Multiple Choice3 moles of an ideal gas fill a cubical box with a side length of 30cm. If the temperature of the gas is 20°C, what is the pressure inside the container?547views1rank
Multiple ChoiceHydrogen gas behaves very much like an ideal gas. If you have a sample of Hydrogen gas with a volume of 1000 cm3 at 30°C with a pressure of 1 × 105 Pa, calculate how many hydrogen atoms (particles) there are in the sample.1359views3rank
Multiple ChoiceA balloon contains 3900cm3 of a gas at a pressure of 101 kPa and a temperature of –9°C. If the balloon is warmed such that the temperature rises to 28°C, what volume will the gas occupy? Assume the pressure remains constant.522views1rank
Multiple ChoiceA sample of gas is heated in a closed container with a volume of 2.2L, from an initial temperature and pressure of 20°C and 1.0 atm to a final temperature of 238°C. What is the final pressure?308views
Multiple ChoiceAn ideal gas is in a sealed container. It has a temperature T when it has volume V at pressure P. What is the temperature of the gas when its volume is quadrupled, and the pressure is halved?501views
Multiple Choice0.00086 moles of an ideal gas undergoes the process shown in the figure. If the initial temperature was 340K and the final pressure is 5.0atm, what is the final temperature? 260views
Textbook QuestionA constant-volume gas thermometer registers an absolute pressure corresponding to 325 mm of mercury when in contact with water at the triple point. What pressure does it read when in contact with water at the normal boiling point?734views
Textbook QuestionThe pressure of a gas at the triple point of water is 1.35 atm. If its volume remains unchanged, what will its pressure be at the temperature at which CO2 solidifies?984views
Textbook QuestionA large cylindrical tank contains 0.750 m^3 of nitrogen gas at 27°C and 7.50 * 10^3 Pa (absolute pressure). The tank has a tight-fitting piston that allows the volume to be changed. What will be the pressure if the volume is decreased to 0.410 m^3 and the temperature is increased to 157°C?325views
Textbook QuestionYou have several identical balloons. You experimentally determine that a balloon will break if its volume exceeds 0.900 L. The pressure of the gas inside the balloon equals air pressure (1.00 atm). (a) If the air inside the balloon is at a constant 22.0°C and behaves as an ideal gas, what mass of air can you blow into one of the balloons before it bursts?491views
Textbook QuestionHelium gas with a volume of 3.20 L, under a pressure of 0.180 atm and at 41.0°C, is warmed until both pressure and volume are doubled. (b) How many grams of helium are there? The molar mass of helium is 4.00 g/mol.553views
Textbook QuestionA 20.0-L tank contains 4.86 * 10^-4 kg of helium at 18.0°C. The molar mass of helium is 4.00 g/mol. (b) What is the pressure in the tank, in pascals and in atmospheres?771views
Textbook QuestionA 20.0-L tank contains 4.86 * 10^-4 kg of helium at 18.0°C. The molar mass of helium is 4.00 g/mol. (a) How many moles of helium are in the tank?411views
Textbook QuestionMartian Climate. The atmosphere of Mars is mostly CO2 (molar mass 44.0 g/mol) under a pressure of 650 Pa, which we shall assume remains constant. In many places the temperature varies from 0.0°C in summer to -100°C in winter. Over the course of a Martian year, what are the ranges of (b) the density (in mol/m^3) of the atmosphere?887views1rank
Textbook QuestionMeteorology. The vapor pressure is the pressure of the vapor phase of a substance when it is in equilibrium with the solid or liquid phase of the substance. The relative humidity is the partial pressure of water vapor in the air divided by the vapor pressure of water at that same temperature, expressed as a percentage. The air is saturated when the humidity is 100%. (a) The vapor pressure of water at 20.0°C is 2.34 * 10^3 Pa. If the air temperature is 20.0°C and the relative humidity is 60%, what is the partial pressure of water vapor in the atmosphere (that is, the pressure due to water vapor alone)?1256views1rank
Textbook QuestionHow Close Together Are Gas Molecules? Consider an ideal gas at 27°C and 1.00 atm. To get some idea how close these molecules are to each other, on the average, imagine them to be uniformly spaced, with each molecule at the center of a small cube. (a) What is the length of an edge of each cube if adjacent cubes touch but do not overlap?505views
Textbook QuestionIn a gas at standard conditions, what is the length of the side of a cube that contains a number of molecules equal to the population of the earth (about 7 * 10^9 people)?379views
Textbook QuestionModern vacuum pumps make it easy to attain pressures of the order of 10^-13 atm in the laboratory. Consider a volume of air and treat the air as an ideal gas. (b) How many molecules would be present at the same temperature but at 1.00 atm instead?411views
Textbook QuestionModern vacuum pumps make it easy to attain pressures of the order of 10^-13 atm in the laboratory. Consider a volume of air and treat the air as an ideal gas. (a) At a pressure of 9.00 * 10^-14 atm and an ordinary temperature of 300.0 K, how many molecules are present in a volume of 1.00 cm^3?441views
Textbook QuestionA large organic molecule has a mass of 1.41 * 10^-21 kg. What is the molar mass of this compound?472views
Textbook QuestionHow many moles are in a 1.00-kg bottle of water? How many molecules? The molar mass of water is 18.0 g/mol651views
Textbook QuestionAt an altitude of 11,000 m (a typical cruising altitude for a jet airliner), the air temperature is -56.5°C and the air density is 0.364 kg/m^3 . What is the pressure of the atmosphere at that altitude? (Note: The temperature at this altitude is not the same as at the surface of the earth, so the calculation of Example 18.4 in Section 18.1 doesn't apply.)1482views
Textbook QuestionIf a certain amount of ideal gas occupies a volume V at STP on earth, what would be its volume (in terms of V) on Venus, where the temperature is 1003°C and the pressure is 92 atm?641views
Textbook QuestionPlanetary Atmospheres. (a) Calculate the density of the atmosphere at the surface of Mars (where the pressure is 650 Pa and the temperature is typically 253 K, with a CO2 atmosphere), Venus (with an average temperature of 730 K and pressure of 92 atm, with a CO2 atmosphere), and Saturn's moon Titan (where the pressure is 1.5 atm and the temperature is -178°C, with a N2 atmosphere).820views
Textbook QuestionA cylindrical tank has a tight-fitting piston that allows the volume of the tank to be changed. The tank originally contains 0.110 m^3 of air at a pressure of 0.355 atm. The piston is slowly pulled out until the volume of the gas is increased to 0.390 m^3. If the temperature remains constant, what is the final value of the pressure?1048views
Textbook QuestionHelium gas with a volume of 3.20 L, under a pressure of 0.180 atm and at 41.0°C, is warmed until both pressure and volume are doubled. (a) What is the final temperature?555views
Textbook QuestionThe solar corona is a very hot atmosphere surrounding the visible surface of the sun. X-ray emissions from the corona show that its temperature is about 2×10^6 K. The gas pressure in the corona is about 0.03 Pa. Estimate the number density of particles in the solar corona.656views
Textbook QuestionThe total lung capacity of a typical adult is 5.0 L. Approximately 20% of the air is oxygen. At sea level and at a body temperature of 37°C, how many oxygen molecules do the lungs contain at the end of a strong inhalation?1086views
Textbook QuestionThe semiconductor industry manufactures integrated circuits in large vacuum chambers where the pressure is 1.0×10^−10 mm of Hg. b. At T=20°C, how many molecules are in a cylindrical chamber 40 cm in diameter and 30 cm tall?305views
Textbook QuestionAn inflated bicycle inner tube is 2.2 cm in diameter and 200 cm in circumference. A small leak causes the gauge pressure to decrease from 110 psi to 80 psi on a day when the temperature is 20°C. What mass of air is lost? Assume the air is pure nitrogen.491views
Textbook QuestionIn Problems 67, 68, 69, and 70 you are given the equation(s) used to solve a problem. For each of these, you are to b. Draw a pV diagram. V₂=(400+273) K / (50+273) K×1×200 cm^3281views
Textbook QuestionThe semiconductor industry manufactures integrated circuits in large vacuum chambers where the pressure is 1.0×10^−10 mm of Hg. a. What fraction is this of atmospheric pressure?286views
Textbook QuestionIn Problems 67, 68, 69, and 70 you are given the equation(s) used to solve a problem. For each of these, you are to a. Write a realistic problem for which this is the correct equation(s). (T₂+273) K=200 kPa / 500 kPa ×1×(400+273) K256views
Textbook QuestionIn Problems 67, 68, 69, and 70 you are given the equation(s) used to solve a problem. For each of these, you are to a. Write a realistic problem for which this is the correct equation(s). p₂=300 cm^3/ 100 cm^3 ×1×2 atm266views
Textbook QuestionFive grams of nitrogen gas at an initial pressure of 3.0 atm and at 20°C undergo an isobaric expansion until the volume has tripled. b. What is the gas temperature after the expansion (in °C)? The gas pressure is then decreased at constant volume until the original temperature is reached.304views
Textbook QuestionFive grams of nitrogen gas at an initial pressure of 3.0 atm and at 20°C undergo an isobaric expansion until the volume has tripled. a. What is the gas volume after the expansion?300views
Textbook QuestionA container of gas at 2.0 atm pressure and 127°C is compressed at constant temperature until the volume is halved. It is then further compressed at constant pressure until the volume is halved again. b. Show this process on a pV diagram.567views
Textbook Question10 g of dry ice (solid CO₂) is placed in a 10,000 cm^3 container, then all the air is quickly pumped out and the container sealed. The container is warmed to 0°C, a temperature at which CO₂ is a gas. a. What is the gas pressure? Give your answer in atm. The gas then undergoes an isothermal compression until the pressure is 3.0 atm, immediately followed by an isobaric compression until the volume is 1000 cm^3.373views
Textbook QuestionA gas with an initial temperature of 900°C undergoes the process shown in FIGURE EX18.35. c. How many moles of gas are there? 591views
Textbook QuestionA gas with an initial temperature of 900°C undergoes the process shown in FIGURE EX18.35. a. What type of process is this? 301views
Textbook QuestionA diver 50 m deep in 10°C fresh water exhales a 1.0-cm-diameter bubble. What is the bubble's diameter just as it reaches the surface of the lake, where the water temperature is 20°C?476views
Textbook QuestionA sealed container holds 3.2 g of oxygen at 1 atm pressure and 20°C. The gas first undergoes an isobaric process that doubles the absolute temperature, then an isothermal process that halves the pressure. What is the final volume of the gas in L?810views
Textbook Question0.0050 mol of gas undergoes the process 1→2→3 shown in FIGURE EX18.37. What are and (c) volume V₃? 292views
Textbook Question0.0050 mol of gas undergoes the process 1→2→3 shown in FIGURE EX18.37. What are (b) pressure p₂, 317views
Textbook Question0.0050 mol of gas undergoes the process 1→2→3 shown in FIGURE EX18.37. What are (a) temperature T₁, 294views
Textbook Question0.10 mol of argon gas is admitted to an evacuated 50 cm^3 container at 20°C. The gas then undergoes an isochoric heating to a temperature of 300°C. b. Show the process on a pV diagram. Include a proper scale on both axes.346views
Textbook Question0.10 mol of argon gas is admitted to an evacuated 50 cm^3 container at 20°C. The gas then undergoes an isochoric heating to a temperature of 300°C. a. What is the final pressure of the gas?536views
Textbook QuestionA 24-cm-diameter vertical cylinder is sealed at the top by a frictionless 20 kg piston. The piston is 84 cm above the bottom when the gas temperature is 303°C. The air above the piston is at 1.00 atm pressure. b. What will the height of the piston be if the temperature is lowered to 15°C?519views
Textbook QuestionA gas with initial state variables p₁, V₁ , and T₁ expands isothermally until V₂=2V₁. What are and (b) p₂?278views
Textbook QuestionA gas with initial state variables p₁, V₁, and T₁ expands isothermally until V₂=2V₁. What are (a) T₂255views
Textbook QuestionA gas with initial state variables p₁, V₁, and T₁ is cooled in an isochoric process until p₂=1/3p₁. What are (a) V₂?338views
Textbook QuestionA 20-cm-diameter cylinder that is 40 cm long contains 50 g of oxygen gas at 20°C. d. What is the reading of a pressure gauge attached to the tank?507views
Textbook QuestionA 20-cm-diameter cylinder that is 40 cm long contains 50 g of oxygen gas at 20°C. c. What is the number density of the oxygen?335views1rank
Textbook QuestionA gas at 100°C fills volume V₀. If the pressure is held constant, what is the volume if (b) the Kelvin temperature is doubled?310views
Textbook QuestionA gas at 100°C fills volume V₀. If the pressure is held constant, what is the volume if (a) the Celsius temperature is doubled346views
Textbook QuestionA cylinder contains nitrogen gas. A piston compresses the gas to half its initial volume. Afterward, a. Has the mass density of the gas changed? If so, by what factor? If not, why not?318views
Textbook QuestionA 6.0-cm-diameter, 10-cm-long cylinder contains 100 mg of oxygen (O₂) at a pressure less than 1 atm. The cap on one end of the cylinder is held in place only by the pressure of the air. One day when the atmospheric pressure is 100 kPa, it takes a 184 N force to pull the cap off. What is the temperature of the gas?401views
Textbook QuestionThe interior of a Boeing 737-800 can be modeled as a 32-m-long, 3.7-m-diameter cylinder. The air inside, at cruising altitude, is 20°C at a pressure of 82 kPa. What volume of outside air, at −40°C and a pressure of 23 kPa, must be drawn in, heated, and compressed to fill the plane?413views
Textbook QuestionThe 50 kg circular piston shown in FIGURE P18.57 floats on 0.12 mol of compressed air. a. What is the piston height h if the temperature is 30°C?272views
Textbook QuestionThe 50 kg circular piston shown in FIGURE P18.57 floats on 0.12 mol of compressed air. b. How far does the piston move if the temperature is increased by 100°C?296views
Textbook QuestionThe cylinder in FIGURE CP18.73 has a moveable piston attached to a spring. The cylinder's cross-section area is 10 cm^2, it contains 0.0040 mol of gas, and the spring constant is 1500 N/m. At 20°C the spring is neither compressed nor stretched. How far is the spring compressed if the gas temperature is raised to 100°C?371views
Textbook QuestionThe closed cylinder of FIGURE CP18.74 has a tight-fitting but frictionless piston of mass M. The piston is in equilibrium when the left chamber has pressure p₀ and length L₀ while the spring on the right is compressed by ΔL. b. Suppose the piston is moved a small distance x to the right. Find an expression for the net force (Fₓ)net on the piston. Assume all motions are slow enough for the gas to remain at the same temperature as its surroundings.336views
Textbook QuestionOn average, each person in the industrialized world is responsible for the emission of 10,000 kg of carbon dioxide (CO₂) every year. This includes CO₂ that you generate directly, by burning fossil fuels to operate your car or your furnace, as well as CO₂ generated on your behalf by electric generating stations and manufacturing plants. CO₂ is a greenhouse gas that contributes to global warming. If you were to store your yearly CO₂ emissions in a cube at STP, how long would each edge of the cube be?258views
Textbook QuestionThe 3.0-m-long pipe in FIGURE P18.49 is closed at the top end. It is slowly pushed straight down into the water until the top end of the pipe is level with the water's surface. What is the length L of the trapped volume of air?300views
Textbook QuestionA diving bell is a 3.0-m-tall cylinder closed at the upper end but open at the lower end. The temperature of the air in the bell is 20°C. The bell is lowered into the ocean until its lower end is 100 m deep. The temperature at that depth is 10°C. a. How high does the water rise in the bell after enough time has passed for the air inside to reach thermal equilibrium?329views
Textbook QuestionAn electric generating plant boils water to produce high-pressure steam. The steam spins a turbine that is connected to the generator. a. How many liters of water must be boiled to fill a 5.0 m^3 boiler with 50 atm of steam at 400°C?265views
Textbook QuestionOn a cool morning, when the temperature is 15°C, you measure the pressure in your car tires to be 30 psi. After driving 20 mi on the freeway, the temperature of your tires is 45°C . What pressure will your tire gauge now show?383views
Textbook QuestionA 10-cm-diameter, 40-cm-tall gas cylinder, sealed at the top by a frictionless 50 kg piston, is surrounded by a bath of 20°C water. Then 50 kg of sand is slowly poured onto the top of the piston, where it stays. Afterward, what is the height of the piston?264views
Textbook QuestionA 6.0-cm-diameter cylinder of nitrogen gas has a 4.0-cm-thick movable copper piston. The cylinder is oriented vertically, as shown in FIGURE P19.49, and the air above the piston is evacuated. When the gas temperature is 20°C, the piston floats 20 cm above the bottom of the cylinder. a. What is the gas pressure?193views1rank
Textbook QuestionA 6.0-cm-diameter cylinder of nitrogen gas has a 4.0-cm-thick movable copper piston. The cylinder is oriented vertically, as shown in FIGURE P19.49, and the air above the piston is evacuated. When the gas temperature is 20°C, the piston floats 20 cm above the bottom of the cylinder. c. What is the new equilibrium temperature of the gas?219views
Textbook Question14 g of nitrogen gas at STP are pressurized in an isochoric process to a pressure of 20 atm. What are (a) the final temperature,264views
Textbook QuestionA 1.0 m ✕ 1.0 m ✕ 1.0 m cube of nitrogen gas is at 20℃ and 1.0 atm. Estimate the number of molecules in the cube with a speed between 700 m/s and 1000 m/s.280views
Textbook QuestionPhotons of light scatter off molecules, and the distance you can see through a gas is proportional to the mean free path of photons through the gas. Photons are not gas molecules, so the mean free path of a photon is not given by Equation 20.3, but its dependence on the number density of the gas and on the molecular radius is the same. Suppose you are in a smoggy city and can barely see buildings 500 m away. b. How far would you be able to see if the temperature suddenly rose from 20°C to a blazing hot 1500°C with the pressure unchanged?226views
Textbook QuestionInterstellar space, far from any stars, is filled with a very low density of hydrogen atoms (H, not H₂). The number density is about 1 atom/cm³ and the temperature is about 3 K. a. Estimate the pressure in interstellar space. Give your answer in Pa and in atm.258views
Textbook QuestionEquation 20.3 is the mean free path of a particle through a gas of identical particles of equal radius. An electron can be thought of as a point particle with zero radius. b. Electrons travel 3.0 km through the Stanford Linear Accelerator. In order for scattering losses to be negligible, the pressure inside the accelerator tube must be reduced to the point where the mean free path is at least 50 km. What is the maximum possible pressure inside the accelerator tube, assuming T = 20℃? Give your answer in both Pa and atm.258views
Textbook Question(II) What is the pressure inside a 41.0-L container holding 105.0 kg of argon gas at 21.6°C?113views
Textbook QuestionA standard cylinder of oxygen used in a hospital has gauge pressure = 2000 psi (13,800 kPa) and volume = 14L (0.014m³) at T = 295 K . How long will the cylinder last if the flow rate, measured at atmospheric pressure, is constant at 2.0 L/min?102views
Textbook QuestionIf a scuba diver fills his lungs to full capacity of 4.8 L when 9.0 m below the surface of sea water, to what volume would his lungs expand if he quickly rose to the surface? Is this advisable?97views
Textbook QuestionA scuba tank when fully charged has an absolute pressure of 185 atm at 18°C. The volume of the tank is 11.3 L.(a) What would the volume of the air be at 1.00 atm and at the same temperature?102views
Textbook Question(III) How well does the ideal gas law describe the pressurized air in a scuba tank?(a) To fill a typical scuba tank, an air compressor intakes about 2300 L of air at 1.0 atm and compresses this gas into the tank’s 12-L internal volume. If the filling process occurs at 20°C, show that a tank holds about 96 mol of air.204views
Textbook QuestionAssuming a typical nitrogen or oxygen molecule is about 0.3 nm in diameter, what percent of the room you are sitting in is taken up by the volume of the molecules themselves?113views
Textbook Question(I) What is the partial pressure of water on a day when the temperature is 25°C and the relative humidity is 75%?97views
Textbook QuestionUsing the ideal gas law, find an expression for the mean free path ℓ_M that involves pressure and temperature instead of (N/V). Use this expression to find the mean free path for nitrogen molecules at a pressure of 7.5 atm and 300 K.106views
Textbook QuestionA helium balloon has volume V₀ and temperature T₀ at sea level where the pressure is P₀ and the air density is ρ₀ . The balloon is allowed to float up in the air to altitude y where the temperature is T₁ .(b) Show that the buoyant force does not depend on altitude y. Assume that the skin of the balloon maintains the helium pressure at a constant factor of 1.05 times greater than the outside pressure. [Hint: Assume that the pressure change with altitude is P = P₀ e⁻ᶜʸ , Eq. 13–6c in Chapter 13.]96views
Textbook Question(III) Estimate how many air molecules rebound from a wall in a typical room per second, assuming an ideal gas of N molecules contained in a cubic room with sides of length ℓ at temperature T and pressure P.(a) Show that the frequency f with which gas molecules strike a wall is ƒ = (υ¯ₓ /2)(P/kT) ℓ² where υ¯ₓ is the average x component of the molecule’s velocity.(b) Show that the equation can then be written as ƒ≈ Pℓ² /√4mkT where m is the mass of a gas molecule.96views
Textbook QuestionAssume that in an alternate universe, the laws of physics are very different from ours and that “ideal” gases behave as follows:(i) At constant temperature, pressure is inversely proportional to the square of the volume.110views
Textbook QuestionAssume that in an alternate universe, the laws of physics are very different from ours and that “ideal” gases behave as follows:(ii) At constant pressure, the volume varies directly with the 2/3 power of the temperature.100views
Textbook QuestionAssume that in an alternate universe, the laws of physics are very different from ours and that “ideal” gases behave as follows:(iii) At 273.15 K and 1.00 atm pressure, 1.00 mole of an ideal gas is found to occupy 22.4 L. Obtain the form of the ideal gas law in this alternate universe, including the value of the gas constant R.104views
Textbook Question(a) From the van der Waals equation of state, show that the critical temperature and pressure are given byT꜀ᵣ = 8a / 27bR , P꜀ᵣ = a / 27b² .[Hint: Use the fact that the P versus V curve has an inflection point at the critical point so that the first and second derivatives are zero.]112views
Textbook Question(b) Show that the bulk modulus (Section 12–5) for an ideal gas held at constant temperature is B = P , where P is the pressure. <IMAGE>86views
Textbook QuestionA sauna has 7.8 m³ of air volume, and the temperature is 85°C. The air is perfectly dry. How much water (in kg) should be evaporated if we want to increase the relative humidity from 0% to 10%? (See Table 18–2.)<IMAGE>81views
Textbook QuestionWhy snorkels are not 4 feet long. Snorkelers breathe through short tubular “snorkels” while swimming under water very near the surface (Fig. 17–24). One end of the snorkel is in the snorkeler’s mouth and the other end protrudes just above the water’s surface. Unfortunately, snorkels cannot support breathing to any great depth: it is said that a typical snorkeler below a water depth of only about 30 cm cannot draw a breath through a snorkel. Based on this observation, what is the approximate change in a typical person’s lung pressure (in atm) when drawing a breath? (Note that your diaphragm muscles, which expand your lungs, must work also against the extra water pressure.)<IMAGE>81views
Textbook QuestionA heat engine takes a diatomic gas around the cycle shown in Fig. 20–23.(a) Using the ideal gas law, determine how many moles of gas are in this engine.<IMAGE>191views
Textbook QuestionA heat engine takes a diatomic gas around the cycle shown in Fig. 20–23.(b) Determine the temperature at point c.<IMAGE>114views
Textbook Question1.00 mole of an ideal monatomic gas at STP first undergoes an isothermal expansion so that the volume at b is 2.5 times the volume at a (Fig. 20–25). Next, heat is extracted at a constant volume so that the pressure drops. The gas is then compressed adiabatically back to the original state.(a) Calculate the pressures at b and c.<IMAGE>141views
Textbook Question1.00 mole of an ideal monatomic gas at STP first undergoes an isothermal expansion so that the volume at b is 2.5 times the volume at a (Fig. 20–25). Next, heat is extracted at a constant volume so that the pressure drops. The gas is then compressed adiabatically back to the original state.(b) Determine the temperature at c.<IMAGE>78views
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