Medium
What happens when a piece of
$(a)$ zinc metal is added to copper sulphate solution?
$(b)$ aluminium metal is added to dilute hydrochloric acid?
$(c)$ silver metal is added to copper sulphate solution?
Also,write the balanced chemical equation if the reaction occurs.
$(a)$ zinc metal is added to copper sulphate solution?
$(b)$ aluminium metal is added to dilute hydrochloric acid?
$(c)$ silver metal is added to copper sulphate solution?
Also,write the balanced chemical equation if the reaction occurs.
(A) Zinc,being more reactive than copper,displaces copper from its solution,and a solution of zinc sulphate is obtained.
$Zn(s) + CuSO_4(aq) \rightarrow ZnSO_4(aq) + Cu(s)$
This is an example of a displacement reaction.
$(b)$ Aluminium,being more reactive,displaces hydrogen from dilute hydrochloric acid solution,and hydrogen gas is evolved.
$2Al(s) + 6HCl(aq) \rightarrow 2AlCl_3(aq) + 3H_2(g)$
$(c)$ Silver metal,being less reactive than copper,cannot displace copper from its salt solution. Therefore,no reaction occurs.
$Ag(s) + CuSO_4(aq) \rightarrow \text{No reaction}$
$Zn(s) + CuSO_4(aq) \rightarrow ZnSO_4(aq) + Cu(s)$
This is an example of a displacement reaction.
$(b)$ Aluminium,being more reactive,displaces hydrogen from dilute hydrochloric acid solution,and hydrogen gas is evolved.
$2Al(s) + 6HCl(aq) \rightarrow 2AlCl_3(aq) + 3H_2(g)$
$(c)$ Silver metal,being less reactive than copper,cannot displace copper from its salt solution. Therefore,no reaction occurs.
$Ag(s) + CuSO_4(aq) \rightarrow \text{No reaction}$
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