The equilibrium system co(h2o)62+ + 4cl– ⇌ cocl42– + 6h2o is endothermic as written, meaning heat is a reactant for the forward reaction and a product for the reverse reaction. based on that information and your findings from this experiment, predict what you would expect to observe in the experiment you described above when you tested the effects of temperature on an equilibrium position.

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 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 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.

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.