Assume that you have a mixture of He (MW = 4 amu) and Xe (MW = 131 amu) at 300 K. The total pressure of the mixture is 750 mmHg. What are the partial pressures of each of the gases? (blue = He; green = Xe)? ▼ Part A What is the partial pressure of He? Express your answer to three significant figures and include the appropriate units. PHe= |μA Value Part B Units Submit Previous Answers Request Answer ? X Incorrect; Try Again; 9 attempts remaining What is the partial pressure of Xe? Express your answer to three significant figures and include the appropriate units.

Assume that you have a mixture of He (MW = 4 amu) and Xe (MW = 131 amu) at 300 K. The total pressure of the mixture is 750 mmHg. What are the partial pressures of each of the gases? (blue = He; green = Xe)? ▼ Part A What is the partial pressure of He? Express your answer to three significant figures and include the appropriate units. PHe= |μA Value Part B Units Submit Previous Answers Request Answer ? X Incorrect; Try Again; 9 attempts remaining What is the partial pressure of Xe? Express your answer to three significant figures and include the appropriate units.

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

please answer the question and show your work 5a. An automobile airbag inflates when sodium azide (NaN3) is converted to sodium (Na) and N2 gas according to the BALANCED equation, 2 NaN3 → 2 Na + 3 N2. What volume in liters (L) of N2 gas will be produced if 115 g of NaN3 completely reacted at STP (standard temperature and pressure). Molar mass of NaN3 = 65.02 g/mol 1 mol of any gas at STP = 22.4 L
How many grams of NaClO3 were decomposed?
A 5.65 L vessel contains 22.0 g of PC13 and 3.35 g of O2 at 15.0 °C. The vessel is heated to 215 °C, and the contents react to give POC13. What is the final pressure in the vessel, assuming that the reaction goes to completion and that all reactants and products are in the gas phase? -- ΑΣΦ P= 1.441 ? atm
5. Does the pressure-volume relationship follow the ideal gas law PV=nRT (is PV constant at constant n and T) Using the room temperature calculate the number of moles in the pressure/volume experiment when the pressure is 1.00atm in 3.1
A 5.00 L tank at 7.96 °C is filled with 10.8 g of chlorine pentafluoride gas and 4.88 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. ol. mole fraction: x10 chlorine pentafluoride Ar ? partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm
#14
10b
we use Pv=nRT. Everything here should be related to H2 (g) --> Chemical equation1Mg +2 HCl à MgCl2 +H2(g) From video : mass of Mg =.0407 g H2 gas volume = 38.2ml Temperature of room=24.0 +273=297k Total Pressure of the room = 30.01 in mmHg Calculations: find total pressure from barometer and convert it to mmHg, 1 in =2.54 cm and 25.4 mm 30.01 in mmHg x 25.4 mm Hg =762.3 mmHg total pressure of room 1in mmHg First step- convert g of Mg to mol of H2 0.0407g Mg x 1mol/24 gx 1molH2 = 0.00169mol 1mol Mg Second step: Total pressure of gas = Pressure of H2 + P of water 762.3 = p H2 + 22.4 FROM reference (canvas)=Pressure of water at 24 C= 22.4 mmHg n= 0.00169mol H2 Pressure of H2= 762.3-22.4= 739.854 x 1atm/760= 0.973 atm H2 Volume of H2= 38.2 ml /1000 =0.038L H2 Temp= 297K anwer this quesions with the information provide: Using PV=nRT, Find R=? (No R averge needed) à 0.973X0.0382=0.00169XRx 297 0.0372=0.50R Then, Percent error…
A quantity of helium gas is originally held under a pressure of 145 kPa at 18°C. If the volume of the container is tripled, and the temperature is increased to 30°C, what is the resulting pressure in kPa? (Hint, can you make up a volume?) H 322181 Li Na Mg Rb Be Sr Cs Ba Fr 22 Ca Sc Ti Ra Raden Lat 94.5 kPa 46.4 kPa 378.3 kPa 453.9 kPa 50.3 kPa MD 45 83-103 482.2 kPa Zr Hf Atvice Ac Th Series 23 VO Vieta VID 24 2 Ta W Tete 104 105 Rf Db Sg Cr Mn Periodic Table of the Elements VID 75 41. 34445 Nb Mo Tc Ru Rh Pd Ag Cd Abaline Tra Saber 26 27 28 29 30 Fe Co Ni Cu Zn Re Os Symbol S 13 13 FIA B Nawww Al Ga Halagan In La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho D IVA 70 Pt Au Hg Tl Pb B Mar 102108, 109 114 Bh Hs Mt Ds Rg Cn Uut "FI 590 U Np Pu Am Cm Bk Cf Es Sn Sb 14 15 16 17 18 Si CI Ar La 16 3514. Ge As Se Br Kr By 17 VIA 18 VELA He Hek 4000 Ne 62 63 64 SA Te I Xe 16 At Rn Fate Bi Po Uup "Lv Uus Uuo Er Tm Yb Lu C Henan 100 100 Fm Md No L
A reaction between liquid reactants takes place at - 14.0 °C in a sealed, evacuated vessel with a measured volume of 40.0 L. Measurements show that the reaction produced 36. g of chlorine pentafluoride gas. Calculate the pressure of chlorine pentafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits. pressure: |II atm
Hello, I need help finding the partial pressure of Hydrogen present. Thank you.
5 Calculate the mass of carbon monoxide gas (in mg) dissolved in 9.8L tank exposed to a pressure of 1.13 atm of air at 25˚C. Assume the mole fraction of carbon monoxide gas in air to be 0.112 given that the Kh for CO is 9.5 x 10-4 M/atm. Report answer to the correct significant figures with no units.