Chemical Properties of Metals Questions in English

(C) When dilute hydrochloric acid $(HCl)$ is added to iron $(Fe)$ filings,a displacement reaction occurs where iron displaces hydrogen from the acid.
This results in the formation of iron$(II)$ chloride $(FeCl_2)$ and the evolution of hydrogen gas $(H_2)$.
The chemical equation for this reaction is:
$Fe_{(s)} + 2HCl_{(aq)} \to FeCl_{2(aq)} + H_{2(g)} \uparrow$

(N/A) The recovery of silver from silver nitrate solution by copper metal is a displacement reaction. Copper is more reactive than silver,so it displaces silver from its salt solution.
The chemical reaction is:
$2AgNO_{3(aq)} + Cu_{(s)} \to Cu(NO_3)_{2(aq)} + 2Ag_{(s)}$
In this reaction,copper metal displaces silver ions from the silver nitrate solution to form copper$(II)$ nitrate and solid silver.

(A) Sodium $(Na)$ and potassium $(K)$ are highly reactive metals.
They react vigorously and explosively when exposed to air (oxygen) and water (moisture).
If kept in the open,they react with atmospheric oxygen and moisture,which can lead to accidental fires.
Therefore,to prevent these reactions and ensure safety,sodium is stored immersed in kerosene oil,as it does not react with kerosene.

(N/A) $(i)$ $3Fe_{(s)} + 4H_2O_{(g)} \rightarrow Fe_3O_{4(s)} + 4H_{2(g)}$
$(ii)$ Calcium with water: $Ca_{(s)} + 2H_2O_{(l)} \rightarrow Ca(OH)_{2(aq)} + H_{2(g)} + \text{Heat}$
$(iii)$ Potassium with water: $2K_{(s)} + 2H_2O_{(l)} \rightarrow 2KOH_{(aq)} + H_{2(g)} + \text{Heat}$

(N/A) Hydrogen gas $(H_2)$ is evolved when dilute hydrochloric acid $(HCl)$ is added to a reactive metal.
When iron $(Fe)$ reacts with dilute sulphuric acid $(H_2SO_4)$,iron$(II)$ sulphate $(FeSO_4)$ is formed along with the evolution of hydrogen gas $(H_2)$.
The chemical equation is:
$Fe(s) + H_2SO_4(aq) \longrightarrow FeSO_4(aq) + H_2(g)$

(N/A) Alloys are homogeneous mixtures of two or more elements.
The elements can be two metals,or a metal and a non-metal.
An alloy is formed by first melting the primary metal and then dissolving the other elements in it.
For example,$Steel$ is an alloy of $Iron$ and $Carbon$.

(D) displacement reaction occurs when a more reactive metal displaces a less reactive metal from its salt solution.
According to the reactivity series,copper $(Cu)$ is more reactive than silver $(Ag)$.
Therefore,copper can displace silver from silver nitrate $(AgNO_{3})$ solution.
The chemical reaction is: $Cu(s) + 2AgNO_{3}(aq) \rightarrow Cu(NO_{3})_{2}(aq) + 2Ag(s)$.
In the other options,the metal added is less reactive than the metal present in the salt solution,so no displacement reaction will occur.

(C) Food cans are coated with tin instead of zinc because zinc is more reactive than tin.
When food (which often contains organic acids) comes into contact with a zinc coating,the zinc reacts with the acids to form toxic zinc salts,which can contaminate the food.
In contrast,tin is less reactive than zinc and does not react easily with food acids,making it a safer choice for preserving food.

(N/A) Amphoteric oxides are those metal oxides which react with both acids as well as bases to produce salts and water.
These oxides exhibit dual nature,showing both acidic and basic properties.
Examples: Aluminium oxide $(Al_2O_3)$ and Zinc oxide $(ZnO)$.

(N/A) Metals that are more reactive than hydrogen in the reactivity series can displace it from dilute acids. Examples of such metals are $Sodium$ $(Na)$ and $Magnesium$ $(Mg)$.
Metals that are less reactive than hydrogen cannot displace it from dilute acids. Examples of such metals are $Copper$ $(Cu)$ and $Silver$ $(Ag)$.

(B) Non-metals react with oxygen to form acidic oxides.
For example:
${S_{(s)}} + {O_{2(g)}} \to {SO_{2(g)}}$ (which is acidic in nature).
When these oxides are dissolved in water,they form acids. For instance,${SO_2} + H_2O \to H_2SO_3$ (sulfurous acid).

(A)

Metal	Non-metal
Metals are electropositive.	Non-metals are electronegative.
They react with oxygen to form basic oxides. $4Na + O_2 \longrightarrow 2Na_2O$. These typically form ionic bonds.	They react with oxygen to form acidic or neutral oxides. $C + O_2 \longrightarrow CO_2$. These typically form covalent bonds.
They react with water to form oxides or hydroxides and hydrogen gas. $2Na + 2H_2O \longrightarrow 2NaOH + H_2 \uparrow$.	They generally do not react with water.
They react with dilute acids to form salt and hydrogen gas. $2Na + 2HCl \longrightarrow 2NaCl + H_2 \uparrow$.	They do not react with dilute acids as they cannot displace hydrogen.
They act as reducing agents because they easily lose electrons. $Na \longrightarrow Na^+ + e^-$.	They act as oxidizing agents because they gain electrons. $Cl_2 + 2e^- \longrightarrow 2Cl^-$.

(A) The man must have used $Aqua$ $Regia$ to clean the ornaments.
$Aqua$ $Regia$ is a freshly prepared mixture of concentrated $HCl$ and concentrated $HNO_3$ in a $3:1$ ratio.
It is a highly corrosive and fuming liquid capable of dissolving noble metals like gold.
When the gold bangles were dipped in this solution,the outer layer of the gold was dissolved,exposing the fresh,shiny inner layer,which made the bangles look new.
However,because the outer layer of gold was dissolved into the solution,the total weight of the bangles was significantly reduced.

(N/A) Copper does not react with cold water,hot water,or steam.
However,iron reacts with steam.
If the hot water tanks are made of steel (an alloy of iron),the iron present in the steel would react vigorously with the steam formed from the hot water.
$3Fe(s) + 4H_2O(g) \to Fe_3O_4(s) + 4H_2(g)$
This reaction would lead to the corrosion and degradation of the tank.
That is why copper is used to make hot water tanks,and not steel.

(N/A) $Sodium$,$potassium$,and $lithium$ are highly reactive metals that react vigorously with both air and water. To prevent them from coming into contact with atmospheric oxygen and moisture,which could lead to spontaneous combustion or oxidation,they are stored immersed in kerosene oil.

(N/A) Silver $(Ag)$ is less reactive than hydrogen in the reactivity series,so it does not displace hydrogen from dilute $HCl$.
$(b)$ The reaction between aluminium and dilute $HCl$ is exothermic,meaning it releases heat energy,which causes the temperature of the reaction mixture to rise.
$(c)$ Sodium is a highly reactive alkali metal. Its reaction with dilute $HCl$ is extremely exothermic and rapid,releasing a large amount of heat that ignites the hydrogen gas produced,making it highly explosive.
$(d)$ Lead reacts with dilute $HCl$ to form lead$(II)$ chloride and hydrogen gas. The bubbles observed are due to the evolution of hydrogen gas: $Pb(s) + 2HCl(aq) \rightarrow PbCl_2(aq) + H_2(g)$.

(N/A) In the reactivity series of metals,zinc is placed above hydrogen,which means it is more reactive than hydrogen. Therefore,zinc can displace hydrogen from dilute hydrochloric acid to form zinc chloride and hydrogen gas.
$Zn(s) + 2HCl(aq) \longrightarrow ZnCl_2(aq) + H_2(g)$
Conversely,copper is placed below hydrogen in the reactivity series,meaning it is less reactive than hydrogen. Consequently,copper cannot displace hydrogen from dilute hydrochloric acid,and no reaction occurs.
$Cu(s) + HCl(aq) \longrightarrow \text{No reaction}$

(N/A) The reaction of $Zn$ granules with:
$(a)$ Dilute $H_{2}SO_{4}$:
$Zn(s) + H_{2}SO_{4}(aq) \rightarrow ZnSO_{4}(aq) + H_{2}(g)$
$(b)$ Dilute $HCl$:
$Zn(s) + 2HCl(aq) \rightarrow ZnCl_{2}(aq) + H_{2}(g)$
$(c)$ Dilute $HNO_{3}$:
Reaction with dilute $HNO_{3}$ is different compared to other acids because nitric acid is a strong oxidizing agent. It oxidizes the $H_{2}$ gas evolved to $H_{2}O$ and gets reduced itself to nitrogen oxides (like $N_{2}O$,$NO$,or $NO_{2}$ depending on concentration). For very dilute $HNO_{3}$,the reaction is:
$4Zn(s) + 10HNO_{3}(aq) \rightarrow 4Zn(NO_{3})_{2}(aq) + 5H_{2}O(l) + N_{2}O(g)$

(N/A) The reaction of $Zn$ granules with:
$(a)$ $NaCl$ solution:
$Zn(s) + NaCl(aq) \rightarrow$ No reaction.
Zinc is less reactive than sodium,so it cannot displace sodium from its salt solution.
$(b)$ $NaOH$ solution:
$Zn(s) + 2NaOH(aq) \rightarrow Na_2ZnO_2(aq) + H_2(g)$
When zinc reacts with a hot concentrated solution of sodium hydroxide,it forms sodium zincate and releases hydrogen gas.

(A) Aqua regia is a freshly prepared mixture of concentrated hydrochloric acid $(HCl)$ and concentrated nitric acid $(HNO_3)$ in the ratio of $3:1$ respectively.
It is a highly corrosive,fuming liquid that is one of the few reagents capable of dissolving noble metals like gold and platinum.
Gold does not dissolve in either acid alone,but the combination produces nitrosyl chloride $(NOCl)$ and chlorine $(Cl_2)$,which react with gold to form soluble gold chloride $(AuCl_3)$.

(D) The reactivity of metals with water depends on their position in the reactivity series.
$Na$ (Sodium) reacts vigorously with cold water.
$Ca$ (Calcium) reacts with cold water,though less violently than sodium.
$Mg$ (Magnesium) does not react with cold water but reacts with hot water to form magnesium hydroxide and hydrogen gas.
$Fe$ (Iron) does not react with either cold or hot water. However,it reacts with steam to form iron oxide $(Fe_3O_4)$ and hydrogen gas.

(A) When iron reacts with steam (water vapor) for a prolonged period,it forms iron($II$,$III$) oxide and releases hydrogen gas.
The balanced chemical equation for this reaction is:
$3Fe(s) + 4H_{2}O(g) \rightarrow Fe_{3}O_{4}(s) + 4H_{2}(g)$
Thus,the oxide obtained is $Fe_{3}O_{4}$.

(D) $1$. Calcium reacts with water less violently compared to sodium or potassium.
$2$. The chemical reaction is: $Ca(s) + 2H_2O(l) \rightarrow Ca(OH)_2(aq) + H_2(g)$.
$3$. During this reaction, the hydrogen gas produced forms bubbles that stick to the surface of the calcium metal.
$4$. Due to these bubbles, the calcium metal starts floating on the surface of the water.
$5$. Thus, statements $(ii)$ and $(iv)$ are correct. Therefore, the correct option is $D$.

(C) Generally, metals react with dilute acids to produce salt and hydrogen gas $(M + \text{dilute acid} \rightarrow \text{salt} + H_2)$.
However, nitric acid $(HNO_3)$ is a strong oxidizing agent.
When a metal reacts with $HNO_3$, the hydrogen gas produced is oxidized to water $(H_2O)$ by the acid, and the acid itself gets reduced to nitrogen oxides $(N_2O, NO, NO_2)$.
Therefore, $HNO_3$ does not evolve hydrogen gas with most metals.
Exceptions are magnesium $(Mg)$ and manganese $(Mn)$, which react with very dilute nitric acid to evolve hydrogen gas.

(D) Aqua-regia is a freshly prepared mixture of concentrated hydrochloric acid $(HCl)$ and concentrated nitric acid $(HNO_3)$.
It is prepared in the ratio of $3:1$ by volume.
Therefore,the correct composition is $3$ parts of concentrated $HCl$ and $1$ part of concentrated $HNO_3$.

(C) Stainless steel is an alloy of iron.
It is primarily composed of iron $(Fe)$,chromium $(Cr)$,and nickel $(Ni)$.
Chromium is added to provide corrosion resistance,while nickel is added to improve the mechanical properties and durability of the steel.
Therefore,the correct combination is $Ni$ and $Cr$.

(D) According to the reactivity series of metals,the order of reactivity is $Mg > Zn > Cu > Ag$.
$A$ metal higher in the reactivity series can displace a metal lower in the series from its salt solution.
Since $Ag$ (Silver) is the least reactive among the given metals,it will be displaced from its salt solution by all the other three metals ($Mg$,$Zn$,and $Cu$).

(A) The properties described are characteristic of alkali metals.
$1$. Alkali metals like sodium $(Na)$ and potassium $(K)$ are soft enough to be cut with a knife.
$2$. They are highly reactive with oxygen in the air,forming oxides,and are therefore stored under kerosene to prevent contact with air and moisture.
$3$. They react vigorously with water to produce hydrogen gas and metal hydroxides.
$4$. Among the given options,$Na$ (Sodium) fits all these criteria perfectly.

(C) Magnesium $(Mg)$ is a moderately reactive metal.
$1$. It burns in oxygen with a dazzling white flame to form magnesium oxide $(2Mg + O_2 \rightarrow 2MgO)$. This statement is correct.
$2$. Magnesium does not react with cold water. It reacts with hot water to form magnesium hydroxide and hydrogen gas $(Mg + 2H_2O \text{ (hot)} \rightarrow Mg(OH)_2 + H_2)$. This makes option $C$ incorrect because it claims reaction with cold water.
$3$. Magnesium reacts with steam to form magnesium oxide and hydrogen gas $(Mg + H_2O \text{ (steam)} \rightarrow MgO + H_2)$. Note: Option $D$ is also technically incorrect as it states magnesium hydroxide is formed with steam, but option $C$ is the most fundamentally incorrect statement regarding cold water reactivity.

(D) An alloy is a homogeneous mixture of two or more metals,or a metal and a non-metal.
An amalgam is a specific type of alloy where one of the constituents is mercury $(Hg)$.
Among the given options,Zinc amalgam is an alloy of zinc $(Zn)$ and mercury $(Hg)$.
Stainless steel is an alloy of iron,chromium,and nickel.
Alnico is an alloy of aluminum,nickel,and cobalt.
Solder is an alloy of lead $(Pb)$ and tin $(Sn)$.

(C) Most metal oxides are basic in nature because they react with acids to form salt and water.
However,some metal oxides,such as aluminum oxide $(Al_2O_3)$ and zinc oxide $(ZnO)$,show both acidic and basic behavior.
These are known as amphoteric oxides.
They react with both acids and bases to produce salt and water.
Among the given options,$Al$ (Aluminum) forms an amphoteric oxide $(Al_2O_3)$,while $Na$ and $Ca$ form basic oxides,and $Cu$ forms a basic oxide.

(C) chemical reaction will occur if a more reactive metal displaces a less reactive metal from its salt solution.
According to the reactivity series,the order of reactivity is $Mg > Zn > Fe > Pb > Cu$.
In option $C$,$Fe$ is more reactive than $Cu$,so $Fe$ can displace $Cu$ from $CuSO_4$ solution to form $FeSO_4$ and $Cu$.
The reaction is: $Fe(s) + CuSO_4(aq) \rightarrow FeSO_4(aq) + Cu(s)$.
In other options $(A, B, D)$,the metal added is less reactive than the metal present in the salt solution,so no reaction will occur.

(N/A) The produced gas can be identified by bringing a burning matchstick near the mouth of the reaction vessel; it will produce a 'pop' sound,which confirms the presence of hydrogen gas $(H_2)$.
The chemical equation for the reaction with sodium hydroxide is:
$M + 2NaOH \rightarrow Na_2MO_2 + H_2 \uparrow$
The chemical equation for the reaction with hydrochloric acid is:
$M + 2HCl \rightarrow MCl_2 + H_2 \uparrow$
Since the element $M$ reacts with both acids and bases to release hydrogen gas,the element $M$ is an amphoteric metal (such as Zinc).

(B) When metals react with most mineral acids (like $HCl$ or $H_2SO_4$),hydrogen gas $(H_2)$ is evolved.
However,$HNO_3$ (nitric acid) is a very strong oxidising agent.
When a metal reacts with $HNO_3$,the hydrogen gas produced is immediately oxidised to water $(H_2O)$ by the nitric acid.
Consequently,the metal itself gets reduced to its corresponding nitrate salt,and the nitric acid is reduced to nitrogen oxides such as $N_2O$,$NO$,or $NO_2$.

(N/A) The compound $X$ is Iron$(III)$ oxide, represented as $Fe_{2}O_{3}$.
$(b)$ This reaction is known as the Thermite reaction.
$(c)$ The chemical equation for the reaction is:
$Fe_{2}O_{3}(s) + 2Al(s) \rightarrow 2Fe(l) + Al_{2}O_{3}(s) + \text{Heat}$

(A) $1$. Given that the molecular formula of the salt $Y$ is $XOH$ and its molecular mass is $40$.
$2$. The atomic mass of $O$ is $16$ and $H$ is $1$. Therefore, $X + 16 + 1 = 40$, which gives $X = 23$. The element with atomic mass $23$ is Sodium $(Na)$.
$3$. Thus, $X$ is $Na$, $Y$ is $NaOH$, and the gas $Z$ liberated is Hydrogen $(H_2)$, which is highly flammable.
$4$. The balanced chemical equation is: $2Na(s) + 2H_2O(l) \rightarrow 2NaOH(aq) + H_2(g) + \text{Heat energy}$.

(A) The metal $A$ used in the thermite process is Aluminum $(Al)$.
When Aluminum is heated with oxygen,it forms Aluminum oxide $(Al_{2}O_{3})$,which is oxide $B$.
Aluminum oxide is amphoteric,meaning it reacts with both acids and bases.
$A = Al$
$B = Al_{2}O_{3}$
Reaction with $HCl$ (acid):
$Al_{2}O_{3} + 6HCl \rightarrow 2AlCl_{3} + 3H_{2}O$
Reaction with $NaOH$ (base):
$Al_{2}O_{3} + 2NaOH \rightarrow 2NaAlO_{2} + H_{2}O$

(C) The tendency to lose an electron is related to the ionization energy of an element. Elements with high ionization energy do not lose electrons easily.
Fluorine $(F)$ is a highly electronegative non-metal located in Group $17$ of the periodic table.
It has a very small atomic size and a high effective nuclear charge,which holds its valence electrons very tightly.
In contrast,$Na$,$Mg$,and $Al$ are metals that have lower ionization energies and tend to lose electrons to form positive ions ($Na^+$,$Mg^{2+}$,$Al^{3+}$).
Therefore,$F$ has the highest tendency to gain an electron rather than lose one,making it the correct answer.

(A) Non-metals generally form acidic oxides. Non-metals typically have $4$ to $8$ electrons in their outermost shell.
The electronic configurations of the given elements are:
$(a)$ Atomic number $7$: $2, 5$ (Nitrogen)
$(b)$ Atomic number $3$: $2, 1$ (Lithium)
$(c)$ Atomic number $12$: $2, 8, 2$ (Magnesium)
$(d)$ Atomic number $19$: $2, 8, 8, 1$ (Potassium)
Since the element with atomic number $7$ is a non-metal,it forms an acidic oxide. The other three elements $(Li, Mg, K)$ are metals and form basic oxides.

(N/A) Although aluminium is a highly reactive metal,it is resistant to corrosion.
This is because aluminium reacts with oxygen present in the air to form a thin,protective layer of aluminium oxide $(Al_2O_3)$.
This oxide layer is very stable and non-porous,which prevents further oxidation and corrosion of the underlying metal.
Additionally,aluminium is lightweight,durable,and an excellent conductor of heat,making it an ideal material for manufacturing cooking utensils.

(A-D) When solutions are kept in a copper container:
$(a)$ Dilute $HCl$: Copper does not react with dilute $HCl$,so it can be kept.
$(b)$ Dilute $HNO_{3}$: Nitric acid is a strong oxidizing agent and reacts with copper,so it cannot be kept.
$(c)$ $ZnCl_{2}$: Zinc is more reactive than copper,so no displacement reaction occurs; it can be kept.
$(d)$ $H_{2}O$: Copper does not react with water,so it can be kept.
$(B)$ When solutions are kept in an aluminium container:
$(a)$ Dilute $HCl$: Aluminium reacts with dilute $HCl$ to form $AlCl_{3}$ and $H_{2}$ gas,so it cannot be kept. Reaction: $2Al + 6HCl \rightarrow 2AlCl_{3} + 3H_{2}$.
$(b)$ Dilute $HNO_{3}$: Aluminium forms a protective oxide layer $(Al_{2}O_{3})$ with dilute $HNO_{3}$,which prevents further reaction,so it can be kept.
$(c)$ $ZnCl_{2}$: Aluminium is more reactive than zinc and will displace zinc from the solution,so it cannot be kept. Reaction: $2Al + 3ZnCl_{2} \rightarrow 2AlCl_{3} + 3Zn$.
$(d)$ $H_{2}O$: Aluminium does not react with cold or hot water,so it can be kept.

(A) The element $A$ is Calcium $(Ca)$.
When $Ca$ reacts with water,it forms Calcium hydroxide $(Ca(OH)_2)$,which is compound $B$ and is used for white washing.
Reaction: $Ca(s) + 2H_2O(l) \rightarrow Ca(OH)_2(aq) + H_2(g)$
When $Ca(OH)_2$ is heated,it decomposes to form Calcium oxide $(CaO)$,which is oxide $C$.
Reaction: $Ca(OH)_2(s) \xrightarrow{\text{Heat}} CaO(s) + H_2O(g)$
When $CaO$ is treated with water,it gives back $Ca(OH)_2$.
Reaction: $CaO(s) + H_2O(l) \rightarrow Ca(OH)_2(aq)$
Therefore,$A = Ca$,$B = Ca(OH)_2$,and $C = CaO$.

(A) The alkali metal $A$ is Sodium $(Na)$.
When $Na$ reacts with water,it forms Sodium hydroxide $(NaOH)$ as compound $B$.
The molecular mass of $NaOH = 23 + 16 + 1 = 40$.
When $NaOH$ $(B)$ reacts with aluminium oxide $(Al_{2}O_{3})$,it forms Sodium aluminate $(NaAlO_{2})$ as compound $C$,which is soluble in water.
The reactions are:
$2Na + 2H_{2}O \rightarrow 2NaOH + H_{2}$
$Al_{2}O_{3} + 2NaOH \rightarrow 2NaAlO_{2} + H_{2}O$

(N/A) The metal $M$ is Copper $(Cu)$.
Copper is less reactive than hydrogen in the reactivity series,so it does not displace hydrogen from dilute acids.
When copper is heated in the presence of oxygen,it undergoes oxidation to form Copper$(II)$ oxide $(CuO)$,which is a black-coloured substance.
The chemical reaction is:
$2Cu(s) + O_2(g) \rightarrow 2CuO(s)$ (Black product)

(N/A) $Fe$ is more reactive than $Cu$. According to the reactivity series,$Fe$ can displace $Cu$ from its salt solution.
When $CuSO_{4}$ solution is kept in an iron pot,$Fe$ reacts with $CuSO_{4}$ to form $FeSO_{4}$ and $Cu$ is deposited.
This reaction causes the iron pot to corrode,leading to the formation of holes.
The chemical equation for this displacement reaction is:
$Fe(s) + CuSO_{4}(aq) \rightarrow FeSO_{4}(aq) + Cu(s)$

(A) $X$ is an alkali metal,such as $Na$ or $K$,which is highly reactive and reacts with cold water.
$Y$ is an alkaline earth metal,such as $Mg$ or $Ca$,which reacts with hot water.
$Z$ is a metal like $Fe$ (iron),which reacts only with steam.
The order of increasing reactivity is $Z < Y < X$,which corresponds to $Fe < Mg < Na$.

(A) Metal oxides that react with both acids and bases to produce salt and water are called Amphoteric oxides. Examples include $Al_2O_3$ and $ZnO$.
$(b)$ Although most non-metals are dull,Iodine is an exception as it possesses a metallic sheen or luster,hence it is described as Lustrous.

(N/A) When steam is passed over hot aluminium,it reacts to form aluminium oxide and hydrogen gas.
The balanced chemical equation for this reaction is:
$2Al(s) + 3H_2O(g) \rightarrow Al_2O_3(s) + 3H_2(g) \uparrow$
In this reaction,aluminium metal reacts with steam (gaseous water) at high temperatures to produce aluminium oxide and hydrogen gas.

(N/A) The given reaction is a displacement reaction.
$(i)$ Metal $X$ is more reactive than metal $Y$.
$(ii)$ Metal $X$ is displacing metal $Y$ from its salt solution. According to the reactivity series,a more reactive metal displaces a less reactive metal from its salt solution. Therefore,$X$ is more reactive than $Y$.

(N/A) Aluminium is more reactive than iron. Therefore,it displaces iron from the ferrous sulphate solution in a displacement reaction.
The chemical reaction is as follows:
$2Al(s) + 3FeSO_4(aq) \to Al_2(SO_4)_3(aq) + 3Fe(s)$
Due to this reaction,the aluminium metal of the can is consumed to form aluminium sulphate,which leads to the formation of holes in the can.