A) A student is studying the equilibrium described below:

blue + 4Br^-(aq)green + 6H₂O(l)

The system is at equilibrium and has a blue color. The student added several crystals to sodium bromide (NaBr) to this blue equilibrium solution. What will happen to the reaction, and why?

It will stay blue because you are adding a reactant so it will make more reactants.

It will turn green because it will make more product because you are adding a product.

It will turn green as it makes more products because you are adding a reactant.

It will stay blue because it will make more reactants as you are adding a product..

It will not change because sodium bromide is neither a reactant or a product for the reaction, so the equilibrium is unaffected.

B) A student is studying the equilibrium described in the equation below:

blue + 4Br^-(aq)green + 6H₂O(l)

The student placed the green equilibrium solution in an ice bath. After a short time, the solution turned blue. What does this tell you about the thermochemical character of the the forward reaction? [ Select ] ["The forward reaction is endothermic.", "The forward reaction is exothermic."] How do you know? [ Select ] ["heat must be a product because removing it made more reactants.", "heat must be a reactant since removing it made more reactants.", "heat must be a reactant because removing it made more products.", "heat must be a product since removing it made more products."]

C) A student obtained a test tube with a suspension of white, slightly soluble magnesium hydroxide in water. This system was at equilibrium as represented by the following equation:

Mg(OH)₂(s)Mg²⁺(aq) + 2OH^-(aq)

According to LeChtelier's principle, what will happen to the system if nitric acid,HNO₃, is added?

MoreMg(OH)₂(s)will be formed.

MoreMg²⁺(aq)will be formed.

MoreOH^-(aq)will be formed.

MoreMg(OH)₂(s)will dissolve.