7. A hyperbaric chamber has a volume of 200. L. (a) How many moles of oxygen areneeded to fill the chamber at room temperature (23°C) and 3.00 atm pressure? (b)How many grams of oxygen are needed? (Hint: Since moles have been asked, whichequation has the moles listed in the equation. Use that to solve this problem. Alsodon't forget to use the equation 1 mole = Formula weight or Molecular weight tocalculate thegramsof02).bility: Good to goO,Focur

Answered: Image /qna-images/answer/d5f2bf18-a1cf-4f90-a92b-fd1be9ce46e2.jpg

7. A hyperbaric chamber has a volume of 200. L. (a) How many moles of oxygen are needed to fill the chamber at room temperature (23°C) and 3.00 atm pressure? (b) How many grams of oxygen are needed? (Hint: Since moles have been asked, which equation has he moles listed in the equation. Use that to solve this problem. Also don't forget to use the equation 1 mole = Formula weight or Molecular weight to calculate the grams of 02).

7. A hyperbaric chamber has a volume of 200. L. (a) How many moles of oxygen are needed to fill the chamber at room temperature (23°C) and 3.00 atm pressure? (b) How many grams of oxygen are needed? (Hint: Since moles have been asked, which equation has he moles listed in the equation. Use that to solve this problem. Also don't forget to use the equation 1 mole = Formula weight or Molecular weight to calculate the grams of 02).

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the molar concentration of the cleaning solutionformed when 10.0 L of ammonia gas at 33°C and 735 torr dis-solves in enough water to give a final volume of 0.750 L?
0.374 m3 of hydrogen was observed at −7.0 oC and atmospheric pressure (105 Pa). The relative molecular mass of hydrogen is 2.02 g mol-1 and the gas constant, R, is 8.314 J K−1 mol−1 a) Calculate the number of moles (round to 2 decimal places): b) Calculate the mass of the gas in g (round to 3 significant figures):
3. A mixture of Na2CO3 and NaHCO3 has a mass of 22.0 g. Treatment with excess HCI solution liberates 6.00 L CO2 at 25°C and 0.947 atm pressure. Determine the percent Na2CO3 in the mixture. Hint: Remember, percent mass is the ratio of the mass of substance and the total mass. 55% O 35% 40% 65%
A sample of helium gas collected at a pressure of 1.11 atm and a temperature of 285 K is found to occupy a volume of 884 milliliters. How many moles of He gas are in the sample?
If a gas sample (containing only N2 and O2) has a partial pressure of N2 of 360 mmHg and a partial pressure of O2 of 225 mmHg, what is the mole fraction of N2 in the sample?
A sample of neon gas occupies a volume of 750 ml at 25°C. What will the gas occupy at 50°C if the pressure remains constant?
The non-ideal molar volume of gaseous helium is approximately 20. L/mol. What is the density of this gas, in g/L?
Please help me with both!! Thank you!!
A sample of xenon gas collected at a pressure of 0.565 atm and a temperature of 26°C is found to occupy a volume of 22.8 liters. How many moles of Xe gas are in the sample? mol
[References] Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H2O2(aq) → 2H2O(1) + O2(g) What volume of pure O2(g), collected at 25°C and 744 torr, would be generated by decomposition of 127 g of a 50.0% by mass hydrogen peroxide solution? Ignore any water vapor that may be present. Volume = L
2 liters of an ideal gas are contained at 3.0 atm and 37 °C. How many moles of this gas are present?