Question

Chemical reaction when chromium metal is immersed in an aqueous solution of cobalt(II) chloride.

Answer 1

2Cr(s) + 3CoCl2 (aq) --> 2CrCl3 (aq) + 3Co (s)

Step-by-step explanation:

Any metal on the activity series can be oxidized by the ions of elements below it. Since cobalt is below chromium, the chromium metal will react with the Co2+ ions of cobalt chloride.

Answer 2

`2Cr + 3CoCl_2`→
`2CrCl_3 + 3Co`

Step-by-step explanation:

• The products formed are chromic chloride and cobalt.

Chromium + Cobaltous Chloride = Chromic Chloride + Cobalt

• Type of reaction is Single Displacement (Substitution) which is there is a displacement of one atom.

Reactants used in the reaction are -

• Chromium
  `(Cr)`

• Cobaltous Chloride
  `(CoCl_2)`

Products formed in the reaction are -

• Chromic Chloride
  `(CrCl_3)`

• Cobalt
  `(Co)`

Hence, the chemical reaction is as follows -

• 
  `Cr + CoCl_2` →
  `CrCl_3 + Co`

For balancing the above chemical equation we need to add a coefficient of 2 in front of chromium and of 3 in front of cobalt(II)chloride on right-hand-side while of 2 in front of chromium chloride and of 3 in front of carbon monoxide on left-hand-side of the equation.

Hence, the balanced equation is -

`2Cr + 3CoCl_2`→
`2CrCl_3 + 3Co`