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Byju's Answer

Standard XII

Chemistry

Electrochemical Cells, Galvanic Cells

Some equipmen...

Question

Some equipments and materials are given.
$Z n {S O}_{4}$ solution, $C u {S O}_{4}$ solution, $Z n$ rod, $C u$ rod, Voltmeter, $K C l$ solution, filter paper.
(a) Draw the diagram of the electrochemical cell which can be constructed using these equipments and materials and label the pans.
(b) Write equations of chemical reactions taking place in the two electrodes of this cell.
(Hint: reactivity $Z n > C u$ )

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Solution

(a) Electrochemical cell
(b) Reaction at the anode:
${Z n}_{(s)} + 2 e^{-} \to {Z n}^{2 +}$
Reaction at the cathode:
${C u}^{2 +} + 2 e^{-} \to {C u}_{(s)}$
Over all reaction:
${Z n}_{(s)} + {C u}^{2 +} \to {Z n}^{2 +} + {C u}_{(s)}$

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Similar questions

Q. Construct the cells in which the following reactions are taking place. Which of the electrodes shall act as anode (negative electrode) and which one as cathode (positive electrode)?
(a)

Z n + C u S O_{4} = Z n S O_{4} + C u

(b)

C u + 2 A g N O_{3} = C u (N O_{3})_{2} + 2 A g

(c)

Z n + H_{2} S O_{4} = Z n S O_{4} + H_{2}

(d)

F e + S n C l_{2} = F e C l_{2} + S n

Q. You are supplied with the following substances:
Copper rod, Zinc rod, Salt bridge, two glass beakers, a piece of wire,

1

M

C u S O_{4}

solution,

1

M

Z n S O_{4}

solution.
(a) Represent the cell made using the above materials.
(b) (i) Write the Nernst equation for the above cell.
(ii) Calculate the standard EMF of the cell if

E_{({Z n}^{2 +} / Z n)}^{o} = - 0.76 V

E_{({C u}^{2 +} / C u)}^{o} = + 0.34 V

Q. Chemical equation for the reaction between

C u S O_{4}

solution and an iron nail is given below.

C u S O_{4} + F e \to F e S O_{4} + C u

(a) Write the reduction reaction taking place here.
(b) Give reason for the displacement of Cu by Fe from

C u S O_{4}

solution.

The SRP values of Zn, Ag, Ni and Cu electrodes are -0.76V, 0.80V, 0.25V and 0.34V respectively in which container $C u S O_{4}$ solution should be stored:

Q. An electrochemical cell is constructed by immersing a piece of copper wire in 50 ml of 0.1 M

C u S O_{4}

solution and zinc strip in 50 ml of 0.1 M

Z n S O_{4}

solution
[

E_{C u^{2 +} / C u}^{0}

= 0.34 V,

E_{Z n^{2 +} / Z n}^{0}

= -0.76 V ]

The emf of the cell increases when small amount of concentrated

N H_{3}

is added to:

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(a) Electrochemical cell(b) Reaction at the anode:Zn(s)+2e−→Zn2+Reaction at the cathode:Cu2++2e−→Cu(s)Over all reaction:Zn(s)+Cu2+→Zn2++Cu(s)

(a) Electrochemical cell
(b) Reaction at the anode:
${Z n}_{(s)} + 2 e^{-} \to {Z n}^{2 +}$
Reaction at the cathode:
${C u}^{2 +} + 2 e^{-} \to {C u}_{(s)}$
Over all reaction:
${Z n}_{(s)} + {C u}^{2 +} \to {Z n}^{2 +} + {C u}_{(s)}$