Long-term space missions require reclamation of the oxygen in the carbon dioxide exhaled by the crew. In one method of reclamation, 1.00 mol of carbon dioxide produces 1.00 mol of oxygen, with 1.00 mal of methane as a by-product. The methane is stored in a tank under pressure and is available to control the attitude of the spacecraft by controlled venting. A single astronaut exhales 1,08 kg of carbon dioxide each day. If the methane generated in the recycling of three astronauts' respiration during one week of flight is stored in an originally empty 165-L tank at -45.0°C, what is the final pressure in the tank? MPa Need Help? Red

Long-term space missions require reclamation of the oxygen in the carbon dioxide exhaled by the crew. In one method of reclamation, 1.00 mol of carbon dioxide produces 1.00 mol of oxygen, with 1.00 mal of methane as a by-product. The methane is stored in a tank under pressure and is available to control the attitude of the spacecraft by controlled venting. A single astronaut exhales 1,08 kg of carbon dioxide each day. If the methane generated in the recycling of three astronauts' respiration during one week of flight is stored in an originally empty 165-L tank at -45.0°C, what is the final pressure in the tank? MPa Need Help? Red

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

1.0 kg of an ideal gas at normal atmospheric pressure was heated in a 1 m3 container until the temperature was doubled while maintaining the pressure. What is the final volume?
The gas law for an ideal gas at absolute temperature T (in kelvins), pressure P (in atmospheres), and volume V (in liters) is PV = nRT, where n is the number of moles of the gas and R = 0.0821 is the gas constant. Suppose that, at a certain instant, P = 9.0 atm and is increasing at a rate of 0.15 atm/min and V = 13 L and is decreasing at a rate of 0.17 L/min. Find the rate of change of T with respect to time at that instant if n = 10 mol. (Round your answer to four decimal places.) dT=0.512 dt X K/min
The air quality index in Beijing last year recorded average ozone (O3) levels of 110 ppb (on a mol basis). Does this exceed Canada's acceptable 24 hour National Ambient Air Quality Objective (NAAQO) of 50 micrograms/M3? Assume the average molar mass of air is 29.0 g/mol and its density is 1.225 kg/M3.
The pressure of a gas in well sealed vertical frictionless piston-cylinder is to be increased by increasing the mass of the piston by 25 kg. If the area of the cylinder is 0.015 m2 , the increase in pressure of the gas is: OPTIONS: 15.5 KPa 16.35 KPa 1.06 KPa 10 KPa
What is the density of water vapor in the air on a hot, dry day in the desert when the temperature is 40.0 °C and the relative humidity is 5.00 %? The vapor pressure of water at 40.0 °C is Py = 7.34 x 10° Pa and the molecular mass of water is M = 18.0 g/mol. Enter your answer in units of grams per cubic meter. density: g/m3
Consider two containers with the same volume and temperature. The first container is labelled "Dry" and holds "dry" air = a ratio of nitrogen (N2) and oxygen (O2). The second container is labelled "Humid" and holds "moist" air = the SAME ratio of nitrogen and oxygen, but also contains water (H2O) vapor. According to the ideal gas law, if the pressures are equal, the weight of the gas inside the "Dry" container will be
The data shown below were obtained by time-lapse photography on a highway. Use regression analysis to fit these data to the Greenshields model and determine the following. Speed (mi/h) Density (veh/mi) 18.4 26.7 33.4 41.1 53.8 56.0 (a) the mean free speed (in mi/h) mi/h 80 65 50 36 15 10 (b) the jam density (in veh/mi) X The response you submitted has the wrong sign. veh/mi (c) the capacity (in veh/h) veh/h (d) the speed at maximum flow (in mi/h) mi/h
A young male adult takes in about 5.87 x 10-4 m3 of fresh air during a normal breath. Fresh air contains approximately 21% oxygen. Assuming that the pressure in the lungs is 1.09 x 105 Pa and air is an ideal gas at a temperature of 310 K, find the number of oxygen molecules in a normal breath.
A 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: 1829.73
Long-term space missions require reclamation of the oxygen in the carbon dioxide exhaled by the crew. In one method of reclamation, 1.00 mol of carbon dioxide produces 1.00 mol of oxygen, with 1.00 mol of methane as a by-product. The methane is stored in a tank under pressure and is available to control the attitude of the spacecraft by controlled venting. A single astronaut exhales 1.13 kg of carbon dioxide each day. If the methane generated in the recycling of three astronauts' respiration during one week of flight is stored in an originally empty 120-L tank at -45.0°C, what is the final pressure in the tank? MPa Need Help? Read It
Problem 5: n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.094 m3. Part (a) The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas? 50% Part (b) The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas?
The gas law for an ideal gas at absolute temperature T (in kelvins), pressure P (in atmospheres), and volume V (in liters) is PV = nRT, where n is the number of moles of the gas and R = 0.0821 is the gas constant. Suppose that, at a certain instant, P = 7.0 atm and is increasing at a rate of 0.15 atm/min and V = 13 and is decreasing at a rate of 0.17 L/min. Find the rate of change of T with respect to time (in K/min) at that instant if n = 10 mol.(Round your answer to four decimal places.)