Time remaining:

Chemistry Question ..

label Chemistry
account_circle Unassigned
schedule 0 Hours
account_balance_wallet $5

Nov 23rd, 2017

We have to use Dalton's law of partial pressures which states that in a mixture of gases each gas will exert its partial pressure corresponding to its molar fraction

In this case mixture consists of hydrogen4moles,helium 3 moles and krypton 2 moles packed in a cylinder of 9 litres and total pressure is 13atm

So partial pressure due to krypton is its mole fraction multiplied by total pressure

As krypton mole fraction is 2/9 its partial pressure is 2/9x13=26/9 atm=2.8888 atm

Now if we introduce  4 moles of xenon into the present system as vol and temperature are fixed

it will result in increase in total pressure corresponding to the moles added.

As the number of moles added are 4,the total moles increases from 9 to 13 and the total pressure in the cylinder will be 

13X13/9=169/9 ATM

 pkr= its changed mole fraction xchanged total pressure

=(2/13)x(169/9)=26/9 atm =2.8888atm

so it remains unchanged even if xenon is added

Now if we introduce 2 moles of krypton into the system without any change of temperature and volume

The total moles become 13+2=15 and the total pressure will be 169/9x15/13=195/9 atm

Krypton molar fraction now is 4/15

hence its partial pressure is molar fractionx total pressure

=(4/15)x(195/9)=52/9 atm=5.7777 atm


Nov 8th, 2014

Studypool's Notebank makes it easy to buy and sell old notes, study guides, reviews, etc.
Click to visit
The Notebank
Nov 23rd, 2017
Nov 23rd, 2017
Nov 24th, 2017
Mark as Final Answer
Unmark as Final Answer
Final Answer

Secure Information

Content will be erased after question is completed.

Final Answer