Exam question PLEASE PLEASE HELP

Chemistry
Tutor: None Selected Time limit: 1 Day

a 667 cm cubed cylinder contains 7.8 moles of nitrogen, 5,0 moles of oxygen, 1.7 moles of helium, and an unknown number of moles of carbon dioxide at 100 degrees celsius. the pressure gauge on the cylinderreads exactly 1500 atm. calculate the partial pressure of each gas in the mixture.

PLEASE SHOW WORK

Aug 5th, 2015

Thank you for the opportunity to help you with your question!

P total = p1+p2+p3+p4

total number of moles=

PV=nRT

n=RT/PV = 8.314*373/[1500 atm *0.000667m3]

  =

moles of Co2



kindly allow me to finish in a followup . It is a long question and I cannot finish in given 20 minutes. Thank you in advance

Please let me know if you need any clarification. I'm always happy to answer your questions.
Aug 5th, 2015
nT=PV/RT = [151978500pa* 0.000667m3]/[8.314*373]=32.68 moles


moles of Co2= 32.68-[7.8+5+1.7]=18.8 moles
partial pressure
partial pressures in atm
CO2=18.8/32.68*15OO=834.45
NITROGEN=7.8/32.68*1500=358.017
O2=5/32.68*1500=229.4
HELIUM =1.7/32.68*1500=78


Aug 5th, 2015

Are you studying on the go? Check out our FREE app and post questions on the fly!
Download on the
App Store
...
Aug 5th, 2015
...
Aug 5th, 2015
Dec 4th, 2016
check_circle
Mark as Final Answer
check_circle
Unmark as Final Answer
check_circle
Final Answer

Secure Information

Content will be erased after question is completed.

check_circle
Final Answer