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13 Dec 2019

The reaction I2(g)+Cl2(g)?2ICl(g) (Kp = 81.9) is carried out at 25?C with these initial partial pressures: PI2 = 0.145 atm ,PCl2 = 0.145 atm ,PICl = 0.00 atm.

1. Find the equilibrium partial pressure of I2.
Express your answer with the appropriate units.

2. Find the equilibrium partial pressure of Cl2.
Express your answer with the appropriate units.

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Tod Thiel
Tod ThielLv2
17 Dec 2019

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Related questions

Consider the following equilibrium at 994 K

. H2(g) + I2(g) equilibrium reaction arrow 2 HI(g); Kp = 43.1

Suppose this reaction is started with 0.326 atm H2 and 0.326 atm I2 at the same temperature. Assume the initial partial pressure of product is equal to 0. Calculate the equilibrium partial pressures of each reaction component.

pH2 = ?? . atm pI2 =?? atm pHI = ?? atm

I don't know how to set this problem up. Could someone pleaseshow me the steps?


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?

At 964 oC the equilibrium constant for the reaction:
2 HI(g) H2(g) + I2(g) is KP = 8.47e-10. If the initial pressure ofHI is 2.92e-03 atm, calculate the equilibrium partial pressures ofHI, H2, and I2. Pick the choice which gives the correct value forthe equilibrium partial pressure of one of these gases.

a) PH2(eq) = 2.13e-08 atm
b) PH2(eq) = 2.55e-07 atm
c) PI2(eq) = 2.55e-07 atm
d) PI2(eq) = 8.50e-08 atm
e) PHI(eq) = 1.70e-07 atm

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