(Solved): If we represent the equilibrium as: Co2+(aq)+4Cl(aq)CoCl42(aq) We can conclude that: 1 ...

If we represent the equilibrium as: $${\mathrm{Co}}^{2+}(aq)+4{\mathrm{Cl}}^{?}(aq)?{\mathrm{CoCl}}_4^{2?}(aq)$$ We can conclude that: 1. This reaction is exothermic. endothermic. neutral. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, $$K$$ : increases. decreases. remains the same. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of $${\mathrm{Co}}^{2+}$$ : increases. decreases. remains the same. More information is needed to answer this question.