Question

A student was given two metal strips X and Y alongwith colourless silver nitrate solution to perform two separate displacement reactions. When the student placed metal strip X in silver nitrate solution for a considerable time, he observed that the solution turned blue and a coating of silver metal was formed on the strip. And when the student immersed metal strip Y in silver nitrate solution for an equal time, he observed that the solution turned light green with the formation of a coating of silver metal on the strip. The correct conclusion of the student about the identity of metals X and Y is (1) X is copper and Y is magnesium
(2) X is zinc and Y is copper
(3) X is iron and Y is copper (4) X is copper and Y is iron

Answer 1

Answer:

(4) X is Copper and Y is Iron

Explanation:

It is given that When X reacts with Silver Nitrate, it changes to blue that's why X is copper

It is given that When Y reacts with Silver Nitrate, it changes to light green which is only possible when Y is Iron

Hence X is Copper and Y is Iron

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Answer 2

The correct conclusion of the student about the identity of metals X and Y is that X is copper and Y is iron.

Explanation:

• For X, it gives the blue color solution when silver nitrate is processed with X, which implies that the solution can contain copper.
• Copper is much more reactive than silver, displacing silver from the silver nitrate and producing copper nitrate compound of blue colour.

$Cu(s)+2AgNO_3 (aq)->Cu(NO_3)_2(aq)+2Ag(s)$

• For Y, when silver nitrate is processed with Y, it provides the light green color solution which implies iron may be present in that solution.
• Iron is much more reactive than silver, it will dislodge silver from the silver nitrate and form compound iron nitrate of green colour.

$Fe(s)+AgNO_3 (aq)-> FeNO_3 (aq)+Ag(s)$