If the aqueous solutions of the following salts are electrolyzed for 1 hour with 10 ampere current- which solution will deposit the maximum mass of the metal at the cathode- The atomic weights are- Fe - 56-Zn - 65- Ag - 108- nbsp-Hf - 178 and W - 184-a- ZnSO4 nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- -b- FeCl3 nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- -c- AgNO3 nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- -d- WCl6

Dear Student, The computation are expressed below, Given:t=1 #160;hr #160;= #160;3600 #160;sI #160;= #160;10 #160;A10 #160;A #160;= #160;1 ...

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Byju's Answer

Standard XII

Chemistry

Charge and Current

If the aqueou...

Question

If the aqueous solutions of the following salts are electrolyzed for 1 hour with 10 ampere current, which solution will deposit the maximum mass of the metal at the cathode? The atomic weights are, Fe = 56.Zn = 65, Ag = 108. Hf = 178 and W = 184
(a) ZnSO₄ (b) FeCl₃ (c) AgNO₃ (d) WCl₆

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Solution

Dear Student,

The computation are expressed below,

$G i v e n : t = 1 h r = 3600 s I = 10 A 10 A = 10 \frac{C}{s} 10 \frac{C}{s} \times 3600 s = 36000 C m o l e s o f e l e c t r o n f o r 36000 C i s, \frac{36000 C}{96485.309 \frac{C}{m o l o f e^{-}}} = 0.373 m o l o f e^{-} T h e m a x i m u m d e p o s i t e d m e t a l i s A g N O_{3} (108 \times 0.373 = 2.68 g m)$
Regards

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Similar questions

Q. If the aqueous solutions of the following salts

A g N O_{3}, F e C l_{3}, H f C l_{4}, Z n S O_{4}

are electrolysed for 1 hour with

10

ampere current, which solution will deposit the maximum mass of the metal at cathode?
The atomic weights are:

F e = 56 u, Z n = 65 u, A g = 108 u, H f = 178 u

Q. If the aqueous solutions of the following salts are electrolysed for

1

hour with

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ampere current, which solution will deposit the maximum mass of the metal at cathode? The atomic weights are:

F e = 56, Z n = 65, A g = 108, H f = 178

and

W = 184

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A g

(atomic mass

= 108

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0.5 a m p

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A solution of

C u S O_{4}

is electrolyzed for

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minutes with a current of

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. What is the mass of copper deposited at the cathode?

[Atomic weight of copper =

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The amount of Ag (atomic mass = 108) deposited at the cathode when a current of 0.5 amp is passed through a solution of AgNO $_{3}$ for 1 hour is closest to :

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If the aqueous solutions of the following salts are electrolyzed for 1 hour with 10 ampere current, which solution will deposit the maximum mass of the metal at the cathode? The atomic weights are, Fe = 56.Zn = 65, Ag = 108. Hf = 178 and W = 184 (a) ZnSO4 (b) FeCl3 (c) AgNO3 (d) WCl6

Dear Student, The computation are expressed below, Given:t=1 hr = 3600 sI = 10 A10 A = 10 Cs10Cs×3600 s = 36000 Cmoles of electron for 36000 C is,36000 C96485.309 Cmol of e-=0.373 mol of e-The maximum deposited metal is AgNO3 (108×0.373=2.68 gm) Regards

If the aqueous solutions of the following salts are electrolyzed for 1 hour with 10 ampere current, which solution will deposit the maximum mass of the metal at the cathode? The atomic weights are, Fe = 56.Zn = 65, Ag = 108. Hf = 178 and W = 184
(a) ZnSO₄ (b) FeCl₃ (c) AgNO₃ (d) WCl₆