Okay guys i need some help with figuring LETTER E out...i understand the rest, i

Question

Okay guys i need some help with figuring LETTER E out...i understand the rest, i just dont understand how to answer E. Please explain E so i can understand to get full points.

Consider the exothermic reaction: Cl2O(g) + H2O(l) - 2HCI(g) + O2(g). At equilibrium, 0.10 mol Cl2O, 5.00 mol O2, 10.0 mol HCI, and 2.00 mol H2O are present in a 20.0 L container at 25 degree C. Do you need to consider the volume occupied by liquid H?0? Justify your answer. Calculate the value for Kc at 25 degree C for the reaction shown above. Calculate the value for Kp at 25 degree C for the reaction shown above. If the system described by the equation above is initially at equilibrium, predict the direction of the shift in the position of equilibrium (left, right, no effect, or cannot be determined) and justify your prediction (be complete) for each of the following. Temperature and container volume remain constant, except where For each of the changes shown in Part d above, what effect (decrease, increase, no effect, or cannot be determined) would there be on the value for the equilibrium constant for the reaction?

Explanation / Answer

Cl2O(g)+ H2O(l) <===> 2HCl(g) + O2(g). Delta H= -ve

Equilibrium constant K = [HCl]^2[O2]/[ClO2]

1. equilibrium shifts towards left. so that backward reaction is favoured.

Equilibrium constant K decreases.

Equilibrium constant K decreases.

3.equilibrium do not effect.

Equilibrium constant K do not changes.

4.equilibrium shifts towards lefts. so that backward reaction is favoured.

Equilibrium constant K decreases.

5.equilibrium shifts towards right. so that forward reaction is favoured.

Equilibrium constant K increases.

6. no effect. due to constant volume.

Equilibrium constant K do not changes.

7. catalyst has no effect on equilibrium.

Equilibrium constant K do not changes.

8. no effect.because by increasing temperature by 10 degree celcius backward reaction is double.at the same time by increasing volume to double forward reaction is double . so that noeffect on reaction equilibrium.

Equilibrium constant K do not changes.

9.equilibrium shifts towards lefts. so that backward reaction is favoured.

Equilibrium constant K decreases.

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