Consider the following system at equilibrium where Kc = 1.29Ã—10-2 and HÂ° = 108 kJ/mol at...

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Chemistry

Consider the following system at equilibrium where Kc =1.29Ã—10-2 and HÂ° = 108 kJ/mol at 600 K.

COCl2 (g) CO (g) + Cl2 (g)

The production of CO (g) is favored by:

Indicate True (T) or False (F) for each of the following:

_
T
F
1. decreasing the temperature.
_
T
F
2. increasing the pressure (by changing the volume).
_
T
F
3. decreasing the volume.
_
T
F
4. adding COCl2 .
_
T
F
5. removing Cl2 .

Consider the following system at equilibrium where Kc = 77.5 and HÂ°= -108 kJ/mol at 600 K.

CO (g) + Cl2 (g) COCl2 (g)

The production of COCl2 (g) is favored by:

Indicate True (T) or False (F) for each of the following:

_
T
F
1. decreasing the temperature.
_
T
F
2. decreasing the pressure (by changing the volume).
_
T
F
3. decreasing the volume.
_
T
F
4. removing COCl2 .
_
T
F
5. removing Cl2 .

Answer & Explanation Solved by verified expert

4.0 Ratings (740 Votes)

PartA The given reaction is COCl2g COg Cl2g H0 108 KJmol Now Expression of Equilibrium constant ie Kc CO g Cl2 g COCl2 g This is an endothermic reaction as H0 ve 1 decreasing the temperature FALSE because according to Lechateliers principle on decreasing the temperature for endothermic reaction equilibrium will shifts in backward direction ie reactant side and viceversa Hence this will not favor production of CO 2 increasing the pressure by changing the volume FALSE because according to Lechateliers principle on increases the pressure equilibrium will shifts in that direction where See Answer

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