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Chemistry Part-I

Electrochemistry

Three electrolytic cells A, B, C containing solutions of ZnSO_

Chemistry Part-I

Class 12

NCERT

Chapter 1: The Solid State

31 questions

Chapter 2: Solutions

54 questions

Chapter 3: Electrochemistry

28 questions

A solution of

N i (N O_{3})_{2}

is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

Three electrolytic cells

A, B, C

containing solutions of

Z n S O_{4}, A g N O_{3}

and

C u S O_{3}

, respectively are connected in series. A steady current of

1.5

amperes was passed through them until

1.45 g

of silver deposited at the cathode of cell

B

. How long did the current flow? What mass of copper and zinc were deposited?

Using the standard electrode potentials given in Table

3.1

, predict if the reaction between the following is feasible:
(i)

F e^{3 +} (a q)

and

I^{-} (a q)

(ii)

A g^{+} (a q)

and

C u (s)

(iii)

F e^{3 +} (a q)

and

B r^{-} (a q)

(iv)

A g (s)

and

F e^{3 +} (a q)

(v)

B r_{2} (a q)

and

F e^{2 +} (a q)

View all question

Chapter 4: Chemical Kinetics

40 questions

Chapter 5: Surface Chemistry

27 questions

Chapter 6: General Principles and Processes of Isolation of Elements

30 questions

Chapter 7: The p-Block Elements

62 questions

Chapter 8: The d-and f-Block Elements

48 questions

Chapter 9: Coordination Compounds

38 questions

Question

Medium

Solving time: 3 mins

Three electrolytic cells $A, B, C$ containing solutions of $Z n S O_{4}, A g N O_{3}$ and $C u S O_{3}$ , respectively are connected in series. A steady current of $1.5$ amperes was passed through them until $1.45 g$ of silver deposited at the cathode of cell $B$ . How long did the current flow? What mass of copper and zinc were deposited?

Views: 6,291 students

Updated on: Feb 24, 2024

Book:

Chemistry Part-I (NCERT)

Found 6 tutors discussing this question

Oliver Discussed

Three electrolytic cells

A, B, C

containing solutions of

Z n S O_{4}, A g N O_{3}

and

C u S O_{3}

, respectively are connected in series. A steady current of

1.5

amperes was passed through them until

1.45 g

of silver deposited at the cathode of cell

B

. How long did the current flow? What mass of copper and zinc were deposited?

15 mins ago

Discuss this question LIVE

15 mins ago

Text solutionVerified

Cell

B

A g^{+} + e^{-} ⇌ A g

at cathode.

1

mole (

108

g) of Ag is deposited by

96500

C

1.45

g of Ag will be deposited by

\frac{96500 \times 1.45}{108} = 1295.6 C

.

Now,

Q = I t

1295.6 = 1.5 \times t

t = 864 s

Cell

A

Z n^{2 +} + 2 e^{-} \to Z n

2

moles of electrons (

2 \times 96500

C of current) produces

1

mole (

63.5

g) of zinc.

1295.6

C

of electricity will deposit

\frac{65.3}{2 \times 96500} \times 1295.6 = 0.438

g of zinc

Cell

C

C u^{2 +} + 2 e^{-} \to C u

2

moles of electrons (

2 \times 96500

C

) of current will produce

1

mole (

63.5

g) of

C u

1295.6

C

of current will deposit

\frac{63.5 \times 1295.6}{2 \times 96500} = 0.426 g

of copper

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Practice more questions from Chemistry Part-I (NCERT)

A solution of

N i (N O_{3})_{2}

is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

Three electrolytic cells

A, B, C

containing solutions of

Z n S O_{4}, A g N O_{3}

and

C u S O_{3}

, respectively are connected in series. A steady current of

1.5

amperes was passed through them until

1.45 g

of silver deposited at the cathode of cell

B

. How long did the current flow? What mass of copper and zinc were deposited?

Using the standard electrode potentials given in Table

3.1

, predict if the reaction between the following is feasible:
(i)

F e^{3 +} (a q)

and

I^{-} (a q)

(ii)

A g^{+} (a q)

and

C u (s)

(iii)

F e^{3 +} (a q)

and

B r^{-} (a q)

(iv)

A g (s)

and

F e^{3 +} (a q)

(v)

B r_{2} (a q)

and

F e^{2 +} (a q)

View all

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Question Text	Three electrolytic cells $A, B, C$ containing solutions of $Z n S O_{4}, A g N O_{3}$ and $C u S O_{3}$ , respectively are connected in series. A steady current of $1.5$ amperes was passed through them until $1.45 g$ of silver deposited at the cathode of cell $B$ . How long did the current flow? What mass of copper and zinc were deposited?
Updated On	Feb 24, 2024
Topic	Electrochemistry
Subject	Chemistry
Class	Class 12
Answer Type	Text solution:1 Video solution: 13
Upvotes	1383
Avg. Video Duration	10 min

Text solutionVerified

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