Question

Two beakers A and B contain Iron (II) sulphate solution. In the beaker A a small piece of copper is placed and in the beaker B a small piece of zinc is placed. It is found that a grey deposit forms on the zinc but not on the copper. From these observations, it can be concluded. *
1 point
(a) Zinc is most reactive metal followed by iron and then copper.
(b) Zinc is most reactive metal followed by copper and then iron.
(c) Iron is most reactive metal followed by zinc and then copper.
(d) Iron is most reactive metal followed by copper and then zinc​

Answer 1

Explanation:

Zinc is most reactive metal followed by copper and then iron.

(c) Iron is most reactive metal followed by zinc and then copper.

(d) Iron is most reactive metal followed by copper and then zin only ok it is your specific answer

Answer 2

Answer: The correct answer is (a); Zinc is most reactive metal followed by iron and then copper.

Explanation:

• When a more reactive element displaces less element from its salt solution, the chemical reaction is known as displacement reaction.

• In Beaker A, containing Iron (II) Sulphate solution and copper, no deposit is found as copper is less reactive than iron, so it cannot displace iron from its solution. Therefore no reaction takes place.

• But in beaker B containing Iron (II) Sulphate solution and zinc, grey deposit is found on its surface. It is due to the reason that more reactive zinc can displace iron from its solution as:

          $FeSO_{4} (aq) + Zn (s)$  → $ZnSO_{4} (aq) + Fe (s)$

Therefore correct answer is option (a).

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