Question

A student adds an equal amount of copper sulphate solution in two beakers. He adds zinc in beaker P and silver in beaker Q. The student observes that the color of the solution in beaker P changes while no change is observed in beaker Q. Which option arranges the metals in increasing order of reactivity? *
silver-zinc-copper
zinc-copper- silver
silver-copper-zinc
copper-silver-zinc

Answer 1

Answer:

option b is the correct one

zinc-copper-silver .

please mark it as a brainlist answer

thank you all .

Answer 2

The metals in increasing order of reactivity are $\[silver < copper < zinc\]$.

Explanation:

• Both the beakers P and Q contain copper sulphate solution in equal amounts.
• When zinc is added to beaker P, it displaces copper from copper sulphate to form zinc sulphate and copper. Therefore, the colour of the solution changes.
• The reaction is given as: $\[Zn + CuS{O_4} \to ZnS{O_4} + Cu\]$
• This happens because zinc is more reactive than copper according to the reactivity series.
• On the other hand, when silver is added to beaker Q, no reaction takes place. Therefore, no change is observed in beaker Q.
• This is because silver is less reactive than copper according to the reactivity series.
• Thus, the increasing order of the reactivity of metals can be given as:

        $\[silver < copper < zinc\]$