Question

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

Answer 1

$2Cr + 3CoCl_2$→ $2CrCl_3 + 3Co$

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 -

$2Cr + 3CoCl_2$→ $2CrCl_3 + 3Co$

Answer 2

Answer:

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

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.