Answer;
-Macroscopic properties remain constant
-Concentrations remain constant
-No change to copper solution seen;
-Rate of reverse/backwards reaction = rate of forward reaction;
Explanation;
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system.
-It is a a condition in the course of a reversible chemical reaction in which no net change in the amounts of reactants and products occurs. A reversible chemical reaction is one in which the products, as soon as they are formed, react to produce the original reactants.
Answer:
- Increasing the temperature: shifts the equilibrium to the products side (towards the right direction).
- Decreasing the temperature: shifts the equilibrium to the reactants (towards the left direction).
Explanation:
Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.
For the mentioned endothermic reaction can be represented as:
Co(H₂O)₆²⁺ + 4Cl⁻ + heat ⇌ CoCl₄²⁻ + 6H₂O.
In endothermic reactions: heat is a reactant for the forward reaction and a product for the reverse reaction.
So the effect of temperature on the equilibrium position is:
- Increasing the temperature:
Increasing the temperature leads to increasing the concentration of the reactants, so the equilibrium will be shifted to the products side (towards the right direction) to suppress the effect of increasing T.
- Decreasing the temperature:
Decreasing the temperature leads to decreasing the concentration of the reactants, so the equilibrium will be shifted to the reactants (towards the left direction) to suppress the effect of decreasing T.