Is cobalt chloride equilibrium endothermic or exothermic?
– heating cobalt(II) chloride hydrate The formation of is endothermic. On heating, the equilibrium shifts to the left and the solution turns blue.
In which direction is the cobalt equilibrium shifted by increasing the temperature of this reaction?
forward direction
Increasing the temperature of an endothermic reaction shifts the equilibrium in the forward direction, to consume some of the excess energy and make more products.
How would the addition of water affect the hydrated cobalt ion equilibrium?
Adding water would shift equilibrium to favor the formation of the hydrous form.
What happens when you heat cobalt II chloride?
The cobalt chloride dihydrate is purple in color and cobalt chloride hexahydrate is pink in color. The cobalt chloride hexahydrate decomposes on heating to form cobalt chloride and water.
Is the cobalt equilibrium reversible?
A solution of cobalt(II) ion in water is pink, the color of the complex ion formed between Co2+ ions and water molecules. This reaction is reversible and quickly reaches a position of chemical equilibrium, which is immediately evident by the color of the solution.
Is the reaction exothermic why co H2O 6 2 +( aq )+ 4cl − AQ ⇌ CoCl4 2 − aq )+ 6h2o L?
The Co(H2O)62+ complex is pink, and the CoCl42- complex is blue. This reaction is endothermic as written, so adding heat causes the equilibrium constant to shift to the right.
What is the molar mass of cobalt II chloride hexahydrate?
237.93
Cobalt chloride hexahydrate
| PubChem CID | 24643 |
|---|---|
| Molecular Formula | Cl2CoH12O6 |
| Synonyms | Cobalt chloride hexahydrate Cobalt dichloride hexahydrate cobalt chloride hydrate cobalt (II) chloride hexahydrate UNII-17AVG63ZBC More… |
| Molecular Weight | 237.93 |
| Component Compounds | CID 962 (Water) CID 313 (Hydrochloric acid) CID 104730 (Cobalt) |
What happens when you add water to cobalt II chloride?
If the chloride or cobalt concentrations increase, the equilibrium will also shift towards the blue anhydrous cobalt chloride. Add water, however, and the equilibrium will shift back towards the pink hydrated species.
How will the cobalt equilibrium be affected?
Watch as the equilibrium between two different coloured cobalt species is disturbed, accompanied by a colour change predicted by Le Chatelier’s principle. This equilibrium can be disturbed by changing the chloride ion concentration or by changing the temperature.
What to know about cobalt (II) chloride?
Cobalt (II) chloride Properties. Cobalt (II) chloride is normally found in the red (or pink) form. The red form has water in it. Preparation. The anhydrous (without water) blue form can be made by reacting cobalt with chlorine. Uses. It is used to place cobalt into other chemical compounds. Safety. It is a weak oxidizing agent, too weak to ignite things.
What is the formula for cobalt(II) chloride?
Cobalt(II) chloride is an inorganic compound of cobalt and chlorine, with the formula CoCl 2. It is a sky blue crystalline solid. The compound forms several hydrates CoCl 2 • nH 2O, for n = 1, 2, 6, and 9. Claims of the formation of tri- and tetrahydrates have not been confirmed.
What is the formula for cobalt II chlorite?
Cobalt(II) chlorate is a chemical compound with the formula Co(ClO 3) 2. It is formed by a double displacement reaction between cobalt(II) sulfate and barium chlorate , barium sulfate precipitates and cobalt chlorate can be crystallized out of the filtrate.
What is the formula for cobalt (II) chlorate dihydrate?
Formula and structure: The cobalt (II) chloride chemical formula is CoCl 2. This molecule present different level of hydratation: anhydrous (CoCl 2 ), dihydrate (CoCl 2 .2H 2 O) and hexahydrate (CoCl 2 .6H 2 O) which have molar mass of 129.839 g mol -1, 165.87 g mol -1 and 297.93 g mol -1.