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Standard XII

Chemistry

Faraday's First Law

One faraday o...

Question

One faraday of charge was passed through the electrolytic cells placed in series containing solutions of $A g^{+}, N i^{2 +}$ and $C r^{3 +}$ respectively. The amount of $A g$ (At. mass $108), N i$ (At. mass $59$ ) and $C r$ (At. mass $52)$ deposited will be:

A g = 108 g, N i = 29.5 g, C r = 17.5 g

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A g = 108 g, N i = 59.0 g, C r = 52.0 g

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A g = 108 g, N i = 108.0 g, C r = 108.0 g

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A g = 108 g, N i = 117.5 g, C r = 166.0 g

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Solution

The correct option is C $A g = 108 g, N i = 29.5 g, C r = 17.5 g$
When 1 faraday of current was passed through the electrolytic cell then amount deposited will be
For Ag , $w = \frac{108}{1}$ = 108 g

for Ni = $w = \frac{59}{2}$ = 29.5 g

for Cr = $w = \frac{52}{3}$ = $17.3$

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Similar questions

Q. One Faraday of current was passed through the electrolytic cells placed in series containing a solution of

A g^{+}, N i^{2 +}

and

C r^{3 +}

respectively. The ratio of amounts of

A g, N i

and

C r

deposited will be:

[A t . w t .

A g = 108, N i = 59, C r = 52]

Q. One Faraday of current was passed through the electrolytic cell placed in series containing solution of

A g^{+}, N i^{+ +}

and

C r^{+ + +}

respectively. The amounts of

A g

(at. wt. = 108),

N i

(at. wt. = 59) and

C r

(at. wt. = 52) deposited will be:

One Faraday of current was passed through the electrolytic cell placed in series containing solution of Ag $^{+}$ , Ni $^{+}$ , Cr $^{+}$ . the amount of Ag (at.wt.=108), Ni (at.wt.=59) and Cr (at.wt.=52) deposited will be :

Q. On passing one faraday of electricity through the electrolytic cells containing

A g^{+}, N i^{+ 2}

and

C r^{+ 3}

ions solution, the deposited

A g (A t . w t . = 108), N i (A t . w t . = 59) a n d C r (A t . w t . = 52)

\begin{matrix} A g (i n g m) & N i (i n g m) & C r (i n g m) a) & 108 & 59 & 52 b) & 108 & 29.5 & 17.3 c) & 36 & 19.6 & 17.3 d) & 108 & 108 & 108 \end{matrix}

Q. On passing one faraday of electricity through the electrolytic cells containing

A g^{+}, N i^{+ 2}

and

C r^{+ 3}

ions solution, the deposited

A g (A t . w t . = 108), N i (A t . w t . = 59) a n d C r (A t . w t . = 52)

\begin{matrix} A g (i n g m) & N i (i n g m) & C r (i n g m) a) & 108 & 59 & 52 b) & 108 & 29.5 & 17.3 c) & 36 & 19.6 & 17.3 d) & 108 & 108 & 108 \end{matrix}

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One faraday of charge was passed through the electrolytic cells placed in series containing solutions of Ag+,Ni2+ and Cr3+ respectively. The amount of Ag (At. mass 108),Ni (At. mass 59) and Cr (At. mass 52) deposited will be:

The correct option is C Ag=108 g,Ni=29.5 g,Cr=17.5 gWhen 1 faraday of current was passed through the electrolytic cell then amount deposited will beFor Ag , w=1081 = 108 gfor Ni = w=592 = 29.5 gfor Cr = w=523 = 17.3

One faraday of charge was passed through the electrolytic cells placed in series containing solutions of $A g^{+}, N i^{2 +}$ and $C r^{3 +}$ respectively. The amount of $A g$ (At. mass $108), N i$ (At. mass $59$ ) and $C r$ (At. mass $52)$ deposited will be:

The correct option is C $A g = 108 g, N i = 29.5 g, C r = 17.5 g$
When 1 faraday of current was passed through the electrolytic cell then amount deposited will be
For Ag , $w = \frac{108}{1}$ = 108 g

for Ni = $w = \frac{59}{2}$ = 29.5 g

for Cr = $w = \frac{52}{3}$ = $17.3$