Br2(l)+Cl2(g) (double arrow) 2BrCl(g)

dH=+29.4 kJ/mol

I am having trouble understanding this. Will the system shift left, right, or unchanged and why?

a.Increasing Temp.
b. Increasing pressure in flask by adding Ar.
c. Increasing volume of flask
d. Adding Br2(l)...is answer move right
e. Removing Cl2(g)...is " left?
f. Adding BrCl(g)...is " left?
g. Adding catalyst

To determine the effect of each change on the equilibrium position, we need to consider Le Chatelier's principle. Le Chatelier's principle states that when a system in equilibrium is subjected to a change, it will adjust itself to minimize the effect of that change.

a. Increasing temperature: According to Le Chatelier's principle, increasing the temperature will favor the endothermic reaction, which is the forward reaction. Therefore, the equilibrium will shift to the right (towards the products) to consume some of the added heat. In this case, the equilibrium will shift to the right, resulting in an increase in the concentration of BrCl(g).

b. Increasing pressure in the flask by adding Ar: The reaction involves only gases, so increasing the pressure will not affect the equilibrium position. The system will remain unchanged.

c. Increasing the volume of the flask: Increasing the volume will decrease the pressure in the flask. According to Le Chatelier's principle, the system will shift in the direction that decreases the number of moles of gas. In this case, the equilibrium will shift to the left (towards the reactants) to reduce the pressure. Therefore, the concentration of BrCl(g) will decrease.

d. Adding Br2(l): Adding more Br2 will increase the concentration of Br2. According to Le Chatelier's principle, the system will shift in the direction that consumes the excess reactant. In this case, the equilibrium will shift to the right (towards the products) to consume the additional Br2. Therefore, the concentration of BrCl(g) will increase.

e. Removing Cl2(g): Removing Cl2 will decrease the concentration of Cl2. According to Le Chatelier's principle, the system will shift in the direction that replenishes the removed component. In this case, the equilibrium will shift to the left (towards the reactants) to produce more Cl2. Therefore, the concentration of BrCl(g) will decrease.

f. Adding BrCl(g): Adding more BrCl will increase the concentration of BrCl. According to Le Chatelier's principle, the system will shift in the direction that reduces the excess product. In this case, the equilibrium will shift to the left (towards the reactants) to consume the additional BrCl. Therefore, the concentration of BrCl(g) will decrease.

g. Adding a catalyst: Adding a catalyst does not affect the equilibrium position. A catalyst only speeds up the rate of the forward and reverse reactions, but it does not change the position of the equilibrium.

In summary:
- Increasing temperature shifts the equilibrium to the right.
- Increasing pressure has no effect on the equilibrium.
- Increasing the volume shifts the equilibrium to the left.
- Adding Br2 shifts the equilibrium to the right.
- Removing Cl2 shifts the equilibrium to the left.
- Adding BrCl shifts the equilibrium to the left.
- Adding a catalyst has no effect on the equilibrium.