Chapter 1

Write each of the following in terms of the SI base unit (that is, express the prefix as the power of 10 ). a \(6.6 \mathrm{mK} \quad\) b \(275 \mathrm{pm}\) c \(22.1 \mathrm{~ms}\) d \(45 \mu \mathrm{m}\)

Tungsten metal, which is used in lightbulb filaments, has the highest melting point of any metal \(\left(3410^{\circ} \mathrm{C}\right) .\) What is this melting point in degrees Fahrenheit?

Titanium metal is used in aerospace alloys to add strength and corrosion resistance. Titanium melts at \(1677^{\circ} \mathrm{C}\). What is this temperature in degrees Fahrenheit?

Calcium carbonate, a white powder used in toothpastes, antacids, and other preparations, decomposes when heated to about \(825^{\circ} \mathrm{C}\). What is this temperature in degrees Fahrenheit?

Sodium hydrogen carbonate (baking soda) starts to decompose to sodium carbonate (soda ash) at about \(50^{\circ} \mathrm{C}\). What is this temperature in degrees Fahrenheit?

Gallium metal can be melted by the heat of one's hand. Its melting point is \(29.8^{\circ} \mathrm{C}\). What is this temperature in kelvins? in degrees Fahrenheit?

Mercury metal is liquid at normal temperatures but freezes at \(-38.9^{\circ} \mathrm{C}\). What is this temperature in kelvins? in degrees Fahrenheit?

Zinc metal can be purified by distillation (transforming the liquid metal to vapor, then condensing the vapor back to liquid). The metal boils at normal atmospheric pressure at \(1666^{\circ} \mathrm{F}\). What is this temperature in degrees Celsius? in kelvins?

Iodine is a bluish-black solid. It forms a violetcolored vapor when heated. The solid melts at \(236^{\circ} \mathrm{F}\). What is this temperature in degrees Celsius? in kelvins?

An aluminum alloy used in the construction of aircraft wings has a density of \(2.70 \mathrm{~g} / \mathrm{cm}^{3}\). Express this density in SI units \(\left(\mathrm{kg} / \mathrm{m}^{3}\right)\).

Vanadium metal is added to steel to impart strength. The density of vanadium is \(5.96 \mathrm{~g} / \mathrm{cm}^{3}\). Express this in SI units \(\left(\mathrm{kg} / \mathrm{m}^{3}\right)\).

The density of quartz mineral was determined by adding a weighed piece to a graduated cylinder containing \(52.2 \mathrm{~mL}\) water. After the quartz was submerged, the water level was \(67.1 \mathrm{~mL}\). The quartz piece weighed \(39.8 \mathrm{~g}\). What was the density of the quartz?

Hematite (iron ore) weighing \(70.7 \mathrm{~g}\) was placed in a flask whose volume was \(53.2 \mathrm{~mL}\). The flask with hematite was then carefully filled with water and weighed. The hematite and water weighed \(109.3 \mathrm{~g}\). The density of the water was \(0.997 \mathrm{~g} / \mathrm{cm}^{3} .\) What was the density of the hematite?

Some bottles of colorless liquids were being labeled when the technicians accidentally mixed them up and lost track of their contents. A \(15.0-\mathrm{mL}\) sample withdrawn from one bottle weighed \(22.3 \mathrm{~g}\). The technicians knew that the liquid was either acetone, benzene, chloroform, or carbon tetrachloride (which have densities of \(0.792 \mathrm{~g} / \mathrm{cm}^{3}\), \(0.899 \mathrm{~g} / \mathrm{cm}^{3}, 1.489 \mathrm{~g} / \mathrm{cm}^{3},\) and \(1.595 \mathrm{~g} / \mathrm{cm}^{3},\) respectively). What was the identity of the liquid?

Providing no reaction occurs, a solid will float on any liquid that is more dense than it is. The volume of a piece of calcite weighing \(35.6 \mathrm{~g}\) is \(12.9 \mathrm{~cm}^{3} .\) On which of the following liquids will the calcite float: carbon tetrachloride (density \(=1.60 \mathrm{~g} / \mathrm{cm}^{3}\) ), methylene bromide (density = \(\left.2.50 \mathrm{~g} / \mathrm{cm}^{3}\right),\) tetrabromoethane (density \(\left.=2.96 \mathrm{~g} / \mathrm{cm}^{3}\right),\) or methylene iodide (density \(\left.=3.33 \mathrm{~g} / \mathrm{cm}^{3}\right) ?\)

Platinum metal is used in jewelry; it is also used in automobile catalytic converters. What is the mass of a cube of platinum \(4.40 \mathrm{~cm}\) on an edge? The density of platinum is \(21.4 \mathrm{~g} / \mathrm{cm}^{3}\).

Ultrapure silicon is used to make solid-state devices, such as computer chips. What is the mass of a circular cylinder of silicon that is \(12.40 \mathrm{~cm}\) long and has a radius of \(4.00 \mathrm{~cm} ?\) The density of silicon is \(2.33 \mathrm{~g} / \mathrm{cm}^{3}\).

Vinegar contains acetic acid (about \(5 \%\) by mass). Pure acetic acid has a strong vinegar smell but is corrosive to the skin. What volume of pure acetic acid has a mass of \(35.00 \mathrm{~g} ?\) The density of acetic acid is \(1.053 \mathrm{~g} / \mathrm{mL}\).

Ethyl acetate has a characteristic fruity odor and is used as a solvent in paint lacquers and perfumes. An experiment requires \(0.070 \mathrm{~kg}\) of ethyl acetate. What volume is this (in liters)? The density of ethyl acetate is \(0.902 \mathrm{~g} / \mathrm{mL}\).

Convert: a \(8.45 \mathrm{~kg}\) to micrograms b \(318 \mu\) s to milliseconds c \(93 \mathrm{~km}\) to nanometers d \(37.1 \mathrm{~mm}\) to centimeters

Convert: a \(127 \AA\) A to micrometers b \(21.0 \mathrm{~kg}\) to milligrams c \(1.09 \mathrm{~cm}\) to millimeters d \(4.6 \mathrm{~ns}\) to microseconds

Convert: a \(5.91 \mathrm{~kg}\) of chrome yellow to milligrams b \(753 \mathrm{mg}\) of vitamin \(\mathrm{A}\) to micrograms c \(90.1 \mathrm{MHz}\) (megahertz), the wavelength of an FM signal, to kilohertz d \(498 \mathrm{~mJ}\) (the joule, \(\mathrm{J}\), is a unit of energy) to kilojoules

Convert: a \(7.19 \mu \mathrm{g}\) of cyanocobalamin (vitamin \(\mathrm{B}_{12}\) ) to milligrams b \(104 \mathrm{pm},\) the radius of a sulfur atom, to angstroms c \(0.010 \mathrm{~mm}\), the diameter of a typical blood capillary, to centimeters d) \(0.0605 \mathrm{kPa}\) (the pascal, \(\mathrm{Pa}\), is a unit of pressure) to centipascals

The largest of the Great Lakes is Lake Superior, which has a volume of \(12,230 \mathrm{~km}^{3}\). What is this volume in liters?

The average flow of the Niagara River is \(3.50 \mathrm{~km}^{3}\) per week. What is this volume in liters?

A room measures \(10.0 \mathrm{ft} \times 11.0 \mathrm{ft}\) and is \(9.0 \mathrm{ft}\) high. What is its volume in liters?

A cylindrical settling tank is \(5.0 \mathrm{ft}\) deep and has a radius of \(15.0 \mathrm{ft}\). What is the volume of the tank in liters?

The masses of diamonds and gems are measured in carats. A carat is defined as \(200 \mathrm{mg}\). If a jeweler has 384 carats of diamonds, how many grams does she have?

One year of world production of gold was \(49.6 \times 10^{6}\) troy ounces. One troy ounce equals \(31.10 \mathrm{~g}\). What was the world production of gold in metric tons \(\left(10^{6} \mathrm{~g}\right)\) for that year?

What are some characteristics of the adhesive used for Post-it Notes?

What do the various chromatographic separation techniques have in common?

Describe how gas chromatography works.

When the quantity \(5 \times 10^{-2} \mathrm{mg}\) is subtracted from \(4.7 \mathrm{mg}\), how many significant figures should be reported in the answer?

A 33.0 -g sample of an unknown liquid at \(20.0^{\circ} \mathrm{C}\) is heated to \(120^{\circ} \mathrm{C}\). During this heating, the density of the liquid changes from \(0.854 \mathrm{~g} / \mathrm{cm}^{3}\) to \(0.797 \mathrm{~g} / \mathrm{cm}^{3}\). What volume would this sample occupy at \(120^{\circ} \mathrm{C} ?\)

A 124 -g sample of a pure liquid, liquid \(A\), with a density of \(3.00 \mathrm{~g} / \mathrm{mL}\) is mixed with a \(40.8-\mathrm{mL}\) sample of a pure liquid, liquid \(\mathrm{B}\), with a density of \(2.00 \mathrm{~g} / \mathrm{mL}\). What is the total volume of the mixture? (Assume there is no reaction upon the mixing of \(\mathrm{A}\) and \(\mathrm{B}\), and volumes are additive.)

Catalytic converters are used in automobiles to convert harmful gaseous substances in the exhaust to more benign substances, for example, carbon monoxide to carbon dioxide. Beads used in these converters have extremely large surface areas. For instance, a single \(3.0-\mathrm{mm}\) porous bead-can have a surface area of \(1.0 \times 10^{6} \mathrm{~cm}^{2}\). If a car has two catalytic converters, each with \(5.0 \times 10^{3}\) beads, calculate the surface area of the two catalytic converters in \(\mathrm{km}^{2}\)

The density of liquid water at \(80^{\circ} \mathrm{C}\) is \(972 \mathrm{~kg} / \mathrm{m}^{3}\) and at \(20^{\circ} \mathrm{C}\) is \(998 \mathrm{~kg} / \mathrm{m}^{3}\). If you have \(200.0 \mathrm{~mL}\) of water at \(20^{\circ} \mathrm{C},\) what volume \((\mathrm{mL})\) will the water occupy at \(80^{\circ} \mathrm{C} ?\) Which will contain more water molecules, \(1.0 \mathrm{~L}\) of water at \(80^{\circ} \mathrm{C}\) or \(1.0 \mathrm{~L}\) of water at \(20^{\circ} \mathrm{C} ?\)

A \(47.0-\mathrm{cm}^{3}\) sample of ocean water has a density of \(1025 \mathrm{~kg} / \mathrm{m}^{3}\). Assuming all of the solids stay in solution, what will be the density of this water sample in units of \(\mathrm{g} / \mathrm{cm}^{3}\) after \(4.1 \mathrm{~mL}\) of water has evaporated?

At \(20^{\circ} \mathrm{C}\) liquid gasoline gas has a density of \(0.75 \mathrm{~g} / \mathrm{cm}^{3} .\) If a 5.5-mL sample of gasoline is placed into a sealed \(3.00-\mathrm{L}\) container at \(50^{\circ} \mathrm{C}\) and allowed to completely evaporate, what will be the density of the gasoline vapor in the container?

An ice cube measures \(3.50 \mathrm{~cm}\) on each edge and weighs \(39.45 \mathrm{~g}\). a Calculate the density of ice. b Calculate the mass of \(400.4 \mathrm{~mL}\) of water in an ice cube.

The total length of all the DNA molecules contained in a human body is \(1 \times 10^{10}\) miles. The population of the United States is about 300 million. What is the total length of all the DNA of the U.S. population in lightyears? (A lightyear is the distance that light travels in a year and is \(9.46 \times 10^{15} \mathrm{~m} .\)

Prospectors are considering searching for gold on a plot of land that contains \(1.31 \mathrm{~g}\) of gold per bucket of soil. If the volume of the bucket is \(4.67 \mathrm{~L}\), how many grams of gold are there likely to be in \(2.38 \times 10^{3}\) cubic feet of soil?

A solution is prepared by dissolving table salt, sodium chloride, in water at room temperature. a Assuming there is no significant change in the volume of water during the preparation of the solution, how would the density of the solution compare to that of pure water? b If you were to boil the solution for several minutes and then allow it to cool to room temperature, how would the density of the solution compare to the density in part a? c If you took the solution prepared in part a and added more water, how would this affect the density of the solution?

Water and saline (salt) solution have in common that they are both homogeneous. How do these materials differ? Be specific and use chemical terms to describe the two systems.

When \(11.1 \mathrm{~g}\) of marble chips (calcium carbonate) is treated with \(54.3 \mathrm{~mL}\) of hydrochloric acid (density \(1.096 \mathrm{~g} / \mathrm{mL}\) ), the marble dissolves, giving a solution and releasing carbon dioxide gas. The solution weighs \(65.7 \mathrm{~g}\). How many liters of carbon dioxide gas are released? The density of the gas is \(1.798 \mathrm{~g} / \mathrm{L}\).

Zinc ore (zinc sulfide) is treated with sulfuric acid, leaving a solution with some undissolved bits of material and releasing hydrogen sulfide gas. If \(10.8 \mathrm{~g}\) of zinc ore is treated with \(50.0 \mathrm{~mL}\) of sulfuric acid (density \(1.153 \mathrm{~g} / \mathrm{mL}\) ), \(65.1 \mathrm{~g}\) of solution and undissolved material remains. In addition, hydrogen sulfide (density \(1.393 \mathrm{~g} / \mathrm{L}\) ) is evolved. What is the volume (in liters) of this gas?

A steel sphere has a radius of 1.58 in. If this steel has a density of \(7.88 \mathrm{~g} / \mathrm{cm}^{3},\) what is the mass of the sphere in grams?

A weather balloon filled with helium has a diameter of \(3.50 \mathrm{ft}\). What is the mass in grams of the helium in the balloon at \(21^{\circ} \mathrm{C}\) and normal pressure? The density of helium under these conditions is \(0.166 \mathrm{~g} / \mathrm{L}\).

The land area of Greenland is \(840,000 \mathrm{mi}^{2},\) with only \(132,000 \mathrm{mi}^{2}\) free of perpetual ice. The average thickness of this ice is \(5000 \mathrm{ft}\). Estimate the mass of the ice (assume two significant figures). The density of ice is \(0.917 \mathrm{~g} / \mathrm{cm}^{3} .\)

Antarctica, almost completely covered in ice, has an area of \(5,500,000 \mathrm{mi}^{2}\) with an average height of \(7500 \mathrm{ft}\). Without the ice, the height would be only \(1500 \mathrm{ft}\). Estimate the mass of this ice (two significant figures). The density of ice is \(0.917 \mathrm{~g} / \mathrm{cm}^{3}\).