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12 Dec 2019

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

Part B at equilibrium Express your answer in kilojoules.

Part C PICl= 2.55 atm ; PI2= 0.325 atm ; PCl2= 0.217 atm . Express your answer using one significant figure.

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13 Dec 2019

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Related questions

Consider the following reaction:

I_2(g) + Cl_2(g) ⇌ 2ICl_(g) K_p= 81.9 at 25^∘C.

Calculate ΔG_rxn for the reaction at 25^∘C under each of the following conditions.

Part A. Standard conditions

Part B. At equilibrium

Part C. P_ICl= 2.59 atm; P_I2= 0.322 atm; P_Cl2= 0.221 atm

ochrekoala614

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.

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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