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chemistry a molecular approach
Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions
The human body obtains 915 kJ of energy from a candy bar.If this energy were used to vaporize water at 100.0 °C, how much water (in liters) could be vaporized? (Assume the density of water is 1.00 g/mL.)
A 100.0-mL sample of water is heated to its boiling point. How much heat (in kJ) is required to vaporize it? (Assume a density of 1.00 g/mL.)
Suppose that 0.95 g of water condenses on a 75.0-g block of iron that is initially at 22 °C. If the heat released during condensation goes only to warming the iron block, what is the final temperature (in °C) of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 kJ/mol.)
Suppose that 1.15 g of rubbing alcohol (C3H8O) evaporates from a 65.0-g aluminum block. If the aluminum block is initially at 25 °C, what is the final temperature of the block after the evaporation of the alcohol? Assume that the heat required for the vaporization of the alcohol comes only from
This table displays the vapor pressure of ammonia at several different temperatures. Use the data to determine the heat of vaporization and normal boiling point of ammonia. Temperature Pressure (K) (torr) 200 65.3 210 134.3 220 255.7 230 456.0 235 597.0
This table displays the vapor pressure of nitrogen at several different temperatures. Use the data to determine the heat of vaporization and normal boiling point of nitrogen. Temperature Pressure (K) (torr) 65 130.5 289.5 570.8 1028 1718 70 75 80 85
Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 °C. What is the vapor pressure of ethanol at 15 °C?
Benzene has a heat of vaporization of 30.72 kJ/mol and a normal boiling point of 80.1 °C. At what temperature does benzene boil when the external pressure is 445 torr?
Carbon disulfide has a vapor pressure of 363 torr at 25 °C and a normal boiling point of 46.3 °C. Find ΔHvap for carbon disulfide.
Methylamine has a vapor pressure of 344 torr at -25 °C and a boiling point of -6.4 °C. Find ΔHvap for methylamine.
How much energy is released when 65.8 g of water freezes?
Calculate the amount of heat required to completely sublime 50.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol.
An 8.5-g ice cube is placed into 255 g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water.
How much ice (in grams) would have to melt to lower the temperature of 352 mL of water from 25 °C to 5 °C? (Assume the density of water is 1.0 g/mL.)
How much heat (in kJ) is required to warm 10.0 g of ice, initially at -10.0 °C, to steam at 110.0 °C? The heat capacity of ice is 2.09 J/g · °C, and that of steam is 2.01 J/g · °C.
Nitrogen has a normal boiling point of 77.3 K and a melting point (at 1 atm) of 63.1 K. Its critical temperature is 126.2 K, and its critical pressure is 2.55 * 104 torr. It has a triple point at 63.1 K and 94.0 torr. Sketch the phase diagram for nitrogen.Does nitrogen have a stable liquid state at
Show how the fluorite structure accommodates a cation-toanion ratio of 1:2.
The phase diagram for sulfur is shown here. The rhombic and monoclinic states are two solid states with different structures.a. Below what pressure does solid sulfur sublime?b. Which of the two solid states of sulfur is more dense? Pressure Rhombic Monoclinic Liquid 119 °C, 0.027 mmHg 96 °C,
The high-pressure phase diagram of ice is shown here. Notice that, under high pressure, ice can exist in several different solid forms. What three forms of ice are present at the triple point marked O? How does the density of ice II compare to ice I (the familiar form of ice)? Would ice III sink or
Water has a high boiling point given its relatively low molar mass. Why?
Water is a good solvent for many substances. What is the molecular basis for this property, and why is it significant?
Explain the role of water in moderating Earth’s climate.
How is the density of solid water compared to that of liquid water atypical among substances? Why is this significant?
Explain the observed trend in the melting points of the hydrogen halides. HI HBr HCI HF -50.8 °C -88.5 °C -114.8 °C -83.1 °C
Explain the observed trend in the boiling points of these compounds. H₂Te H₂Se H₂S H₂O -2°C -41.5 °C -60.7 °C 100 °C
The vapor pressure of water at 25 °C is 23.76 torr. If 1.25 g of water is enclosed in a 1.5-L container, will any liquid be present?If so, what mass of liquid?
The vapor pressure of CCl3F at 300 K is 856 torr. If 11.5 g of CCl3F is enclosed in a 1.0-L container, will any liquid be present?If so, what mass of liquid?
Examine the phase diagram for iodine shown in Figure 12.39(a).FIGURE 12.39aWhat state transitions occur as we uniformly increase the pressure on a gaseous sample of iodine from 0.010 atm at 185 °C to 100 atm at 185 °C? Make a graph, analogous to the heating curve for water shown in Figure 12.36.
Carbon tetrachloride displays a triple point at 249.0 K and a melting point (at 1 atm) of 250.3 K. Which state of carbon tetrachloride is more dense, the solid or the liquid? Explain.
Four ice cubes at exactly 0 °C with a total mass of 53.5 g are combined with 115 g of water at 75 °C in an insulated container. If no heat is lost to the surroundings, what is the final temperature of the mixture?
Draw a heating curve (such as the one in Figure 12.36) for 1 mole of methanol beginning at 170 K and ending at 350 K.Assume that the values given here are constant over the relevant temperature ranges. Melting point Boiling point A Hius A Hvap Cs, solid Cs, liquid Cs, ga 176 K 338 K 2.2 kJ/mol 35.2
A sample of steam with a mass of 0.552 g and at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °C. Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?
Draw a heating curve (such as the one in Figure 12.36) for 1 mol of benzene beginning at 0 °C and ending at 100 °C. Assume that the values given here are constant over the relevant temperature ranges. Melting point Boiling point A Hius A Hvap Cs, solid Cs, liquid Cs, gas 5.4 °C 80.1 °C 9.9
Air conditioners not only cool air but dry it as well. A room in a home measures 6.0 m * 10.0 m * 2.2 m. If the outdoor temperature is 30 °C and the partial pressure of water in the air is 85% of the vapor pressure of water at this temperature, what mass of water must be removed from the air each
Based on the phase diagram of CO2 shown in Figure 12.39(b), describe the state changes that occur when the temperature of CO2 is increased from 190 K to 350 K at a constant pressure of (a) 1 atm, (b) 5.1 atm, (c) 10 atm, and (d) 100 atm. Carbon Dioxide Pressure (not to scale) 72.9 atm 5.1 atm 1
A sealed flask contains 0.55 g of water at 28 °C. The vapor pressure of water at this temperature is 28.35 mmHg. What is the minimum volume of the flask in order that no liquid water be present in the flask?
Consider a planet where the pressure of the atmosphere at sea level is 2500 mmHg. Does water behave in a way that can sustain life on the planet?
Liquid nitrogen can be used as a cryogenic substance to obtain low temperatures. Under atmospheric pressure, liquid nitrogen boils at 77 K, allowing low temperatures to be reached. However, if the nitrogen is placed in a sealed, insulated container connected to a vacuum pump, even lower
Given that the heat of fusion of water is -6.02 kJ/mol, the heat capacity of H2O(l) is 75.2 J/mol · K, and the heat capacity of H2O(s) is 37.7 J/mol · K, calculate the heat of fusion of water at -10 °C.
Two liquids, A and B, have vapor pressures at a given temperature of 24 mmHg and 36 mmHg, respectively. We prepare solutions of A and B at a given temperature and measure the total pressures above the solutions. We obtain these data:Predict the total pressure above a solution of 5 mol A and 1 mol
The heat of combustion of CH4 is 890.4 kJ/mol, and the heat capacity of H2O is 75.2 J/mol · K. Find the volume of methane measured at 298 K and 1.00 atm required to convert 1.00 L of water at 298 K to water vapor at 373 K.
Three 1.0-L flasks, maintained at 308 K, are connected to each other with stopcocks. Initially, the stopcocks are closed. One of the flasks contains 1.0 atm of N2; the second, 2.0 g of H2O; and the third, 0.50 g of ethanol, C2H6O. The vapor pressure of H2O at 308 K is 42 mmHg, and that of ethanol
Butane (C4H10) has a heat of vaporization of 22.44 kJ/mol and a normal boiling point of -0.4 °C. A 250-mL sealed flask contains 0.55 g of butane at -22 °C. How much butane is present as a liquid? If the butane is warmed to 25 °C, how much is present as a liquid?
The following image is an electrostatic potential map for ethylene oxide, (CH2)2O, a polar molecule. Use the electrostatic potential map to predict the geometry for how one ethylene oxide molecule interacts with another. Draw structural formulas, using the 3D bond notation introduced in Section
One prediction of global warming is the melting of global ice, which may result in coastal flooding. A criticism of this prediction is that the melting of icebergs does not increase ocean levels any more than the melting of ice in a glass of water increases the level of liquid in the glass. Is this
The rate of vaporization depends on the surface area of the liquid.However, the vapor pressure of a liquid does not depend on the surface area. Explain.
Substance A has a smaller heat of vaporization than substance B.Which of the two substances will undergo a larger change in vapor pressure for a given change in temperature?
The density of a substance is greater in its solid state than in its liquid state. If the triple point in the phase diagram of the substance is below 1.0 atm, which will necessarily be at a lower temperature, the triple point or the normal melting point?
Examine the heating curve for water in Section 12.7 (Figure 12.36). If heat is added to the water at a constant rate, which of the three segments in which temperature is rising will have the least steep slope? Why? Temperature (°C) 125 100 75 Ice warming 0.941
A substance has a heat of vaporization of ΔHvap and a heat of fusion of ΔHfus. Express the heat of sublimation in terms of ΔHvap and ΔHfus.
A root cellar is an underground chamber used to store fruits, vegetables, and even meats. In extreme cold, farmers put large vats of water into the root cellar to prevent the fruits and vegetables from freezing. Explain why this works.
Refer to Figure 12.36 to answer each question.a. A sample of steam begins on the line segment labeled 5 on the graph. Is heat absorbed or released in moving from the line segment labeled 5 to the line segment labeled 3? What is the sign of q for this change?b. In moving from left to right along the
Suggest an explanation for the observation that the heat of fusion of a substance is always smaller than its heat of vaporization.
The boiling points of three compounds are tabulated here.Answer the following questions without looking up the structures for these molecules: Which compound experiences hydrogen bonding? Which compound is polar but is unable to experience hydrogen bonding? Which is neither polar nor capable of
The vapor pressure for pure water and pure acetone is measured as a function of temperature. In each case, a graph of the log of the vapor pressure versus 1/T is found to be a straight line. The slope of the line for water is -4895 K, and the slope of the line for acetone is -3765 K. Determine
Based on the heating curve for water, does it take more energy to melt a mole of water or to boil a mole of water? Does it take more energy to warm the solid, the liquid, or the gas by 10 °C?Explain your answers clearly.
We have seen that molar mass and molecular structure influence the boiling point of a substance. We can see these two factors at work in the boiling points of the group 6A hydrides shown in the following graph.In order to disentangle the effects of molar mass and molecular structure on the boiling
Sketch the phase diagram for carbon dioxide. If you have carbon dioxide at 1.0 atm and 25 °C, could you make it a liquid by cooling it down? How could you make it a liquid at 25 °C? If you increase the pressure of carbon dioxide that is at body temperature (37 °C), will it ever liquefy?
When an X-ray beam of λ = 154 pm is incident on the surface of an iron crystal, it produces a maximum diffraction at an angle of θ = 32.6°. Assuming n = 1, calculate the separation between layers of iron atoms in the crystal.
A body-centered cubic unit cell has an edge length of 588 pm. What is the radius of the atoms composing the unit cell?(a) 588 pm (b) 294 pm (c) 255 pm (d) 208 pm
An X-ray beam of λ = 154 pm is incident on the surface of an unknown metallic crystal. It produces a maximum diffraction at an angle of θ = 29.1°. Assuming n = 1, calculate the separation between layers of metal atoms in the crystal.a) 316 pmb) 105 pmc) 154 pmd) 158 pm
What is graphene? Why is graphene unique?
Calculate the packing efficiency of the simple cubic unit cell.
How many atoms are in the unit cell in the face-centered cubic structure?(a) 1 (b) 2 (c) 4 (d) 14
How many atoms are in the body-centered cubic unit cell?a) 1b) 2c) 4d) 5
Explain the basic principles involved in X-ray crystallography.Include Bragg’s law in your explanation.
A body-centered cubic unit cell has a volume of 4.32 * 10- 23 cm3. Find the radius of the atom in pm.
Aluminum crystallizes with a face-centered cubic unit cell. The radius of an aluminum atom is 143 pm.Calculate the density of solid crystalline aluminum in g/cm3. SORT You are given the radius of an aluminum atom and its crystal structure. You are asked to find the density of
Which solid would you expect to have the highest melting point?(a) MgO(s) (b) I2(s) (c) Kr(s)
What is the coordination number of an atom in a facecentered unit cell?a) 4b) 6c) 8d) 12
What is a crystalline lattice? How is the lattice represented with the unit cell?
Which compound is most likely to crystallize in the zinc blende structure?(a) RbCl (Rb+ radius = 148 pm; Cl– radius = 181 pm)(b) MgCl2 (Mg2+ radius = 65 pm; Cl– radius = 181 pm)(c) CuI (Cu+ radius = 96 pm; I– radius = 216 pm)
Classify each crystalline solid as molecular, ionic, or atomic.(a) Au(s) (b) CH3CH2OH(s) (c) CaF2(s)
What is the packing efficiency of the face-centered cubic unit cell?a) 52 %b) 68 %c) 74%d) 88%
Make a drawing of each unit cell: simple cubic, body-centered cubic, and face-centered cubic.
High pressure favors the formation of diamond from graphite. What can you conclude about the relative densities of the two substances?(a) Diamond is denser than graphite.(b) Graphite is denser than diamond.(c) Nothing can be determined about the relative densities of the two substances without more
What is the edge length of a body-centered cubic unit cell made up of atoms that each has a radius of 168 pm?a) 388 pmb) 336 pmc) 475 pmd) 84 pm
For each of the cubic cells in the previous problem, give the coordination number, edge length in terms of r, and number of atoms per unit cell.Previous problemMake a drawing of each unit cell: simple cubic, body-centered cubic, and face-centered cubic.
Which element would you dope into germanium to create a p-type semiconductor?(a) Indium (b) Tin (c) Arsenic
Rhodium crystallizes in a face-centered cubic unit cell. The radius of a rhodium atom is 135 pm. Determine the density of rhodium in g/cm3.a) 3.07 g/cm3b) 12.3 g/cm3c) 278 g/cm3d) 0.337 g/cm3
What is the difference between hexagonal closest packing and cubic closest packing? What are the unit cells for each of these structures?
Which type of solid is dry ice (solid carbon dioxide)?a) Ionicb) Molecularc) Atomicd) None of the above
What are the three basic types of solids and the composite units of each? What types of forces hold each type of solid together?
Which solid has the highest melting point?a) CS2(s)b) CaF2(s)c) C8H18(s)d) Ar(s)
What are the three categories of atomic solids?
Which material is a common oxide ceramic?a) N2Ob) Al2O3c) Fe2O3d) CuO
What kinds of forces hold each of the three basic categories of atomic solids together?
What is the main component of glass?a) Al2O3b) SiO2c) CaF2d) SiC
Which substance has the greatest band gap?a) Siliconb) Germaniumc) Leadd) Gold
In an ionic compound, how are the relative sizes of the cation and anion related to the coordination number of the crystal structure?
Which element produces a p-type semiconductor when doped into silicon?a) Geb) Asc) Gad) Sb
Show how the cesium chloride, sodium chloride, and zinc blende unit cells each contain a cation-to-anion ratio of 1:1.
Which monomer produces the addition polymer shown here? CH-CH₂-CH-CH₂-CH... | F I F (a) H₂C=CH₂ (b) HC=CH2 F (c) HC=CH II F F (d) F-C=C-F F F T F
Name and describe the different allotropes of carbon.
What are silicates? What is quartz?
What is the definition of a ceramic? What are the three categories of ceramics?
List the major and minor components of Portland cement.What is the difference between the hardening process of Portland cement and the hardening process of clays?
How is concrete made from Portland cement? What advantage does concrete have for building compared to the construction methods that predated the development of concrete?
Describe what happens on the molecular level when silica is heated and then cooled to make glass.
Describe the difference between vitreous silica and soda-lime glass. What are some advantages and disadvantages of each of these types of glass?
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