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chemistry for engineering students

Chemistry For Engineering Students 4th Edition Lawrence S. Brown, Tom Holme - Solutions

Define the term mean free path.
There are two parameters in the van der Waals equation for real gases. Which parameter corrects for the volume of gas molecules? Use the equation to explain your answer.
Scientists routinely use several different types of pressure gauges, and sometimes a single vacuum chamber may be equipped with more than one type of gauge. Why do you suppose that this is so?
What is actually measured in an ionization gauge pressure sensor? How is this actual measurement related to pressure?
Use the web to find out what type of sensor is used to determine the oxygen pressure in the exhaust manifold of automotive fuel injection system engines.
Do a web search to learn about at least one other type of pressure sensor not described in the chapter. Describe how the gauge operates in a way that your roommate could understand.
Why should temperature always be converted to kelvins when working with gases in problem solving?
What evidence gave rise to the establishment of the absolute temperature scale?
A balloon filled to its maximum capacity on a chilly night at a carnival pops without being touched when it is brought inside. Explain this event.
Why is it dangerous to store compressed gas cylinders in places that could become very hot?
Which postulates of the kinetic theory are the most likely to break down under the conditions of high pressure present inside volcanoes?
Under what conditions do the postulates of the kinetic theory break down?
The following figure shows the distribution of speeds for two samples of N2 gas. One sample is at 300 K, and the other is at 1000k. Which is which? N()/Ntotal 0 500 1000 1500 Molecular speed (m/s) 2000 2500
Use the kinetic theory to explain what happens to the pressure exerted by a gas as its temperature is increased.
Suppose that speed distributions for each of the following gases were added to Figure 5.7. Which of the four gases in the original figure would each most closely resemble? Explain your answer. (a) Ar (b) Ne (c) CH4Figure 5.7 N(v)/N total 0 500 N₂ H₂O 1000 1500 Molecular speed
Why do heavier gases move more slowly than light gases at the same temperature?
Consider a sample of an ideal gas with n and T held constant. Which of the graphs below represents the proper relationship between P and V? How would the graph differ for a sample with a larger number of moles? P P V V P P P V V V
Consider a sample of N2 gas under conditions in which it obeys the ideal gas law exactly. Which of these statements is true?(a) A sample of Ne(g) under the same conditions must obey the ideal gas law exactly.(b) The speed at which one particular N2 molecule is moving changes from time to time.(c)
A gas mixture contains 10.0% CH4 and 90.0% Ar by moles. Find the density of this gas at 250.0°C and 2.50 atm.
Liquid oxygen for use as a rocket fuel can be produced by cooling dry air to -183°C, where the O2 condenses. How many liters of dry air at 25°C and 750 torr would need to be processed to produce 150 L of liquid O2 at -183°C? (The mole fraction of oxygen in dry air is 0.21, and the density of
A number of compounds containing the heavier noble gases, and especially xenon, have been prepared. One of these is xenon hexafluoride (XeF6), which can be prepared by heating a mixture of xenon and fluorine gases. XeF6 is a white crystalline solid at room temperature and melts at about 325 k. A
A 0.2500-g sample of an Al–Zn alloy reacts with HCl to form hydrogen gas:The hydrogen produced has a volume of 0.147 L at 25°C and 755 mm Hg. What is the percentage of zinc in the alloy? 2 Al(s) + 6 H+ (aq) → 2 Al³+ (aq) + 3 H₂(g) Zn(s) + 2 H+ (aq) → Zn²+ (aq) + H₂(g)
You work in a semiconductor production plant that relies on several chlorofluorocarbons in its manufacturing process. One day, you find an unlabeled gas cylinder, and you are assigned to figure out what is in the tank. First, you fill a 1.000-L flask with the gas. At a pressure of 250.0 torr and a
The complete combustion of octane can be used as a model for the burning of gasoline:Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of
A mixture of Ar (0.40 mol), O2 (0.50 mol), and CH4 (0.30 mol) exerts a pressure of 740 mm Hg. If the methane and oxygen are ignited and complete combustion occurs, what is the final pressure of Ar, CO2, H2O, and the remainder of the excess reactant? What is the total pressure of the system?
Some engineering designs call for the use of compressed air for underground work. If water containing iron (II) ions is present, oxygen in the compressed air may react according to the following unbalanced net ionic equation:(a) Write the balanced net ionic equation. Remember that the amounts of
Mining engineers often have to deal with gases when planning for the excavation of coal. Some of these gases, including methane, can be captured and used as fuel to support the mining operation. For a particular mine, 2.4 g of CH4 is present for every 100.0 g of coal that is extracted. If 45.6% of
You are designing a warning system for a semiconductor fabrication facility that must have fewer than 1000 oxygen molecules per cm3 to operate successfully. While researching possible design options, you learn about a new sensor that can detect partial pressures of oxygen in the range of 1–2
Consider the apparatus shown, in which two 1.00-L bulbs are initially separated from one another by a closed valve. One bulb is filled with 500 torr of sulfur dioxide and the other with 400 torr of oxygen, and the entire apparatus is at an initial temperature of 27°C.The valve separating the bulbs
Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a
Pure gaseous nitrogen dioxide (NO2) cannot be obtained, because NO2 dimerizes, or combines with itself, to produce a mixture of NO2 and N2O4. A particular mixture of NO2 and N2O4 has a density of 2.39 g/L at 50°C and 745 torr. What is the partial pressure of NO2 in this mixture?
One of the noble gases (Group 18 in the periodic table) has a density of 1.783 g/L at 0°C and 1 atm. Which noble gas is this?
A mixture of CH4(g) and C3H8(g) with a total pressure of 425 torr is prepared in a reaction vessel. Just enough O2(g) is added to allow complete combustion of the two hydrocarbons. The gas mixture is ignited, and the resulting mixture of CO2(g) and H2O(g) is cooled back to the original temperature.
Aerospace engineers sometimes write the gas law in terms of the mass of the gas rather than the number of moles:In such a formulation, the molar mass of the gas must be incorporated into the value of the gas constant, which means that the gas constant would differ from one gas to another. (We have
A mixture of helium and neon gases has a density of 0.285 g/L at 31.0°C and 374 torr. Find the mole fraction of neon in this mixture.
The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited:A 42.4-g sample of Hg (SCN)2 is placed into a 2.4-L vessel
Before the introduction of unleaded gasoline, the amount of lead in severe pollution episodes in air could be measured at levels of 2.85 μg/m3. Describe how you could determine the number of lead atoms in the active space of your lungs (the air that is actively exchanged during a breath) if the
The best way to generate small amounts of oxygen gas in a laboratory setting is by the decomposition of potassium permanganate:Suppose that you are carrying out an experiment for which you need exactly 2.00 L of oxygen. Describe how you would determine the mass of potassium permanganate needed to
A soft drink can’s label indicates that the volume of the soda it contains is 12 oz or 355 mL. There is probably some empty space at the top of the can. Describe what you can measure and how that measurement allows you to determine the actual density of the soda.
An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what volume of CO2 is evolved during the process. What would have to be measured to predict the needed
Suppose that you are going to collect H2 gas produced from the reaction of an acid with a metal such as zinc.This reaction gives off heat, so the temperature of the solution will increase as the reaction proceeds. You need to know the partial pressure of the H2 you generate as precisely as
Trace analysis may be carried out via nondestructive testing. How does this differ from other types of trace analysis? Give an example of a situation in which non-destructive analysis might be important.
Ammonia is not the only possible fertilizer. Others include urea, which can be produced by the reaction:A scientist has 75 g of dry ice to provide the carbon dioxide. If 4.50 L of ammonia at 15°C and a pressure of 1.4 atm is added, which reactant is limiting? What mass of urea will form? CO,(g) +
A 0.0125-g sample of a gas with an empirical formula of CHF2 is placed in a 165-mL flask. It has a pressure of 13.7 mm Hg at 22.5°C. What is the molecular formula of the compound?
Nitric acid can be prepared by bubbling dinitrogen pentoxide into water.(a) How many moles of H1 are obtained when 1.50 L of N2O5 at 25°C and 1.00 atm pressure is bubbled into water?(b) The solution obtained in part (a) after reaction is complete has a volume of 437 mL. What is the molarity of the
Consider a room that is 14 ft × 20 ft with an 8-ft ceiling.(a) How many molecules of air are present in this room at20°C and 750 torr?(b) If a pollutant is present at 2.3 ppm, how many pollutant molecules are in this room?
Chromium can be detected in atomic absorption spectroscopy by monitoring the absorbance of UV light at a wavelength of 357.8 nm. What is the energy of a photon of this light?Strategy We know the connection between photon energy and wavelength, which is given by Equation 6.3. Again, care with units
Unlike XRF, AAS cannot be used for nondestructive testing. Explain why not.
In a photoelectric effect experiment, ultraviolet light with a wavelength of 337 nm was directed at the surface of a piece of potassium metal. The kinetic energy of the ejected electrons was measured as 2.30 × 10-19j. What is the electron binding energy for potassium?Strategy We know that energy
In analysis by atomic absorption spectroscopy, the wavelengths of light being absorbed reveal the identity of the elements present in the sample. What information is used to determine the relative amounts of the different elements?
The first four energy levels for the hydrogen atom are shown in the diagram below. The lowest energy state is labeled E1, and the higher states are labeled E2, E3, and E4, respectively. When a hydrogen atom undergoes a transition from E3 to E1, it emits a photon with λ = 102.6 nm. Similarly, if
An X-ray fluorescence instrument must include a source of high-energy X-rays. Explain the role of these X-rays in the fluorescence process.
The fluorescence emitted in XRF is also in the X-ray range of the spectrum, but is always at lower energies than the X-rays used to initiate the process. Explain why this must be true.
As part of its analytical capabilities, the Curiosity Mars rover carries a novel instrument called ChemCam. Do a web search to learn what ChemCam does and how it works and write a short paragraph comparing ChemCam to an AAS instrument like the one shown in Figure 6.1.
Write all of the allowed sets of quantum numbers (n, ℓ and mℓ) for a 3p orbital.Strategy The 3p designation tells us the values of the n and, quantum numbers, and we can use the relationship between, and mℓ to determine the possible values of m,ℓ
The presence of sulfur in steel alloys can have a negative effect on ductility and other properties. So trace analysis is often used to monitor the level of sulfur present. What is the electron configuration of a sulfur atom?Strategy We use the energy ordering and number of orbitals for each
If a string of decorative lights includes bulbs with wavelengths of 480, 530, 580, and 700 nm, what are the frequencies of the lights? Use Figure 6.6 to determine which colors are in the set.Figure 6.6 1024 10-16 1022 y-rays 10-14 400 1020 1018 1016 10-12 X-rays UV 10-10 500 Energy
Arrange the following regions of the electromagnetic spectrum in order of increasing frequency: IR, UV, radio wave, visible.
Rewrite the electron configuration for sulfur (Example Problem 6.6) using the shorthand notation introduced earlier.Strategy We found the electron configuration in Example Problem 6.6. Now we simply need to identify the core electrons and replace them with the symbol for the corresponding noble
Calculate the wavelengths, in meters, of radiation of the following frequencies.(a) 5.00 × 1015 s–1, (b) 2.11 × 1014 s–1, (c) 5.44 × 1012 s−1
Tungsten alloys are often used for parts that must withstand high temperatures. Use the periodic table to determine the electron configuration of tungsten (W).Strategy Begin by finding tungsten in the periodic table. Use the rare gas element from the previous period to abbreviate the core
Referring to Figure 6.15, draw a 4p orbital, showing all of its nodes.Figure 6.15 The 3s orbital has two spherical nodes. + A 3p orbital has one planar node (right) and a second hyperbolic node (left). A 3d orbital has two planar nodes.
Define the term nodal plane (or node).
Find the energy of a photon with each of the following frequencies (see Table 1.2 if needed). (a) 15.3 THz, (b) 1.7EHz,(c) 6.22 × 1010 HzTable 1.2
Using only the periodic table, rank the following elements in order of increasing size:Fe, K, Rb, S, and Se.Strategy We want to arrange the elements from smallest to largest. Begin by finding each element in the periodic table. Then use the general trends for atomic size to place them in the
Define the term photon.
For photons with the following energies, calculate the wavelength and identify the region of the spectrum they are from. (a) 3.5 × 10-20 J, (b) 8.7 × 10-26 J,(c) 7.1 × 10-17 J, (d) 5.5 × 10-27 J
For photons with the following energies, calculate the wavelength and identify the region of the spectrum they are from.(a) 6.0 × 10-19 J, (b) 8.7 × 10-22 J, (c) 3.2 × 10-24 J, (d) 1.9 × 10-28 J
Various optical disk drives rely on lasers operating at different wavelengths, with shorter wavelengths allowing a higher density of data storage. For each of the following drive types, find the energy of a single photon at the specified wavelength. (a) CD, λ = 780 nm, (b) DVD, λ = 650 nm, (c)
The laser in most supermarket barcode scanners operates at a wavelength of 632.8 nm. What is the energy of a single photon emitted by such a laser? What is the energy of one mole of these photons?
Assume that a microwave oven operates at a frequency of 1.00 × 1011 s-1.(a) What is the wavelength of this radiation in meters? (b) What is the energy in joules per photon?(c) What is the energy per mole of photons?
Fill in the blanks below to complete a description of the photoelectric effect experiment. (You should be able to do this with just one or two words in each blank.) A beam of — strikes — , causing — to be emitted.
When light with a wavelength of 58.5 nm strikes the surface of tin metal, electrons are ejected with a maximum kinetic energy of 2.69 × 10-18 j. What is the binding energy of these electrons to the metal?
The electron binding energy for copper metal is 7.18 × 10-19j. Find the longest wavelength of light that could eject electrons from copper in a photoelectric effect experiment.
What was novel about Bohr’s model of the atom?
Describe how the Bohr model of the atom accounts for the spectrum of the hydrogen atom.
According to the Bohr model of the atom, what happens when an atom absorbs energy?
The figure below depicts the first four energy levels in a hydrogen atom. The three transitions shown as arrows emit ultraviolet light and occur at wavelengths of 121.566 nm, 102.583 nm, and 97.524 nm, respectively. Find the frequency of light that would be emitted in a transition from the state
Define the term ground state.
A neon atom emits light at many wavelengths, two of which are at 616.4 and 638.3 nm. Both of these transitions are to the same final state.(a) What is the energy difference between the two states for each transition? (b) If a transition between the two higher energy states could be observed, what
A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) If a transition between the two higher energy states could be observed,
How did the observation of electron diffraction affect the development of the quantum mechanical model of the atom?
Why do we use a wave function to describe electrons?
What are the mathematical origins of quantum numbers?
What are the allowed values for the principal quantum number? For the secondary quantum number?
Why are there no 2d orbitals?
Consider a 3d orbital. (a) What are the allowed values for the n and , quantum numbers for a 3d orbital?(b) What are the allowed values for the m, quantum number for a 3d orbital?(c) What is the maximum number of 3d orbitals that could be present in any one atom? (d) What is the maximum number of
Does the fact that the fourth quantum number is called the spin quantum number prove that electrons are spinning? What observations gave rise to this name?
Define the term spin paired.
On what does the Pauli exclusion principle place a limit?
Define the term shielding.
What is effective nuclear charge and how does it influence the size of an orbital?
Depict two ways to place electrons in the 2p orbitals for a nitrogen atom. Which depiction is correct according to Hund’s rule?
Write the ground state electron configuration for (a) B,(b) Ba, (c) Be, (d) Bi, (e) Br.
Halogen lamps rely on the predictable chemistry of the halogen elements. Compare the electron configurations of three halogens and use this comparison to justify the similarity of the chemistry of these elements.
Which of these electron configurations are for atoms in the ground state? In excited states? Which are impossible?(a) 1s22s1, (b) 1s22s22p3, (c) [Ne] 3s23p34s1, (d) [Ne] 3s23p64s33d2,(e) [Ne] 3s23p64 f 4, (f) 1s22s22p43s2
From the list of atoms and ions given, identify any pairs that have the same electron configurations and write that configuration: Na+, S2-, Ne, Ca2+, Fe2+, Kr, I-.
Look at the table of electron configurations in Appendix c. Which elements have configurations that are exceptions to the aufbau principle? Propose a reason why these elements have these exceptions.Data from appendix c
Distinguish between the terms core electrons and valence electrons.
If another 50 elements were discovered, how would you expect the appearance of the periodic table to change?

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