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STP. The conditions of standard temperature and pressure (STP) are a temperature of 0.00°C and a pressure of 1.00 atm. (a) How many liters does 1.00 mol of any ideal gas occupy at STP? (b) For a scientist on Venus, an absolute pressure of 1 Venusian-atmosphere is 92 earth-atmospheres. Of course she would use the Venusian-atmosphere to define STP. Assuming she kept the same temperature, how many liters would 1 mole of ideal gas occupy on Venus?
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College Physics Plus Mastering Physics with eText - Access Card Package (10th Edition)
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- In the text, it was shown that N/V=2.681025m3 for gas at STP. (a) Show that this quantity is equivalent to N/V=2.681019cm3, as stated. (b) About how many atoms are mere in one m3 (a cubic micrometer) at STP? (c) What does your answer to part (b) imply about the separation of Mama and molecules?arrow_forwardOne process for decaffeinating coffee uses carbon dioxide ( M=44.0 g/mol) at a molar density of about 14,0 mol/m3 and a temperature of about 60 . (a) Is CO2 a solid, liquid, gas, or supercritical fluid under those conditions? (b) The van der Waals constants for carbon dioxide are a=0.3658 Pa m6/mol2 and b=4.286105 m3/mol. Using the van der Waals equation, estimate pressure of CO2 at that temperature and density. `arrow_forward(a) An ideal gas occupies a volume of 1.0 cm3 at 20.C and atmospheric pressure. Determine the number of molecules of gas in the container, (b) If the pressure of the 1.0-cm3 volume is reduced to 1.0 1011 Pa (an extremely good vacuum) while the temperature remains constant, how many moles of gas remain in the container?arrow_forward
- On a hot summer day, the density of air at atmospheric pressure at 35.0C is 1.1455 kg/m3. a. What is the number of moles contained in 1.00 m3 of an ideal gas at this temperature and pressure? b. Avogadros number of air molecules has a mass of 2.85 102 kg. What is the mass of 1.00 m3 of air? c. Does the value calculated in part (b) agree with the stated density of air at this temperature?arrow_forwardTwo containers hold ideal gases at the same temperature.Container A has twice the volume and half the number of molecules as container B. What is the ratio PA>PB, where PA is the pressure in container A and PB is the pressure in container B?arrow_forwardWhat is the volume of 67 mol of gas, in the unit of m3, when the pressure is 87 kPa and the temperature is 68°C? Use R = 8.314 J/(K mol) for the gas constant. Be careful with units, and remember that the temperature must be in Kelvin when you use the ideal gas equation.arrow_forward
- Two containers of equal volume each hold samples of the same ideal gas. Container A has 2 times as many molecules as container B. If the gas pressure is the same in the two containers, find the ratio of the the absolute temperatures TA and TB ( i.e TA / TB ) . Calculate to 2 decimals.arrow_forwardIdeal gases are often studied at standard ambient temperature and pressure (SATP). The International Union of Pure and Applied Chemistry (IUPAC) defines SATP to be T = 25° C and P = 100 kPa. a. Calculate N/V (in particles per cubic meter) for an ideal gas at SATP b. How many atoms of an ideal gas at SATP are there in one cubic centimeter?arrow_forwardA container holds 2.5 moles of an ideal gas at a pressure of 3.5 atmospheres and a temperature of 300 Kelvin. If the volume of the container is 10 liters, what is the value of the gas constant (R) in J/(mol·K)?arrow_forward
- When air expands adiabatically (without gaining or losing heat), its pressure P and volume V are related by the equation PV4 =C where C is a constant. Suppose that at a certain instant the volume is 600 cubic centimeters and the pressure is 79 kPa and is decreasing at a rate of 14 kPa/minute. At what rate in cubic centimeters per minute is the volume increasing at this instant? cm min (Pa stands for Pascal -- it is equivalent to one Newton/(meter squared); kPa is a kiloPascal or 1000 Pascals.arrow_forwardA sample of an ideal gas is compressed and cooled as it is taken from state 1 to state 2. The given properties for the gas in the two states are: p1 = 94.0 kPa, V1 = 0.0500 m3, V2 = 0.0400 m3, T1 = 300. K, T2 = 260. K.Calculate the pressure of the gas in state 2. Note: You must enter units with your answer.arrow_forwardA gas with a volume of 640 mL at a pressure of 2.91 atm is allowed to expand to a volume of 3.58 L. What is the pressure in the container if the temperature remains constant? Be sure to enter a unit with your answer. Answer: .052atm If the pressure of a sample of gas is tripled under constant temperature, what will happen to the volume? Select one: a. The volume will decrease by one-third. b. The volume will triple. c. The volume will be reduced by one-half. d. The volume will double. e. The volume will remain the same. Clear my choice If 173 mL of neon at 39.9 °C is allowed to expand to 422 mL, what must the new temperature be to maintain constant pressure? Express your answer in °C. You do not need to enter units. Answer: 1829.73arrow_forward
- College PhysicsPhysicsISBN:9781285737027Author:Raymond A. Serway, Chris VuillePublisher:Cengage LearningPhysics for Scientists and Engineers: Foundations...PhysicsISBN:9781133939146Author:Katz, Debora M.Publisher:Cengage LearningCollege PhysicsPhysicsISBN:9781938168000Author:Paul Peter Urone, Roger HinrichsPublisher:OpenStax College
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