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All Textbook Solutions for Chemistry: Principles and Practice
Define science in your own words. List three fields that are science and three fields that are not science.Compare the uses of the words theory and hypothesis by scientists and by the general public.Explain how the coach of an athletic team might use scientific methods to enhance the teams performance.Some scientists think the extinction of the dinosaurs was due to a collision with a large comet or meteor. Is this statement a hypothesis or a theory? Justify your answer.1.6QEDefine matter, mass, and weight.Matter occupies space and has mass. Are the astronauts in a space shuttle composed of matter while they are weight-less? Explain your answer.Give three examples of homogeneous and heterogeneous mixtures.Do you think it is easier to separate a homogeneous mixture or a heterogeneous mixture, or would both be equally difficult? Explain your answer.A solution made by dissolving sugar in water is homogeneous because the composition is the same everywhere. But if you could look with very high magnification, you would see locations with water particles and other locations with particles of sugar. How can we say that a sugar solution is homogenous?Is the light from an electric bulb an intensive or extensive property?Are all alloys homogeneous solutions? Explain your answer.1.14QE1.16QEDescribe a computation in which your calculator does not display the correct number of significant digits.Draw a block diagram (see Example 1.8) that illustrates the processes used to convert km/hr to m/s.1.19QEIf you repeat the same measurement many times, will you always obtain exactly the same result? Why or why not? What factors influence the repeatability of a measurement?1.21QE1.23QE1.24QEEach of the following parts contains an underlined property. Classify the property as intensive or extensive and as chemical or physical. (a) Bromine is a reddish liquid. (b) A ball is a spherical object. (c) Sodium and chlorine react to form table salt. (d) A sample of water has a mass of 45 g. (e) The density of aluminum is 2.70 g/cm3.1.26QEClassify each of the following processes as a chemical change or a physical change. (a) Water boiling (b) Glass breaking (c) Leaves changing color (d) Iron rustingClassify each of the following processes as a chemical change or a physical change. (a) Tea leaves soaking in warm water (b) A firecracker exploding (c) Magnetization of an iron nail (d) A cake baking1.29QE1.30QE1.31QE1.32QE1.33QEIn the following description of the element iron, identify which of the properties are chemical and which are physical. Iron is rarely found as the free element in nature. Mostly it is found combined with oxygen in an ore. The metal itself can be obtained by reacting the ore with carbon, producing iron and carbon dioxide. Iron is a silver colored metal that conducts heat and electricity well. It is one of the most structurally important metals because of its hardness and mechanical strength, and it makes alloys with many other metals. Stainless steel is one useful alloy of iron that does not corrode in the presence of water and I oxygen, like pure iron does.1.35QEIn the following description of the element bromine, identify which of the properties are chemical and which are physical. Bromine is one of the few elements that is a liquid at room temperature. It is an acrid-smelling substance that reacts readily with most metals. It evaporates easily, so most containers of bromine are filled with visible amounts of red fumes. Most bromine is obtained from sodium bromide, a compound found in salt beds.Classify each of the following as an element, a compound, or a mixture. Identify mixtures as homogeneous or heterogeneous. (a) Air (b) Sugar (c) Cough syrup (d) CadmiumClassify each of the following as an element, a compound, or a mixture. Identify mixtures as homogeneous or heterogeneous. (a) Water (b) Window cleaner (c) 14-karat gold (d) Copper1.39QEClassify each of the following as an element, a compound, or a mixture. (a) Gold (b) Milk (c) Sugar (d) Vinaigrette dressing with herbs1.41QE1.42QEA samples true mass is 2.54 g. For each set of measurements, characterize the set as accurate, precise, both, or neither. (a) 2.50, 2.55, 2.59, 2.60 (b) 2.53, 2.54, 2.54, 2.55 (c) 2.49, 2.51, 2.53, 2.63 (d) 2.44, 2.44, 2.45, 2.47A measurements true value is 17.3 g. For each set of measurements, characterize the set as accurate, precise, both, or neither. (a) 17.2, 17.2, 17.3, 17.3 g (b) 16.9, 17.3, 17.5, 17.9 g (c) 16.9, 17.2, 17.9, 18.8 g (d) 17.8, 17.8, 17.9, 18.0 gHow many significant figures are in each value? (a) 1.5003 (b) 0.007 (c) 5.70 (d) 2.00 107How many significant figures are there in each of the following? (a) 0.136 m (b) 0.0001050 g (c) 2.700 103 nm (d) 6 104 L (e) 56003 cm3How many significant figures are in each measurement? (a) 5 103 m (b) 5.0005 g/mL (c) 22.9898 g (d) 0.0040 VHow many significant figures are in each measurement? (a) 3.1416 degrees (b) 0.00314 K (c) 1.0079 s (d) 6.022 1023 particlesExpress the measurements to the requested number of significant figures. (a) 96,485 J/C to three significant figures (b) 2.9979 g/cm3 to three significant figures (c) 0.0597 mL to one significant figure (d) 6.626 1034 kg to two significant figures1.50QE1.51QE1.52QE1.53QE1.54QE
Perform the indicated calculations, and express the answer to the correct number of significant figures. Use scientific notation where appropriate.
13.51 + 0.0459
16.45/32.0 + 10
3.14 × 104 − 15.0
7.18 × 103 ÷ 1.51 × 105
1.56QE1.57QE1.58QECalculate the result of the following equation, and use the convention of significant figures to express the answer correctly. x=10121101211.01Calculate the result of the following equation, and use the convention of significant figures to express the uncertainty in the answer. x=2.0510653.41051+1.91031.61QEWhat base SI unit is used to express each of the following quantities? (a) The mass of a bag of flour (b) The distance from the Earth to the Sun (c) The temperature of a sunny August day (d) The time it takes to run a marathon (26.2 miles)1.63QEWrite two conversion factors between grams (g) and megagrams (Mg).1.65QE1.66QE1.67QE1.68QEThe speed of sound in air at sea level is 340 m/s. Express this speed in miles per hour.
The area of the 48 contiguous states is 3.02 × 106 mi2. Assume that these states are completely flat (no mountains and no valleys). What volume of water, in liters, would cover these states with a rainfall of two inches?
1.71QE1.72QE1.73QE1.74QE1.75QE1.76QEWine is sold in 750-mL bottles. How many quarts of wine are in a case of 12 bottles?The speed limit on limited-access roads in Canada is 100 km/h. How fast is this in miles per hour? In meters per second?1.79QEMany soft drinks are sold in 2.00-L containers. How many fluid ounces is this?(a) Helium has the lowest boiling point of any substance; it boils at 4.21 K. Express this temperature in degrees Celsius and degrees Fahrenheit. (b) The oven temperature for a roast is 400 F. Convert this temperature to degrees Celsius.(a) The boiling point of octane is 126 C. What is this temperature in degrees Fahrenheit and in kelvins? (b) Potatoes are cooked in oil at a temperature of 350 F. Convert this temperature to degrees Celsius.The melting point of sodium chloride, table salt, is 801 C. What is this temperature in degrees Fahrenheit and in kelvins?1.86QEThe density of benzene at 25.0 C is 0.879 g/cm3. What is the volume, in liters, of 2.50 kg benzene?Ethyl acetate, one of the compounds in nail polish remover, has a density of 0.9006 g/cm3. Calculate the volume of 25.0 g ethyl acetate.Lead has a density of 11.4 g/cm3. What is the mass, in kilograms, of a lead brick measuring 8.50 5.10 3.20 cm?1.90QEAn irregularly shaped piece of metal with a mass of 147.8 g is placed in a graduated cylinder containing 30.0 mL water. The water level rises to 48.5 mL. What is the density of the metal in g/cm3?A solid with an irregular shape and a mass of 11.33 g is added to a graduated cylinder filled with water (d = 1.00 g/mL) to the 35.0-mL mark. After the solid sinks to the bottom, the water level is read to be at the 42.3-mL mark. What is the density of the solid?How many square meters will 4.0 L (about 1 gal) of paint cover if it is applied to a uniform thickness of 8.00 102 mm (volume = thickness area)?1.94QE1.95QE1.96QEGold leaf, which is used for many decorative purposes, is made by hammering pure gold into very thin sheets. Assuming that a sheet of gold leaf is 1.27 105 cm thick, how many square feet of gold leaf could be obtained from 28.35 g gold? The density of gold is 19.3 g/cm3.1.98QE1.99QE1.101QE1.102QE1.103QE1.104QEThe main weapon on a military tank is a cannon that fires a blunt projectile specially designed to cause a shock wave when it hits another tank. The projectile fits into a finned casing that improves its accuracy. Calculate the mass of the projectile, assuming it is a cylinder of uranium (density = 19.05 g/cm3) that is 105 mm in diameter and 30 cm in height. The volume of a cylinder is given by the equation V = r2h1.106QE2.1QEState how Daltons atomic theory explains (a) the law of conservation of mass. (b) the law of constant composition.2.3QE2.4QE2.5QE2.6QE2.7QEDescribe the arrangement of protons, neutrons, and electrons in an atom.2.9QE2.10QEA mass spectrometer determines isotopic masses to eight or nine significant digits. What limits the atomic mass of carbon to only five significant digits?2.12QE2.13QE2.14QE2.15QE2.16QESulfur dioxide, SO2, is a molecular compound that contributes to acid rain, and CaCO3 is an ionic compound that can neutralize acid rain. Explain the difference in the meanings of these two formulas.2.18QE2.19QE2.20QE2.21QE2.22QE2.23QE2.24QE2.25QE2.26QE2.27QE2.28QE2.29QEGive the complete symbol (XZA), including atomic number and mass number, of (a) a nickel atom with 31 neutrons, and (b) a tungsten atom with 110 neutrons.2.31QE2.32QE2.33QE2.34QE2.35QE2.36QE2.37QE2.38QE2.39QE2.40QE2.41QE2.42QE2.43QE2.44QE2.45QE2.46QE2.47QE2.48QE2.49QE2.50QE2.51QE2.52QE2.53QE2.54QE2.55QE2.56QE2.57QE2.58QE2.59QE2.60QE2.61QE2.62QE2.63QE2.64QE2.65QE2.66QE2.67QE2.68QE2.69QE2.70QE2.71QE2.72QE2.73QE2.74QE2.75QE2.76QE2.77QE2.78QE2.79QE2.80QE2.81QE2.82QE2.83QE2.84QE2.85QE2.86QE2.87QE2.88QE2.89QE2.90QE2.91QE2.92QE2.93QE2.94QE2.95QE2.96QEWrite the formula of (a) manganese(III) sulfide. (b) iron(II) cyanide. (c) potassium sulfide. (d) mercury(II) chloride.2.98QE2.99QE2.100QE2.101QE2.102QE2.103QE2.104QE2.105QE2.106QE2.107QE2.108QE2.109QE2.110QE2.111QE2.112QE2.113QE2.114QE2.115QE2.116QE2.117QE2.118QE2.119QE2.120QE2.121QE2.122QE2.123QE2.124QE2.125QE2.126QE2.127QE2.128QE2.129QE2.130QE2.131QE2.132QE2.133QE2.134QE2.135QE2.136QE3.1QE3.2QEUsing solid circles for H atoms and open circles for O atoms, make a drawing that shows the molecular level representation for the balanced equation of H2 and O2 reacting to form H2O.3.4QE3.5QEHow many objects are in 1 mol? What is the common name for this number of objects?3.7QE3.8QE3.11QEDescribe an experiment that would enable someone to determine the percentages of carbon and hydrogen in a sample of a newly prepared hydrocarbon.Only the empirical formula can be calculated from percentage composition data. What additional information is needed to calculate the molecular formula from the empirical formula, and if given this information, how is the molecular formula determined?3.14QE3.15QE3.16QE3.17QE3.18QE3.19QEA mixture of sulfur dioxide and oxygen gas reacts as shown below. (a) Write the balanced equation (remember to express the coefficients as the lowest set of whole numbers) (b) Name the product.3.21QE3.22QE3.23QE3.24QE3.25QE3.26QE3.27QE3.28QE3.29QE3.30QE3.31QE3.32QE3.33QE3.34QE3.35QE3.36QEAcetone, (CH3)2CO, is an important industrial compound. Although its toxicity is relatively low, workers using it must be careful to avoid flames and sparks because this compound burns readily in air. Write the balanced equation for the combustion of acetone.3.38QE3.39QE3.40QE3.41QE3.42QE3.43QE3.44QE3.45QE3.46QE3.47QE3.48QE
One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack emissions is by reaction with ammonia gas, NH3. The products of the reaction, N2 and H2O, are not toxic. Write the balanced equation for this reaction. Assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
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