A mixture of 0.737 atm CIF, , 0.419 atm F, , and 0.396 atm ClIF is heated in a closed vessel to 700 K. CIF, (g) = CIF(g) + F,(g) Kp = 0.140 at 700 K Calculate the equilibrium pressure of each gas at 700 K.

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Chapter1: Chemical Foundations
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A mixture of 0.737 atm ClF30.737 atm ClF3 , 0.419 atm F20.419 atm F2 , and 0.396 atm ClF0.396 atm ClF is heated in a closed vessel to 700 K700 K .

 

ClF3(g)↽−−⇀ClF(g)+F2(g)?p=0.140 at 700 KClF3(g)↽−−⇀ClF(g)+F2(g)Kp=0.140 at 700 K

 

Calculate the equilibrium pressure of each gas at 700 K700 K .

?ClF3=
 
?ClF=
 
?F2=
 
A mixture of 0.737 atm CIF, , 0.419 atm F, , and 0.396 atm CIF is heated in a closed vessel to 700 K.
CIF, (g) = CIF(g) + F, (g)
= 0.140 at 700 K
Calculate the equilibrium pressure of each gas at 700 K.
PCIF,
atm
PCIF
atm
PF,
atm
Transcribed Image Text:A mixture of 0.737 atm CIF, , 0.419 atm F, , and 0.396 atm CIF is heated in a closed vessel to 700 K. CIF, (g) = CIF(g) + F, (g) = 0.140 at 700 K Calculate the equilibrium pressure of each gas at 700 K. PCIF, atm PCIF atm PF, atm
Expert Solution
Step 1

The equilibrium reaction given is,

=> ClF3 (g)  ClF (g) + F2 (g)                  Kp = 0.140

Given: Initial pressure of ClF3 = 0.737 atm.

Initial pressure of ClF = 0.396 atm.

And initial pressure of F2 = 0.419 atm.

 

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