In an aqueous chloride solution cobalt (ii) exists in equilibrium with the complex ion cocl42-. co2 + (aq) is pink and cocl42 - (aq) is blue ... at low temperature the pink color predominates ... at high temperature the blue color is strong ... if we represent the equilibrium as: ... co2 + (aq) + 4cl - (aq) cocl42 - (aq) we can conclude that: 1. this reaction is:

a. exothermic

b. endothermic

c. neutral

d. more information is needed to answer this question.

Question

Chemistry

Harper Barrera

19 July, 15:34

In an aqueous chloride solution cobalt (ii) exists in equilibrium with the complex ion cocl42-. co2 + (aq) is pink and cocl42 - (aq) is blue ... at low temperature the pink color predominates ... at high temperature the blue color is strong ... if we represent the equilibrium as: ... co2 + (aq) + 4cl - (aq) cocl42 - (aq) we can conclude that: 1. this reaction is:

a. exothermic

b. endothermic

c. neutral

d. more information is needed to answer this question.

+4

Answers (1)

Know the Answer?

Princess Snyder · Answer 1

Answer is: this reaction is b. endothermic, when heat is added to equilibrium, the position of equilibrium moves to right.

Chemical reaction: Co ²⁺ (aq) + 4Cl⁻ (aq) ⇄ CoCl₄²⁻ (aq).

According to Le Chatelier's Principle, the position of equilibrium moves to counteract the change, the position of equilibrium will move so that the concentration of products of chemical reaction increase if we increase temperature.