Answer the questions for the following reaction at chemical equilibrium: cl2(g) + kbr(aq) < > kcl(aq) + br2(l) + heat 1. which reaction (forward, backward, or neither) would be favored by increasing the temperature? 2. which reaction (forward, backward, or neither) would be favored by adding cao? 3. which reaction (forward, backward, or neither) would be favored if the amount of chlorine gas (cl2 gas) was decreased? 4. which reaction (forward, backward, or neither) would be favored if the pressure was increased? 5. which reaction (forward, backward, or neither) would be favored if more cl2 gas is added?

1.Backward

2.Neither

3.Backward

4.Forward

5.Forward

Explanation:

When we increase the temperature

Then, by Lechatelier principle

It states that if a constraints such as concentration of reactants,change in volume , pressure,temperature  is applied to a system of equilibrium ,the equilibrium shift in a direction in which oppose the effect of constraints.

Using Lechatelier principle

1.The equilibrium shift in backward direction when we increase the temperature.

2.When we add CaO then it is not reactant of given reaction or not a product therefore, when we add CaO then it does not effect euilibrium condition.

Then , the equilibrium neither shift in any direction.

3.When we decrease the concentration of chlorine gas then the number of

Then the equilibrium shift in backward direction by Le chetelier principle.

Hence , the reaction would be favored backward  if the amount of chlorine gas was decreased.

4.When we increase the pressure then the equilibrium shift in forward direction.

Hence, the reaction would be favored in forward reaction when we increase the pressure.

5.When we increase concentration of any  reactant then the equilibrium shift in forward direction.

Hence, when we add more chlorine gas then the reaction would be favored forward reaction.