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chemistry
physical chemistry

Questions and Answers of Physical Chemistry

Chlorine dioxide gas (ClO2) is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced. (a) What is the Lewis
Natural gas is very abundant in many Middle Eastern oil fields. However, the costs of shipping the gas to markets in other parts of the world are high because it is necessary to liquefy the gas,
Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2 (s) + 5F2 (g) → 2IF5 (g) A 5.00-L flask containing 10.0 g I2 is charged with 10.0 g F2,
How does a gas compare with a liquid for each of the following properties? (a) Density, (b) Compressibility, (c) Ability to mix with other substances of the same phase to form homogeneous
A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas 28oC at and 743 torr
(a) A liquid and a gas are moved to larger containers. How does their behavior differ once they are in the larger containers? Explain the difference in molecular terms. (b) Although liquid water and
Suppose that a woman weighing 130 lb and wearing high-heeled shoes momentarily places all her weight on the heel of one foot. If the area of the heel is 0.50 in2 calculate the pressure exerted on the
A set of bookshelves rests on a hard floor surface on four legs, each having a cross-sectional dimension of 3.0 x 4.1 cm in contact with the floor. The total mass of the shelves plus the books
(a) How high in meters must a column of water be to exert a pressure equal to that of a 760-mm column of mercury? The density of water is 1.0 g/ml, whereas that of mercury is 13.6 g / mL. (b) What is
The compound 1-iodododecane is a nonvolatile liquid with a density of 1.20 g/mL. The density of mercury is 13.6 g/mL. What do you predict for the height of a barometer column based on 1-iodododecane,
Each of the following statements concerns a mercury barometer such as that shown in Figure 10.2. Identify any incorrect statements and correct them.(a) The tube must be 1cm2 in cross-sectional
You have a sample of gas in a container with a movable piston, such as the one in the drawing.(a) Redraw the container to show what it might look like if the temperature of the gas is increased from
Suppose you make a mercury barometer using a glass tube about 50 cm in length, closed at one end. What would you expect to see if the tube is filled with mercury and inverted in a mercury dish, as in
Perform the following conversions: (a) 0.912 atm to torr, (b) 0.685 bar to kilopascals, (c) 655 mm Hg to atmospheres, (d) 1.323 x 105 Pa to atmospheres, (e) 2.50 atm to psi.
Perform the following conversions: (a) 0.912 atm to torr, (b) 0.685 bar to kilopascals, (c) 655 mm Hg to atmospheres, (d) 1.323 x 105 to atmospheres, (e) 2.50 atm to psi.
In the United States, barometric pressures are generally reported in inches of mercury (in. Hg) on a beautiful summer day in Chicago the barometric pressure is 30.45 in. Hg. (a) Convert this
Hurricane Wilma of 2005 is the most intense hurricane on record in the Atlantic basin, with a low-pressure reading of 882 mbar (milli bars). Convert this reading into (a) Atmospheres, (b) Torr,
If the atmospheric pressure is 0.995 atm, what is the pressure of the enclosed gas in each of the three cases depicted in the drawing? Assume that the gray liquid is mercury.
An open-end manometer containing mercury is connected to a container of gas, as depicted in Sample Exercise 10.2. What is the pressure of the enclosed gas in torr in each of the following situations?
You have a gas confined to a cylinder with a movable piston. What would happen to the gas pressure inside the cylinder if you do the following? (a) Decrease the volume to one-fourth the original
A fixed quantity of gas at 21oC exhibits a pressure of 752 torr and occupies a volume of 5.12 L. (a) Calculate the volume the gas will occupy if the pressure is increased to 1.88 atm while the
(a) How is the law of combining volumes explained by Avogadro's hypothesis? (b) Consider a 1.0-L flask containing neon gas and a 1.5-L flask containing xenon gas. Both gases are at the same pressure
Consider the sample of gas depicted here. What would the drawing look like if the volume and temperature remained constant while you removed enough of the gas to decrease the pressure by a factor of
Nitrogen and hydrogen gases react to form ammonia gas as follows: N2 (g) + 3 H2 → 2NH3 (g) At a certain temperature and pressure, 1.2 L of N2 reacts with 3.6 L of H2. If all the N2 and H2 are
(a) What is an ideal gas? (b) Show how Boyle's law, Charles's law, and Avogadro's law can be combined to give the ideal-gas equation. (c) Write the ideal-gas equation, and give the units used for
(a) What conditions are represented by the abbreviation STP? (b) What is the molar volume of an ideal gas at STP? (c) Room temperature is often assumed to be 25oC Calculate the molar volume of an
Suppose you are given two 1-L flasks and told that one contains a gas of molar mass 30, the other a gas of molar mass 60, both at the same temperature. The pressure in flask A is X atm, and the mass
Suppose you are given two flasks at the same temperature, one of volume 2 L and the other of volume 3 L. The 2-L flask contains 4.8 g of gas, and the gas pressure is X atm. The 3-L flask contains
Complete the following table for an ideal gas:
Calculate each of the following quantities for an ideal gas: (a) The volume of the gas, in liters, if 1.50mol has a pressure of 1.25 atm at a temperature of -6 °C; (b) The absolute tempera ture of
The Goodyear blimps, which frequently fly over sporting events, hold approximately 175000ft3 of helium. If the gas is at 23oC and 1.0 atm, what mass of helium is in a blimp?
A neon sign is made of glass tubing who's inside diameter is 2.5 cm and whose length is 5.5 m. If the sign contains neon at a pressure of 1.78 torr at 35oC, how many grams of neon are in the sign?
(a) Calculate the number of molecules in a deep breath of air whose volume is 2.25 L at body temperature, 37oC, and a pressure of 735 torr. (b) The adult blue whale has a lung capacity of 5.0 x 103
Imagine that the reaction 2CO (g) + O2 (g) → 2CO2 (g) Occurs in a container that has a piston that moves to maintain a constant pressure when the reaction occurs at constant temperature (a) What
(a) If the pressure exerted by ozone, O3, in the stratosphere is 3.0 x 10-3 and the temperature is 250 K, how many ozone molecules are in a liter? (b) Carbon dioxide makes up approximately 0.04% of
A scuba divers tank contains 0.29 kg of O2 compressed into a volume of 2.3 L. (a) Calculate the gas pressure inside the tank at 9oC. (b) What volume would this oxygen occupy at and 0.95 atm?
An aerosol spray can with a volume of 250 mL contain 2.30 g of propane gas (C3H8) as a propellant. (a) If the can is at 23oC, what is the pressure in the can? (b) What volume would the propane
Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 895 torr and 24oC. (a) How many
Many gases are shipped in high-pressure containers. Consider a steel tank whose volume is 55.0 gallons that contains O2 gas at a pressure of 16,500 kPa at 23oC. (a) What mass of O2 does the tank
In an experiment reported in the scientific literature, male cockroaches were made to run at different speeds on a miniature treadmill while their oxygen consumption was measured. In one hour the
The physical fitness of athletes is measured by "VO2 max," which is the maximum volume of oxygen consumed by an individual during incremental exercise (for example, on a treadmill). An average male
Mercury is a liquid at room temperature and pressure, but its vapor is present in the atmosphere from natural sources, such as volcanoes, and from human ("anthropogenic") activities such as coal
After the large eruption of Mount St. Helens in 1980, gas samples from the volcano were taken by sampling the downwind gas plume. The unfiltered gas samples were passed over a gold coated wire coil
Which gas is most dense at 1.00 atm and 298 K: CO2, N2O, or Cl2? Explain.
Suppose you have a fixed amount of an ideal gas at a constant volume. If the pressure of the gas is doubled while the volume is held constant, what happens to its temperature?
Rank the following gases from least dense to most dense at atm and 298 K: SO2, HBr, CO2 Explain.
Which of the following statements best explains why a closed balloon filled with helium gas rises in air? (a) Helium is a monatomic gas, whereas nearly all the molecules that make up air, such as
(a) Calculate the density of NO2 gas at 0.970 atm and 35oC. (b) Calculate the molar mass of a gas if 2.50 g occupies 0.875 L at 685 torr and 35oC.
(a) Calculate the density of sulfur hexafluoride gas at 707 torr and 21oC. (b) Calculate the molar mass of a vapor that has a density of 7.135 g/L at 12oC and 743 torr.
In the Dumas-bulb technique for determining the molar mass of an unknown liquid, you vaporize the sample of a liquid that boils below 100oC in a boiling-water bath and determine the mass of vapor
Magnesium can be used as a "getter" in evacuated enclosures to react with the last traces of oxygen. (The magnesium is usually heated by passing an electric current through a wire or ribbon of the
Calcium hydride, CaH2, reacts with water to form hydrogen gas: CaH2 (s) + 2 H2O (l) → Ca (OH)2 (aq) + 2H2 (g) This reaction is sometimes used to inflate life rafts, weather balloons, and the like,
The metabolic oxidation of glucose, C6H12O6, in our bodies produces CO2, which is expelled from our lungs as a gas: C6H12O6 (aq) + 6O2 (g) → 6CO2 (g) + 6H2O (l) (a) Calculate the volume of dry CO2
The apparatus shown here has two gas-filled containers and one empty container, all attached to a hollow horizontal tube. When the valves are opened and the gases are allowed to mix at constant
Both Jacques Charles and Joseph Louis Guy-Lussac were avid balloonists. In his original flight in 1783, Jacques Charles used a balloon that contained approximately 31,150 L of H2. He generated the H2
Hydrogen gas is produced when zinc reacts with sulfuric acid: Zn(s) + H2SO4 (aq) → ZnSO4 (aq) + H2(g) If 159 mL of wet H2 is collected over water at 24oC and a barometric pressure of 738 torr, how
Acetylene gas, C2H2 (g), can be prepared by the reaction of calcium carbide with water: CaC2 (s) + 2 H2O (l) → Ca (OH)2 (s) + C2H2 (g) Calculate the volume of C2H2 that is collected over water at
Consider the apparatus shown in the following drawing.(a) When the valve between the two containers is opened and the gases allowed mixing, how does the volume occupied by the N2 gas change? What is
Consider a mixture of two gases, A and B, confined in a closed vessel. A quantity of a third gas, C, is added to the same vessel at the same temperature. How does the addition of gas C affect the
A mixture containing 0.765 mol He (g), 0.330 mol Ne (g) and 0.110 mol Ar (g) is confined in a 10.00-L vessel at 25oC. (a) Calculate the partial pressure of each of the gases in the mixture. (b)
A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51.2 g of O2 and 32.6 g of He. Calculate the partial pressure of each gas and the total pressure if the temperature of
The atmospheric concentration of CO2 gas is presently 390 ppm (parts per million, by volume; that is, 390 L of every 106 L of the atmosphere are CO2).What is the mole fraction of CO2 in the
A plasma-screen TV contains thousands of tiny cells filled with a mixture of Xe, Ne, and He gases that emits light of specific wavelengths when a voltage is applied. A particular plasma cell, 0.900
A piece of dry ice (solid carbon dioxide) with a mass of 5.50 g is placed in a 10.0-L vessel that already contains air at 705 torr and 24oC. After the carbon dioxide has totally vaporized, what is
The accompanying drawing represents a mixture of three different gases.(a) Rank the three components in order of increasing partial pressure.(b) If the total pressure of the mixture is 1.40 atm,
A sample of 5.00 mL of diethylether (C2H5OC2H5, density = 0.7134 g / mL) is introduced into a 6.00-L vessel that already contains a mixture of N2 and O2, whose partial pressures are PN2 = 0.751 atm
A mixture of gases contains 0.75 mol N2, 0.30 mol O2, and 0.15 mol CO2. If the total pressure of the mixture is 2.15 atm, what is the partial pressure of each component?
A mixture of gases contains 10.25 g of N2, 1.83 g of H2, and 7.95 g of NH3. If the total pressure of the mixture is 1.85 atm, what is the partial pressure of each component?
At an underwater depth of 250 ft, the pressure is 8.38 atm. What should the mole percent of oxygen be in the diving gas for the partial pressure of oxygen in the mixture to be 0.21 atm, the same as
(a) What are the mole fractions of each component in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2? (b) What is the partial pressure in atm of each component of this mixture if it is
A quantity of N2 gas originally held at 5.25 atm pressure in a 1.00-L container at 26oC is transferred to a 12.5-L container at 20oC .A quantity of O2 gas originally at 5.25 atm and 26oC in a 5.00-L
A sample of 3.00 g of SO2 (g) originally in a 5.00-L vessel at 21oC is transferred to a 10.0-L vessel at 26oC. A sample of 2.35 g N2 (g) originally in a 2.50-L vessel at 20oC is transferred to this
Indicate which of the following statements regarding the kinetic molecular theory of gases are correct. For those that are false, formulate a correct version of the statement. (a) The average
On a single plot, qualitatively sketch the distribution of molecular speeds for (a) Kr (g) at - 50oC, (b) Kr (g) at - 0oC, (c) Ar (g) at - 0oC
Newton had an incorrect theory of gases in which he assumed that all gas molecules repel one another and the walls of their container. Thus, the molecules of a gas are statically and uniformly
Explain the difference between average speed and root-mean-square speed. Which is larger for a given gas sample at a fixed temperature?
You have an evacuated container of fixed volume and known mass and introduce a known mass of a gas sample. Measuring the pressure at constant temperature over time, you are surprised to see it slowly
The temperature of a 5.00-L container of N2 gas is increased from 20oC to 250oC. If the volume is held constant, predict qualitatively how this change affects the following: (a) The average kinetic
Suppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (a) Number of molecules, (b) Density, (c) Average kinetic
(a) Place the following gases in order of increasing average molecular speed at 25oC: Ne, HBr, SO2, NF3, CO. (b) Calculate the rms speed of NF3 molecules at 25oC. (c) Calculate the most probable
(a) Place the following gases in order of increasing average molecular speed at 300 K: CO, SF6, H2S, Cl2, HBr. (b) Calculate and compare the rms speeds of CO and Cl2 molecules at 300 K. (c)
Explain the difference between effusion and diffusion.
At constant pressure, the mean free path (λ) of a gas molecule is directly proportional to temperature. At constant temperature, λ is inversely proportional to pressure. If you compare two
Hydrogen has two naturally occurring isotopes, 1H and 2H. Chlorine also has two naturally occurring isotopes, 35Cl and 37Cl. Thus, hydrogen chloride gas consists of four distinct types of molecules:
Consider the following graph.(a) If curves A and B refer to two different gases, He and O2, at the same temperature, which is which? Explain.(b) If A and B refer to the same gas at two different
As discussed in the "Chemistry Put to Work" box in Section 10.8, enriched uranium can be produced by gaseous diffusion of UF6. Suppose a process were developed to allow diffusion of gaseous uranium
Arsenic (III) sulfide sublimes readily, even below its melting point of 320oC. The molecules of the vapor phase are found to effuse through a tiny hole at 0.28 times the rate of effusion of Ar atoms
A gas of unknown molecular mass was allowed to effuse through a small opening under constant-pressure conditions. It required 105 s for 1.0 L of the gas to effuse. Under identical experimental
(a) List two experimental conditions under which gases deviate from ideal behavior. (b) List two reasons why the gases deviate from ideal behavior. (c) Explain how the function PV/RT can be used to
The planet Jupiter has a surface temperature of 140 K and a mass 318 times that of Earth. Mercury (the planet) has a surface temperature between 600 K and 700 K and a mass 0.05 times that of Earth.
Based on their respective van der Waals constants (Table 10.3), is Ar or CO2 expected to behave more nearly like an ideal gas at high pressures? Explain.
In Sample Exercise 10.16, we found that one mole of Cl2 confined to 22.41 L at 0oC deviated slightly from ideal behavior. Calculate the pressure exerted by 1.00 mol Cl2 confined to a smaller volume,
Calculate the pressure that CCl4 will exert at 40oC if 1.00 mol occupies 33.3 L, assuming that(a) CCl4 obeys the ideal-gas equation;(b) CCl4 obeys the van der Waals equation. (Values for the van der
Table 10.3 shows that the van der Waals b parameter has units of L>mol. This implies that we can calculate the size of atoms or molecules from b. Using the value of b for Xe, calculate the radius of
Does the diagramBest describe a crystalline solid, a liquid, or a gas? Explain.
(a) How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in solids, liquids, and gases? (b)Why does increasing the temperature cause a
Arrange substances CCl4, Si, and Ar in order of increasing boiling point?
Arrange substances Ga, Ne, and Br2 in order of increasing boiling point?
At standard temperature and pressure the molar volume of Cl2 and NH3 gases are 22.06 L and 22.40 L, respectively. (a) Given the different molecular weights, dipole moments, and molecular shapes, why
Benzoic acid, C6H5COOH, melts at 122 oC. The density in the liquid state at is 130 oC is 1.08 g/cm3. The density of solid benzoic acid at 15 oC is 1.266 g/cm3. (a) In which of these two states is the

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