.015 hour, and the assembly expands from an initial volume of 0.85 L to a final volume of 5.88 L against an external pressure of 1.0 atm. Use the wattage of the lightbulb and the time it is on
LP gas burns according to the exothermic reaction:What mass of LP gas is necessary to heat 1.5 L of water from room temperature (25.0 °C) to boiling (100.0 °C)? Assume that during heating, 15% of the heat emitted by the LP gas combustion goes to heat the water. The rest is lost as heat to the
Derive a relationship between ΔH and ΔE for a process in which the temperature of a fixed amount of an ideal gas changes.
Under certain nonstandard conditions, oxidation by O2(g) of 1 mol of SO2(g) to SO3(g) absorbs 89.5 kJ. The enthalpy of formation of SO3(g) is -204.2 kJ under these conditions. Find the enthalpy of formation of SO2(g).
One tablespoon of peanut butter has a mass of 16 g. It is combusted in a calorimeter whose heat capacity is 120.0 kJ/°C. The temperature of the calorimeter rises from 22.2 °C to 25.4 °C.Find the food caloric content of peanut butter.
A mixture of 2.0 mol of H2( g) and 1.0 mol of O2( g) is placed in a sealed evacuated container made of a perfect insulating material at 25 °C. The mixture is ignited with a spark and reacts to form liquid water. Determine the temperature of the water.
A 20.0-L volume of an ideal gas in a cylinder with a piston is at a pressure of 3.0 atm. Enough weight is suddenly removed from the piston to lower the external pressure to 1.5 atm. The gas then expands at constant temperature until its pressure is 1.5 atm. Find ΔE, ΔH, q, and w for this change
When 10.00 g of phosphorus is burned in O2(g) to form P4O10(s), enough heat is generated to raise the temperature of 2950 g of water from 18.0 °C to 38.0 °C. Calculate the enthalpy of formation of P4O10(s) under these conditions.
The ΔH for the oxidation of sulfur in the gas phase to SO3 is -204 kJ/mol and for the oxidation of SO2 to SO3 is 89.5 kJ/mol.Find the enthalpy of formation of SO2 under these conditions.
The ΔH°f of TiI3(s) is -328 kJ/mol and the ΔH° for the reaction 2 Ti(s) + 3 I2( g) → 2 TiI3(s) is -839 kJ. Calculate the ΔH of sublimation of I2(s), which is a solid at 25 °C.
A gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and the rest propane (C3H8) by volume. When the fuel mixture contained in a 1.55 L tank, stored at 755 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion
A gaseous fuel mixture stored at 745 mmHg and 298 K contains only methane (CH4) and propane (C3H8). When 11.7 L of this fuel mixture is burned, it produces 769 kJ of heat. What is the mole fraction of methane in the mixture? (Assume that the water produced by the combustion is in the gaseous state.)
A copper cube with an edge measuring 1.55 cm and an aluminum cube with an edge measuring 1.62 cm are both heated to 55.0 °C and submerged in 100.0 mL of water at 22.2 °C. What is the final temperature of the water when equilibrium is reached?
A pure gold ring and a pure silver ring have a total mass of 14.9 g.The two rings are heated to 62.0 °C and dropped into 15.0 mL of water at 23.5 °C. When equilibrium is reached, the temperature of the water is 25.0 °C. What is the mass of each ring?
A typical frostless refrigerator uses 655 kWh of energy per year in the form of electricity. Suppose that all of this electricity is generated at a power plant that burns coal containing 3.2% sulfur by mass and that all of the sulfur is emitted as SO2 when the coal is burned. If all of the SO2 goes
A large sport utility vehicle has a mass of 2.5 * 103 kg. Calculate the mass of CO2 emitted into the atmosphere upon accelerating the SUV from 0.0 mph to 65.0 mph. Assume that the required energy comes from the combustion of octane with 30% efficiency.
Combustion of natural gas (primarily methane) occurs in most household heaters. The heat given off in this reaction is used to raise the temperature of the air in the house. Assuming that all the energy given off in the reaction goes to heating up only the air in the house, determine the mass of
The heat of vaporization of water at 373 K is 40.7 kJ/mol. Find q, w, ΔE, and ΔH for the evaporation of 454 g of water at this temperature at 1 atm.
Find ΔE, ΔH, q, and w for the change in state of 1.0 mol H2O(l ) at 80 °C to H2O( g) at 110 °C. The heat capacity of H2O(l) = 75.3 J/mol K, the heat capacity of H2O( g) = 25.0 J/mol K, and the heat of vaporization of H2O is 40.7 * 103 J/mol at 100 °C.
The heat of combustion of liquid octane (C8H18) to carbon dioxide and liquid water at 298 K is -1303 kJ/mol. Find ΔE for this reaction.
Find ΔH for the combustion of ethanol (C2H6O) to carbon dioxide and liquid water from the following data. The heat capacity of the bomb calorimeter is 34.65 kJ/K, and the combustion of 1.765 g of ethanol raises the temperature of the calorimeter from 294.33 K to 295.84 K.
Which statement is true of the internal energy of the system and its surroundings following a process in which ΔEsys = +65 kJ ?Explain.a. The system and the surroundings both lose 65 kJ of energy.b. The system and the surroundings both gain 65 kJ of energy.c. The system loses 65 kJ of energy and
The internal energy of an ideal gas depends only on its temperature. Which statement is true of an isothermal (constant-temperature) expansion of an ideal gas against a constant external pressure? Explain.a. ΔE is positive. b. w is positive.c. q is positive. d. ΔE is negative.
Which expression describes the heat evolved in a chemical reaction when the reaction is carried out at constant pressure? Explain.a. ΔE - w b. ΔE c. ΔE - q
Two identical new refrigerators are plugged in for the first time. Refrigerator A is empty (except for air) and refrigerator B is filled with jugs of water. The compressors of both refrigerators immediately turn on and begin cooling the interiors of the refrigerators. After two hours, the
A 1-kg cylinder of aluminum and 1-kg jug of water, both at room temperature, are put into a refrigerator. After 1 hour, the temperature of each object is measured. One of the objects is much cooler than the other. Which one is cooler and why?
Two substances A and B, initially at different temperatures, are thermally isolated from their surroundings and allowed to come into thermal contact. The mass of substance A is twice the mass of substance B, but the specific heat capacity of substance B is four times the specific heat capacity of
When 1 mol of a gas burns at constant pressure, it produces 2418 J of heat and does 5 J of work. Determine ΔE, ΔH, q, and w for the process.
Have each group member write a problem involving the transfer of heat from one material in Table 7.4 to another material in the table. Working as a group, solve each problem. The group member who wrote each problem may act as the group facilitator when the group is working on his or her problem.
In an exothermic reaction, the reactants lose energy, and the reaction feels hot to the touch. Explain why the reaction feels hot even though the reactants are losing energy. Where does the energy come from?
Which statement is true of a reaction in which ΔV is positive?Explain.a. ΔH = ΔE b. ΔH > ΔE c. ΔH < ΔE
The heating value of combustible fuels is evaluated based on the quantities known as the higher heating value (HHV) and the lower heating value (LHV). The HHV has a higher absolute value and assumes that the water produced in the combustion reaction is formed in the liquid state. The LHV has a
Classify each process as endothermic or exothermic. What is the sign of ΔH for each process? Explain your answers.a. Gasoline burning in an engine b. Steam condensing on a mirror c. Water boiling in a pot Provide at least two additional examples of exothermic processes and two additional
Calculate the wavelength (in nm) of the red light emitted by a barcode scanner that has a frequency of 4.62 * 1014 s-1.
Which statement best describes the differences between a bright green laser and a dim red laser?(a) The two lasers emit light of the same frequency, and the light from the green laser has a greater amplitude.(b) The two lasers emit light of different frequencies, and the light from the green laser
A nitrogen gas laser pulse with a wavelength of 337 nm contains 3.83 mJ of energy. How many photons does it contain? SORT You are given the wavelength and total energy of a light pulse and asked to find the number of photons it contains. STRATEGIZE In the first part of the conceptual
Which wavelength of light has the highest frequency?a) 10 nm b) 10 mm c) 1 nm d) 1 mm
Why is the quantum-mechanical model of the atom important for understanding chemistry?
Arrange the following types of electromagnetic radiation in order of increasing wavelength: visible, X-ray, infrared.(a) X-ray 6 visible 6 infrared (b) X-ray 6 infrared 6 visible (c) Visible 6 infrared 6 X-ray (d) Infrared 6 X-ray 6 visible
Which kind of electromagnetic radiation contains the greatest energy per photon?a) Microwaves b) Gamma raysc) X-rays d) Visible light
What is light? How fast does it travel in a vacuum?
We shine light of three different wavelengths—325 nm, 455 nm, and 632 nm—on a metal surface and record the following observations for each wavelength, labeled A, B, and C:Observation A: No photoelectrons were observed.Observation B: Photoelectrons with a kinetic energy of 155 kJ/mol were
Calculate the wavelength of an electron traveling with a speed of 2.65 * 106 m/s. SORT You are given the speed of an electron and asked to calculate its wavelength. STRATEGIZE The conceptual plan shows how the de Broglie relation relates the wavelength of an electron to its mass
How much energy (in J) is contained in 1.00 mole of 552-nm photons?a) 3.60 * 10-19 J b) 2.17 * 105 Jc) 3.60 * 10-28 Jd) 5.98 * 10-43 J
Define the wavelength and amplitude of a wave. How are these related to the energy of the wave?
Since quantum-mechanical theory is universal, it applies to all objects, regardless of size. Therefore, according to the de Broglie relation, a thrown baseball should also exhibit wave properties. Why don’t we observe such properties at the ballpark?(a) Because of the baseball’s large mass, its
Light from three different lasers (A, B, and C), each with a different wavelength, was shined onto the same metal surface.Laser A produced no photoelectrons. Lasers B and C both produced photoelectrons, but the photoelectrons produced by laser B had a greater velocity than those produced by laser
What are the quantum numbers and names of the orbitals in the n = 4 principal level?How many n = 4 orbitals exist?
Define the frequency of electromagnetic radiation. How is frequency related to wavelength?
Which statement best summarizes the uncertainty principle?(a) Both the position and the velocity of an electron can be accurately known at the same instant.(b) Either the position or the velocity of an electron can be accurately known at the same instant.(c) Neither the position nor the velocity of
Calculate the wavelength of an electron traveling at 1.85 * 107 m/s.a) 2.54 * 1013 m b) 3.93 * 10-14 mc) 2.54 * 1010 m d) 3.93 * 10-11 m
What determines the color of light? Describe the difference between red light and blue light.
These sets of quantum numbers are each supposed to specify an orbital. One set, however, is erroneous. Which one and why?(a) n = 3; l = 0; ml = 0 (b) n = 2; l = 1; ml = -1(c) n = 1; l = 0; ml = 0 (d) n = 4; l = 1; ml = -2
Which set of three quantum numbers does not specify an orbital in the hydrogen atom? a) n = 2; 1= 1; m₁ = − 1 c) n = 2; 1= 0; m₁ = 0 b) n = 3; 1= d) n = 3; 1= 3; m₁ = −2 2; m₁ = 2
What values of l are possible for n = 3?(a) 0 (or s) (b) 0 and 1 (or s and p)(c) 0, 1, and 2 (or s, p, and d) (d) 0, 1, 2, and 3 (or s, p, d, and f)
Determine the wavelength of light emitted when an electron in a hydrogen atom makes a transition from an orbital in n = 6 to an orbital in n = 5. SORT You are given the energy levels of an atomic transition and asked to find the wavelength of emitted light. STRATEGIZE In the first part of the
What determines the color of a colored object? Explain why grass appears green.
Give an approximate range of wavelengths for each type of electromagnetic radiation and summarize the characteristics and/or the uses of each.a. Gamma rays b. X-raysc. Ultraviolet radiation d. Visible lighte. Infrared radiation f. Microwave radiationg. Radio waves
Which transition emits light with the shortest wavelength? (a) n = 5→→→→→→→n (c) n = 3n = 4 = 2 (b) n=4 → n = 3
Explain the wave behavior known as interference. Explain the difference between constructive and destructive interference.
Which electron transition produces light of the highest frequency in the hydrogen atom? a) 5p - c) 3p 1s 1s b) 4p d) 2p 1s 1s
How much time (in seconds) does it take light in a vacuum to travel 1.00 billion km? a) 3.00 x 10¹7 s c) 3.33 x 10³ s b) 3.33 s d) 3.00 x 1020 s
Explain the wave behavior known as diffraction. Draw the diffraction pattern that occurs when light travels through two slits comparable in size and separation to the light’s wavelength.
Which orbital is a d orbital? a) b) c) d) None of the above
Describe the photoelectric effect. How did experimental observations of this phenomenon differ from the predictions of classical electromagnetic theory?
How did the photoelectric effect lead Einstein to propose that light is quantized?
What is a photon? How is the energy of a photon related to its wavelength? Its frequency?
Describe the Bohr model for the atom. How did the Bohr model account for the emission spectra of atoms?
Explain electron diffraction.
What is the de Broglie wavelength of an electron? What determines the value of the de Broglie wavelength for an electron?

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