Be sure to answer all parts. A mixture of CO2 and Kr weighs 47.9 g and exerts a pressure of 0.751 atm in its container. Since Kr is expensive, you wish to recover it from the mix…

Question

asked Mar 26, 2020 137k views

1 Answer

Arpit Gupta · Answer 1 · 2020-03-30T20:59:31+0000

Answer:a) Mass of
in mixture = 26.3 grams

b) Mass of
in mixture that can be recovered= 21.5 grams

Step-by-step explanation:

Given :

Total Pressure = pressure of krypton + pressure of carbon dioxide = 0.751 atm

pressure of krypton = 0.231 atm

Thus pressure of carbon dioxide = 0.751 - 0.231 =0.52 atm

As we know:

p=x* P

where,

= partial pressure

= total pressure = 0.751 atm

= mole fraction

For

x_(CO_2)=(p_(CO_2))/(P)=(0.52)/(0.751)=0.70

${\text {Mass of} CO_2}=moles* {\text {Molar mass}}=0.70* 44=30.8g$

For

x_(Kr)=(p_(Kr))/(P)=(0.231)/(0.751)=0.30

${\text {Mass of} Kr}=moles* {\text {Molar mass}}=0.30* 84=25.2g$

Total mass = Mass of
CO_2 + Mass of krypton = 30.8 + 25.2 = 56 g

Percentage of
$CO_2=(30.8)/(56)* 100=55\%$

a) Thus Mass of
in mixture =
(55)/(100)* 47.9=26.3g

Percentage of
$Kr=(25.2)/(56)* 100=45\%$

b) Thus Mass of
in mixture that can be recovered=
(45)/(100)* 47.9=21.5g