Question

what is the balanced chemical equation between iron(II) sulphate and sulfuric acid?
A. \[Fe+{{H}_{2}}S{{O}_{4}}\to FeS{{O}_{4}}+{{H}_{2}}\]
B. \[Fe+2{{H}_{2}}S{{O}_{4}}\to 2FeS{{O}_{4}}+{{H}_{2}}\]
C. $Fe+{{H}_{2}}S{{O}_{4}}\to FeS{{O}_{3}}+{{H}_{2}}O$
D.$2Fe+{{H}_{2}}S{{O}_{4}}\to FeS{{O}_{2}}+{{H}_{2}}O$

Answer 1

Hint Metals those are more reactive than hydrogen when added into an acid or base solution or even in water, displaces hydrogen from their compounds and forms with metal salt and along with that hydrogen gas forms. So metals that are more reactive than hydrogen displaces the hydrogen from its compounds.

Complete Step by step solution:
Reactivity series of metals
K
Na
Li
Ca
Mg
Al
Zn
Fe
Sn
Pb
${{H}_{2}}$
All the metals above hydrogen are more reactive than hydrogen, here more reactive than hydrogen means they have a higher tendency to oxidize than hydrogen, so when they are put into acid solutions, they will displace hydrogen and reduction of hydrogen will take place along with oxidation of metal.
Iron is also more reactive than hydrogen, so in acid solutions it will also act the same way.
As we know that sulfate ion has 2- charge over it, so in this reaction iron atom will lose two electrons and will form $F{{e}^{2+}}$which is called as ferrous ion and this ferrous iron will form an ionic bond with sulfate ion in the ratio of 1:1 and name of the compound will be ferrous sulfate.
Both the electrons lost by Fe atom will be gained by two hydrogen ions and these two nascent hydrogen atoms and they will combine together to form hydrogen gas.
Following will be the reaction of Fe with sulfuric acid
\[Fe+{{H}_{2}}S{{O}_{4}}\to FeS{{O}_{4}}+{{H}_{2}}\]
If we compare both sides, both sides iron is equal. Similarly hydrogen, oxygen and sulfur are also equal on both sides. It means this reaction is completely balanced as the number of atoms of each type on the right side is equal to the number of atoms of each type on the left side.
This reaction of Fe with sulfuric acid will be known as displacement reaction.

So correct answer for the question is Option (A)

Additional Information:
This reactivity series is very useful in determining the comparative reactivity of metals. Metal that comes above the other metal is more reactive than that. More reactivity means, high reactive metal can reduce less reactive metal.
We can use this comparative reactivity in metallurgy. For example in extraction of silver, in the solution of the complex of silver formed, we add more reactive zinc metal that displaces silver from its complex.
Highly reactive metals like Al can be used to reduce less reactive metals from its oxides.
Also in electrochemical cells, information of reactivity helps us to decide which metal electrode should be the cathode and which metal electrode should be the anode.
 In corrosion prevention of Iron, galvanization method is used where we apply the coating of more reactive zinc metal on. When moisture arrives with oxygen near an iron object, zinc reacts with moisture before iron because it is more reactive and that’s how it prevents iron from getting corroded.

Note: Always remember that for the acids like $HN{{O}_{3}}$ hydrogen gas doesn’t get liberated when metal more reactive than hydrogen is put into them because$HN{{O}_{3}}$is a very strong oxidizing reagent, so it oxidizes the hydrogen released into water. Only Manganese and Magnesium metals give off hydrogen gas along with very dilute Nitric acid.