A constant current (0.5 amp) is passed for 1 hour through (i) aqueous $A g N O_{3}$ , (ii) aqueous $C u S O_{4}$ and (iii) molten $A l F_{3}$ , separately. The ratio of the mass of the metals deposited on the cathode is:
[ $M_{A g}, M_{C u}, M_{A l}$ are molar masses of the respective metals]

M_{A g} : 2 M_{C u} : 3 M_{A 1}

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M_{A g} : M_{C u} : M_{A 1}

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6 M_{A g} : 3 M_{C u} : 2 M_{A 1}

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3 M_{A g} : 2 M_{C u} : M_{A 1}

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Solution

The correct option is C $6 M_{A g} : 3 M_{C u} : 2 M_{A 1}$

$A g^{+}$ $C u^{2 +}$ $A l^{3 +}$

No. of eq. deposit $x$ $x$ $x$

No. of mol deposit $\frac{x}{1}$ $\frac{x}{2}$ $\frac{x}{3}$

6x 3x 2x

No. of mole deposit 6 3 2

Mass deposit $6 M_{A g}$ $3 M_{C u}$ $2 M_{A l}$

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Similar questions

Q. A constant current(

0.5

amp) is passed for

1

hour through (i) aqueous

A g N O_{3}

, (ii) aqueous

C u S O_{4}

and (iii) molten

A l F_{3}

, separately. The ratio of the mass of the metals deposited on the cathode is? [

M_{A g}, M_{C u}, M_{A l}

are molar masses of the respective metals].

Q. Passage of three faradays of charge through an aqueous solution of

A g N O_{3}, C u S O_{4}, A l (N O_{3})_{3} and N a C l

will deposit metals at the cathode in the molar ratio of :

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 :

965

amp current is passed through molten metal chloride for one minute and

40

seconds during electrolysis. The mass of metal deposited is

9 g m

at the cathode. The valency of metal atom (at.wt

= 27

) is:

One faraday of electricity is passed separately through one litre of one molar aqueous solution of

I) AgNO $_{3}$ , ii) SnCl $_{4}$ and iii) CuSO $_{4}$ .The number of moles of ag, Sn, and Cu deposited at cathode are respectively :

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	$A g^{+}$	$C u^{2 +}$	$A l^{3 +}$
No. of eq. deposit	$x$	$x$	$x$
No. of mol deposit	$\frac{x}{1}$	$\frac{x}{2}$	$\frac{x}{3}$
	6x	3x	2x
No. of mole deposit	6	3	2
Mass deposit	$6 M_{A g}$	$3 M_{C u}$	$2 M_{A l}$

A constant current (0.5 amp) is passed for 1 hour through (i) aqueous AgNO3, (ii) aqueous CuSO4 and (iii) molten AlF3, separately. The ratio of the mass of the metals deposited on the cathode is: [MAg, MCu, MAl are molar masses of the respective metals]

The correct option is C 6MAg:3MCu:2MA1 Ag+ Cu2+ Al3+ No. of eq. deposit x x x No. of mol deposit x1 x2 x3 6x 3x 2x No. of mole deposit 6 3 2 Mass deposit 6MAg 3MCu 2MAl

A constant current (0.5 amp) is passed for 1 hour through (i) aqueous $A g N O_{3}$ , (ii) aqueous $C u S O_{4}$ and (iii) molten $A l F_{3}$ , separately. The ratio of the mass of the metals deposited on the cathode is:
[ $M_{A g}, M_{C u}, M_{A l}$ are molar masses of the respective metals]

The correct option is C $6 M_{A g} : 3 M_{C u} : 2 M_{A 1}$

$A g^{+}$ $C u^{2 +}$ $A l^{3 +}$

No. of eq. deposit $x$ $x$ $x$

No. of mol deposit $\frac{x}{1}$ $\frac{x}{2}$ $\frac{x}{3}$

6x 3x 2x

No. of mole deposit 6 3 2

Mass deposit $6 M_{A g}$ $3 M_{C u}$ $2 M_{A l}$