Question

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Q. A small amount of Ferrous sulphate is heated in hard glass tube.

a) Write the balanced chemical reaction involved.

b) Name the type of reaction taking place.​

Answer 1

`a)\ 2FeSO4 \xrightarrow{\text{Heat}} SO_3+SO_2+Fe_2O_3\\b)\ Decomposition\ Reaction`

Step-by-step explanation:

Ferrous Sulphate
`(FeSO4)` is generally found as Lime-Green Crystals. On heating, these crystals almost immediately turn white-yellow. They then, break down to produce an anhydrous mixture of Sulphur Trioxide
`(SO_3)`, Sulphur Dioxide
`(SO_2)` as well as Ferric Oxide
`(Fe_2O_3)`.

We can hence, frame a skeletal equation of this reaction and try to balance it.

Hence,

`FeSO4 \xrightarrow{\text{Heat}} SO_3+SO_2+Fe_2O_3`

Now,

a)In order to balance it through the 'Hit &Trial Method', we'll follow a series of steps:

1. First, lets compare the number of Fe (Iron) atoms on the RHS and LHS. We find that, the no. of Fe Atoms on the RHS is twice the number of Fe Atoms on the LHS. We hence, add a co-effecient 2 beside
`FeSO_4`.

2. Now, Iron atoms, Sulphur Atoms and Oxygen atoms occur 2, 2, 8 respectively on both the sides:

Hence, As all the other elements as well as iron, balance, we've arrived upon our Balanced Equation :

`2FeSO4 \xrightarrow{\text{Heat}} SO_3+SO_2+Fe_2O_3`

b) We know that, decomposition reactions are [generally] endothermic reactions in which Large Compounds decompose into smaller elements and compounds. Here, as Ferrous Sulphate decomposes into Sulphur Dioxide, Sulphur Trioxide and Ferric Oxide, the reaction that occurs here is Decomposition Reaction.