Write the balanced chemical equation for each of the following cases:
$(a)$ Magnesium is treated with very dilute $HNO_3$.
$(b)$ Aluminium powder is added to $Fe_2O_3$.
$(c)$ Zinc sulphide is roasted.
$(a)$ Magnesium is treated with very dilute $HNO_3$.
$(b)$ Aluminium powder is added to $Fe_2O_3$.
$(c)$ Zinc sulphide is roasted.
(N/A) Magnesium reacts with very dilute nitric acid to produce magnesium nitrate and hydrogen gas:
$Mg(s) + 2HNO_3(aq) \longrightarrow Mg(NO_3)_2(aq) + H_2(g)$
$(b)$ Aluminium powder reacts with iron$(III)$ oxide in a thermite reaction to produce iron and aluminium oxide:
$Fe_2O_3(s) + 2Al(s) \longrightarrow 2Fe(l) + Al_2O_3(s) + \text{Heat}$
$(c)$ Zinc sulphide is roasted in the presence of oxygen to produce zinc oxide and sulphur dioxide gas:
$2ZnS(s) + 3O_2(g) \xrightarrow{\Delta} 2ZnO(s) + 2SO_2(g)$
$Mg(s) + 2HNO_3(aq) \longrightarrow Mg(NO_3)_2(aq) + H_2(g)$
$(b)$ Aluminium powder reacts with iron$(III)$ oxide in a thermite reaction to produce iron and aluminium oxide:
$Fe_2O_3(s) + 2Al(s) \longrightarrow 2Fe(l) + Al_2O_3(s) + \text{Heat}$
$(c)$ Zinc sulphide is roasted in the presence of oxygen to produce zinc oxide and sulphur dioxide gas:
$2ZnS(s) + 3O_2(g) \xrightarrow{\Delta} 2ZnO(s) + 2SO_2(g)$
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Give reasons for the following:
$(i)$ Alloys are used in electrical heating devices rather than pure metals.
$(ii)$ Gold ornaments look new even after several years of use.
$(iii)$ An iron grill should be painted frequently.
$(i)$ Alloys are used in electrical heating devices rather than pure metals.
$(ii)$ Gold ornaments look new even after several years of use.
$(iii)$ An iron grill should be painted frequently.
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$(i)$ Metals are good conductors of heat.
$(ii)$ Addition of some silver to pure gold for making ornaments.
$(iii)$ Inability of non-metals to displace hydrogen from dilute sulphuric acid.
$(i)$ Metals are good conductors of heat.
$(ii)$ Addition of some silver to pure gold for making ornaments.
$(iii)$ Inability of non-metals to displace hydrogen from dilute sulphuric acid.
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View SolutionSamples of four metals $A$,$B$,$C$ and $D$ were taken and added to the following solutions one by one. The results obtained have been tabulated as follows.
Metal Iron $(II)$ sulphate Copper $(II)$ sulphate Zinc sulphate Silver nitrate $A$ No reaction Displacement No reaction Displacement $B$ Displacement Displacement No reaction Displacement $C$ No reaction No reaction No reaction Displacement $D$ No reaction No reaction No reaction No reaction
Use the table above to answer the following questions about metals $A$,$B$,$C$ and $D$:
$(i)$ Which is the most reactive metal?
$(ii)$ What would you observe if $B$ is added to a solution of Copper $(II)$ sulphate?
$(iii)$ Arrange the metals $A$,$B$,$C$ and $D$ in the order of decreasing reactivity.
| Metal | Iron $(II)$ sulphate | Copper $(II)$ sulphate | Zinc sulphate | Silver nitrate |
| $A$ | No reaction | Displacement | No reaction | Displacement |
| $B$ | Displacement | Displacement | No reaction | Displacement |
| $C$ | No reaction | No reaction | No reaction | Displacement |
| $D$ | No reaction | No reaction | No reaction | No reaction |
Use the table above to answer the following questions about metals $A$,$B$,$C$ and $D$:
$(i)$ Which is the most reactive metal?
$(ii)$ What would you observe if $B$ is added to a solution of Copper $(II)$ sulphate?
$(iii)$ Arrange the metals $A$,$B$,$C$ and $D$ in the order of decreasing reactivity.
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