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Consider the reaction between iodine gas and chlorine gas toform iodine monochloride:
I2(g)+Cl2(g)?2ICl(g)Kp=81.9(at 298 K)
A reaction mixture at 298 K initially contains PI2=0.35atmand PCl2=0.35atm.


What is the partial pressure of iodine monochloride when thereaction reaches equilibrium?

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Related questions

What is the partial pressure of iodine monochloride when the reaction reaches equilibrium? Express your answer to two significant figures and include the appropriate units.

Consider the reaction between iodine gas and chlorine gas to form iodine monochloride:
I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K)
A reaction mixture at 298 K initially contains PI2=0.30 atm and PCl2=0.30 atm .

Consider the reaction between iodine gas and chlorine gas to form iodine monochloride:
I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K)
A reaction mixture at 298 K initially contains PI2=0.25 atm and PCl2=0.25 atm .

You may want to reference (Page) Section 15.8 while completing this problem.

Part A

What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?

Express your answer to two significant figures and include the appropriate units.

atm

SubmitPrevious AnswersR

1) Consider the reaction: X2(g)?2X(g). When a vessel initially containing 700torr of X2 comes to equilibrium at 298 K, the equilibrium partial pressure of X is 108torr . The same reaction is repeated with an initial partial pressure of 755torr of X2 at 700K ; the equilibrium partial pressure of X is 596torr .

Find ?H? for the reaction.

2) Consider the following reaction:
I2(g)+Cl2(g) ? 2ICl(g)
Kp= 81.9 at 25 ? C.
Calculate ?Grxn for the reaction at 25 ? C under each of the following conditions.

A) standard conditions:

?G?rxn = ____________ kJ

B) PICl= 2.60atm ;
PI2= 0.317atm ;
PCl2= 0.217atm .

?Grxn = ___________________ kJ

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