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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Write chemical equations for the reactions taking place when:
$(i)$ iron is strongly heated in air.
$(ii)$ lead carbonate is calcined.
$(iii)$ chromium oxide $(Cr_{2}O_{3})$ is heated with aluminium powder.
$(i)$ iron is strongly heated in air.
$(ii)$ lead carbonate is calcined.
$(iii)$ chromium oxide $(Cr_{2}O_{3})$ is heated with aluminium powder.
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$(a)$ An element which is a soft and reactive metal.
$(b)$ The metal which is an important constituent of limestone.
$(c)$ The metal which exists in a liquid state at room temperature.
$(a)$ An element which is a soft and reactive metal.
$(b)$ The metal which is an important constituent of limestone.
$(c)$ The metal which exists in a liquid state at room temperature.
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View Solution$A, B$ and $C$ are three elements which undergo chemical reactions according to the following equations:
$A_{2}O_{3} + 2B \rightarrow B_{2}O_{3} + 2A$
$3CSO_{4} + 2B \rightarrow B_{2}(SO_{4})_{3} + 3C$
$3CO + 2A \rightarrow A_{2}O_{3} + 3C$
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$(a)$ Which element is the most reactive?
$(b)$ Which element is the least reactive?
$(c)$ What is the type of reactions listed above?
$A_{2}O_{3} + 2B \rightarrow B_{2}O_{3} + 2A$
$3CSO_{4} + 2B \rightarrow B_{2}(SO_{4})_{3} + 3C$
$3CO + 2A \rightarrow A_{2}O_{3} + 3C$
Answer the following questions with reasons:
$(a)$ Which element is the most reactive?
$(b)$ Which element is the least reactive?
$(c)$ What is the type of reactions listed above?
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View SolutionMetallic oxides of zinc,magnesium,and copper were heated with the following metals. In which cases will you find displacement reactions taking place?
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