a. The space station uses prepackaged 25.0 kg cartridges of lithium oxide. How much water does each cartridge remove? If the environmental control unit on the space station reports that 29.5 kg of water should be removed from the air, how many lithium oxide cartridges need to be used? b. Lithium hydroxide, the same compound that is produced when water is removed from the air, can remove the excess carbon dioxide exhaled by the astronauts: LiOH(s) + CO2 (g) ? LiHCO3(s) Each lithium hydroxide cartridge that is used to remove carbon dioxide from the air has a lithium hydroxide mass of 32.0 kg. If the process for removing the carbon dioxide has a percentage yield of 88 percent, what mass of carbon dioxide is removed by each canister of lithium hydroxide?

a. The space station uses prepackaged 25.0 kg cartridges of lithium oxide. How much water does each cartridge remove? If the environmental control unit on the space station reports that 29.5 kg of water should be removed from the air, how many lithium oxide cartridges need to be used? b. Lithium hydroxide, the same compound that is produced when water is removed from the air, can remove the excess carbon dioxide exhaled by the astronauts: LiOH(s) + CO2 (g) ? LiHCO3(s) Each lithium hydroxide cartridge that is used to remove carbon dioxide from the air has a lithium hydroxide mass of 32.0 kg. If the process for removing the carbon dioxide has a percentage yield of 88 percent, what mass of carbon dioxide is removed by each canister of lithium hydroxide?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter5: Gases

Section: Chapter Questions

Problem 101E: At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A...

See similar textbooks

Similar questions

Mass of the gelatin capsule was: 0.1134 g Mass of the capsule and the allow sample was: 0.3218 g Ambient Temperature was: 23°C Mass of empty beaker: 154.3 g Mass of beaker with water: 401.6 g Vapor pressure of water for this data: 21.1 mmHg Atmospheric Pressure: 732 mmHg Assume density of water to be 1.0000 g/mL What is the volume of the displaced water in Liters? Using PH2V= nH2RT, nH2=PH2V/RT how many moles of H2 were evolved? Determine the number of moles of H2 per gram of sample. Determine the %Al using NH2= (%AL/100 * 0.0556) + (100-%AL/100 * 0.0153)
The ozone concentration at a monitoring site is measured as 0,11 ppm, at 25 °C and 1 atm. What is the concentration (in pg/m3) at 25 °C and 1 atm? (MW of ozone is 48)a. 155 pg/m3b. 190 pg/m3c. 215 pg/m3d. 260 pg/m3
-ELON TWEETED HOD * OWLV2 | Online teaching and I + UPDATES AVAILABLE akeAssignment/takeCovalentActivity.do?locator=assignment-take Do you want to restart to install these un or try tonight? [Review Topics] [References) 2req Use the References to access important values if needed for this question. A sample of hydrogen gas at a pressure of 810 mm Hg and a temperature of 42 °C, occupies a volume of 14.4 liters. If the gas is heated at constant pressure to a temperature of 76 °C, the volume of the gas sample will be L. 2req Submit Answer Retry Entire Group 9 more group attempts remaining Visited Next Previous
I'm sorry. I actually forgot to ask the full question earlier about the mass of ammonium at stp. The entire question was what is the mass of 3 L of ammonia at stp?
Mind Tap - Cengage Learning X om/ilrn/takeAssignment/takeCovalent Activity.do?locator=assignment-take me teaching and le X [Review Topics] [References] Use the References to access important values if needed for this question. An 1.11 mol sample of nitrogen gas at a temperature of 10.0°C is found to occupy a volume of 27.5 liters. The pressure of this gas sample is atm. Submit Answer 888 F4 + A FS Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support MacBook Air VA DII DD Previous
1000 ml of oxygen at STP were passed through an ozoniser and the resulting volume was 888 ml at STP. This quantity of ozonised oxygen is passed through excess of KI solution. The weight of I2 liberated is(a) 25.4 g (b) 12.7 g(c) 2.54 g (d) 1.27 g
Which of these criticality scenarios—subcritical, critical, or supercritical—is desirable in a nuclear power plant that generates electricity?
ng and le X Mind Tap - Cengage Learning X + takeAssignment/takeCovalent Activity.do?locator=assignment-take Submit Answer - [Review Topics] [References] Use the References to access important values if needed for this question. A sample of oxygen gas occupies a volume of 9.60 L at 51.0°C and 358 torr. If the volume of the gas sample is decreased to 7.02 L, while its temperature is decreased to -9.0°C, the resulting gas pressure will be torr. Retry Entire Group 7 more group attempts remaining Cengage Learning Cengage Technical Support û MacBook Air ☐ Previous Next Save and
The stopcock connecting a l.13 L bulb containing xenon gas at a pressure of 5.08 atm, and a 4.71 L bulb containing krypton gas at a pressure of 1.31 atm, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is atm. Submit Answer Retry Entire Group 9 more group attempts remaining
What is the interior layers of a mercury?
ving a piece of pine wood 7. Calculate the mass of 0.5 moles of (NH4)3ASO4. -1....pdf F4 d 10 % Diffusion and O....docx tv KO F5 A C F6 ∞ .ılı A very brief Hist....pdf F7 F8 F9
SpaceX recently launched their Falcon Heavy rocket (Feb. 6, 2018). It is based on their existing Falcon 9 rocket. The Falcon 9 rocket has a first stage which is a 40 m high by 3.7 m diameter cylinder. This cylinder contains the fuel used to propel the rocket which consists of RP-1 (rocket propellant-1, high grade kerosene), and liquid oxygen, O2 (`). RP-1 is a complex mixture of hydrocarbons but let’s approximate it with a chemical composition of C12H26. The densities of the fuel are ρ (RP − 1) = 0.83 g cm3 ρ (liquid O2) = 1.141 g cm3 If the total volume available for the two tanks is contained in the 40 m high by 3.7 m diameter first stage, determine the volume of each individual tank that will provide the exact amount of RP-1 and oxygen for the reation (no limiting reagent) and take up the entire volume of the first stage. Here are some suggestions to guide you. 1. Write a balanced combustion reaction for C12H26 with O2. 2. Determine the ratio of the volumes of the individual RP-1…

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781285199023

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781285199023

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS