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Standard XII

Chemistry

Introduction

In the electr...

Question

In the electrolysis of $A g N O_{3}$ solution 0.7 g of Ag is deposited after a certain period of time. Calculate the quantity of electricity required in coulomb. Molar mass of Ag is $107.9 g m o l^{- 1}$ .

426^{o} C

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536^{o} C

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626^{o} C

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736^{o} C

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Solution

The correct option is C $626^{o} C$
$M a s s D e p o s i t e d = 0.7 g$
$n = 1$
$M o l a r m a s s = 107.9 g m o l^{- 1}$
$m = \frac{A t o m i c M a s s}{n \times F} \times i \times t$
$0.7 = \frac{107.9}{1 \times 96500} \times i \times t$
$\frac{0.7 \times 96500}{107.9} = i \times t$
$i \times t = 626.04 C$
The quantity of electricity required in Coulomb is $626^{o} C$

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Similar questions

Q. In the electroysis of

A g N O_{3}

solution, 0.7 g of Ag is deposited after a certain period of time. Calculate the quantity of electricity required in coulomb. (Molar mass of Ag is 107.9 g mol

^{- 1}

A certain quantity of electricity is passed through an aqueous solution of $A g N O_{3}$ and cupric salt solution connected in series. The amount of silver deposited is 1.08 g. The amount of copper deposited is :

[At.wt. of $C u = 63.54; A g = 108$ ]

Q. When

96.5

coulomb of electricity is passed throught a solution of

A g N O_{3}

, the amount of

A g

deposited is:

Q. A solution of

A g N O_{3}

was electrolysed between silver electrodes. Before electrolysis, 10 g of solution contained 0.01788 g of

A g N O_{3}

. After the experiment, 20.09 g of the anodic solution contained 0.06227 g of

A g N O_{3}

. At the same time, 0.009479 g of Cu was deposited in the copper coulometer placed in series. Calculate transport no. of

A g^{+}

. Write answer to the nearest integer after multiplying transport number calculated with 10.

Q. Calculate the mass of Ag deposited at cathode when a current of 2A was passed through a solution of

A g {N O}_{3}

for 15 min.
(Given : Molar mass of

A g = 108 g {m o l}^{- 1}

1 F = 96500 C {m o l}^{- 1}

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In the electrolysis of AgNO3 solution 0.7 g of Ag is deposited after a certain period of time. Calculate the quantity of electricity required in coulomb. Molar mass of Ag is 107.9gmol−1.

The correct option is C 626oCMass Deposited=0.7 gn=1Molar mass=107.9 gmol−1m=Atomic Massn×F×i×t0.7=107.91×96500×i×t0.7×96500107.9=i×ti×t=626.04 CThe quantity of electricity required in Coulomb is 626 oC

In the electrolysis of $A g N O_{3}$ solution 0.7 g of Ag is deposited after a certain period of time. Calculate the quantity of electricity required in coulomb. Molar mass of Ag is $107.9 g m o l^{- 1}$ .