What would you observe when zinc is added to a solution of iron $(II) $ sulphate ? Write the chemical reaction that takes place.
What would you observe when zinc is added to a solution of iron $(II) $ sulphate ? Write the chemical reaction that takes place.
Zinc is more reactive than iron. Therefore, if zinc is added to a solution of iron $II$ sulphate, then it would displace iron from the solution.
$\text{Z}{{\text{n}}_{(s)}}\,+\,FeS{{O}_{4(aq)}}\,\to \,ZnS{{O}_{4(aq)}}\,+\,F{{e}_{(s)}}$
Similar Questions
Metallic oxides of zinc, magnesium and copper were heated with the following metals.
Metal
Zinc
Magnesium
Copper
Zinc oxide
-
-
-
Magnesium oxide
-
-
-
Copper oxide
-
-
-
In which cases will you find displacement reactions taking place ?
Metallic oxides of zinc, magnesium and copper were heated with the following metals.
| Metal | Zinc | Magnesium | Copper |
| Zinc oxide | - | - | - |
| Magnesium oxide | - | - | - |
| Copper oxide | - | - | - |
In which cases will you find displacement reactions taking place ?
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Give reasons : Sodium, potassium and lithium are stored under oil.
Give an example of a metal which
$(i)$ is a liquid at room temperature.
$(ii)$ can be easily cut with a knife.
$(iii)$ is the best conductor of heat.
$(iv)$ is a poor conduct of heat.
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$(i)$ is a liquid at room temperature.
$(ii)$ can be easily cut with a knife.
$(iii)$ is the best conductor of heat.
$(iv)$ is a poor conduct of heat.
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