QUESTION 2 A room is filled with an ideal gas at a temperature T= 407 K and pressure p = 2 atmospheres (abbreviated atm). The dime Use the ideal gas law pV = NkT to calculate the number of molecules in the room. The constant k is Boltzmann's constan item on Blackboard. Be careful to choose a value with the right set of units for this problem. %3D %3! Note that 1 atm = 1.013 x 10° Pa, where the SI unit for pressure is pascal (Pa), a N m (Newton, not number). Note that if you use SI units consistently, then your answer will be in terms of number of molecules, which is dimensionles Submit your numerical answer in exponential form as described in the worksheet instructions. %3! QUESTION 3 If the molecules in a gas are nitrogen (N2) molecules, calculate their root mean squared (RMS) speed, (v²), in m/s whi Hint: You will need to calculate the mass of the nitrogen molecule, which is its atomic mass number multiplied by the atom Write your answer in normal form as described in the instructions to the worksheet Click Save and Submit to save and submit. Click Save All Answers to save all answers. P Type here to search

QUESTION 2 A room is filled with an ideal gas at a temperature T= 407 K and pressure p = 2 atmospheres (abbreviated atm). The dime Use the ideal gas law pV = NkT to calculate the number of molecules in the room. The constant k is Boltzmann's constan item on Blackboard. Be careful to choose a value with the right set of units for this problem. %3D %3! Note that 1 atm = 1.013 x 10° Pa, where the SI unit for pressure is pascal (Pa), a N m (Newton, not number). Note that if you use SI units consistently, then your answer will be in terms of number of molecules, which is dimensionles Submit your numerical answer in exponential form as described in the worksheet instructions. %3! QUESTION 3 If the molecules in a gas are nitrogen (N2) molecules, calculate their root mean squared (RMS) speed, (v²), in m/s whi Hint: You will need to calculate the mass of the nitrogen molecule, which is its atomic mass number multiplied by the atom Write your answer in normal form as described in the instructions to the worksheet Click Save and Submit to save and submit. Click Save All Answers to save all answers. P Type here to search

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter10: Thermal Physics

Section: Chapter Questions

Problem 60AP: A 20.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.50 105 Pa and temperature of 19.0C...

See similar textbooks

Similar questions

Two small containers, each with a volume of 1.00 102cm3, contain helium gas at 0C and 1.00 atm pressure. The two containers are joined by a small open tube of negligible volume, allowing gas to flow from one container to the other. What common pressure will exist in the two containers if the temperature of one container is raised to 1.00 102 C while the other container is kept at 0C?
The pressure gauge on a cylinder of gas registers the gauge pressure, which is the difference between the interior pressure and the exterior pressure P0. Lets call the gauge pressure Pg. When the cylinder is full, the mass of the gas in it is mi at a gauge pressure of Pgi. Assuming the temperature of the cylinder remains constant, show that the mass of the gas remaining in the cylinder when the pressure reading is Pgf is given by mf=mi(Pgf+P0Pgi+P0)
The density or gasoline is 7.30 102 kg/m3 at 0C. Its average coefficient of volume expansion is 9.60 104(C)1 and note that 1.00 gal = 0.003 80 m3. (a) Calculate the mass of 10.0 gal of gas at 0C. (b) If 1.000 m3 of gasoline at 0C is warmed by 20.0C, calculate its new volume. (c) Using the answer to part (b), calculate the density of gasoline at 20.0C. (d) Calculate the mass of 10.0 gal of gas at 20.0C. (e) How many extra kilograms of gasoline would you get if you bought 10.0 gal of gasoline at 0C rather than at 20.0C from a pump that is not temperature compensated?
The density or gasoline is 7.30 102 kg/m3 at 0C. Its average coefficient of volume expansion is 9.60 104(C)1 and note that 1.00 gal = 0.003 80 m3. (a) Calculate the mass of 10.0 gal of gas at 0C. (b) If 1.000 m3 of gasoline at 0C is warmed by 20.0C, calculate its new volume. (c) Using the answer to part (b), calculate the density of gasoline at 20.0C. (d) Calculate the mass of 10.0 gal of gas at 20.0C. (e) How many extra kilograms of gasoline would you get if you bought 10.0 gal of gasoline at 0C rather than at 20.0C from a pump that is not temperature compensated?
How does the kinetic theory describe a gas?
A 20.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.50 105 Pa and temperature of 19.0C (a) Calculate the temperature of the gas in Kelvin. (b) Use the ideal gas law to calculate the number of moles of gas in the tank. (c) Use the periodic table to compute the molecular weight of carbon dioxide, expressing it in grams per mole. (d) Obtain the number of grains of carbon dioxide in the tank. (e) A fire breaks out, raising the ambient temperature by 224.0 K while 82.0 g of gas leak out of the tank. Calculate the new temperature and the number of moles of gas remaining in the tank. (f) Using a technique analogous to that in Example 10.6b, find a symbolic expression for the final pressure, neglecting the change in volume of the tank. (g) Calculate the final pressure in the tank as a result of the fire and leakage.
em>. The volume of an ideal gas enclosed in a thin, elastic membrane in a room at sea level where the air temperature is 18°C is 8 10-3 m3 .If the temperature of the room is increased by 10°C, what is the new volume of the gas?
An ideal gas has a pressure of 2.5 atm, a volume of 1 x 10-3 m3 at a temperature of 30ºC. How many molecules are there in the gas? Boltzmann’s constant = 1.38 x 10-23 J/K. (1atm = 1.013x105 N/m2)
1) Determine the number of air particles in an empty 12 fl oz bottle (about 3.5*10^-4 m^3) at a pressure of 1.01*10^5 Pa and a temperature of 25 oC. 8.6*10^6 8.6*10^11 8.6*10^18 8.6*10^21 2)Determine the average speed of an air particle at 15 oC. The mass of one air particle is about 4.81*10^-26 kg. 489 m/s 45 m/s 5044 m/s 16 m/s
Why is Charles’ Law valid only when the temperature is expressed on absolute scale?
There are lots of examples of ideal gases in the universe, and they exist in many different conditions. In this problem we will examine what the temperature of these various phenomena are. a. Give an expression for the temperature of an ideal gas in terms of pressure P, particle density per unit volume ρ, and fundamental constants. b. Near the surface of Venus, its atmosphere has a pressure fv= 95 times the pressure of Earth's atmosphere, and a particle density of around ρv = 1.1 × 1027 m-3. What is the temperature of Venus' atmosphere (in C) near the surface? c. The Orion nebula is one of the brightest diffuse nebulae in the sky (look for it in the winter, just below the three bright stars in Orion's belt). It is a very complicated mess of gas, dust, young star systems, and brown dwarfs, but let's estimate its temperature if we assume it is a uniform ideal gas. Assume it is a sphere of radius r = 4.7 × 1015 m (around 6 light years) with a total mass 4000 times the mass of the…
The temperature of an ideal gas is directly proportional to the average kinetic energy of its molecules. If a container of ideal gas is moving past you at 2000 m/s, is the temperature of the gas higher than if the container was at rest? Explain your reasoning.