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Standard XII

Chemistry

Charge and Current

ntA certain q...

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ntA certain quantity of electricity is passed through an aqueous solutions of AgNO3 and CuSO4 connected in series. IF the mass of Ag deposited is 1.08 g , the mass of Cu deposited will be ?n

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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. A certain quantity of electricity is passed through aqueous

A l_{2} (S O_{4})_{3}

and

C u S O_{4}

solutions connected in series

0.09

g of Al is deposited on cathode during electrolysis. The amount of copper deposited on cathode in grams is:

(At. wt of Al

= 27;

= 63.6

)

Q. When same quantity of electricity is passed through aqueous

A g N O_{3}

and

H_{2} S O_{4}

solutions connected in series,

5.04 \times 10^{- 2} g

H_{2}

is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen

= 1.008

, silver

= 108

)

When same quantity of electricity is passed through $A g N O_{3}$ and $H_{2} S O_{4}$ solution connected in series 5.04 $\times 10^{- 2}$ g of $H_{2}$ is liberated. Calculate the mass of silver deposited:

Q. Some quantity of electricity was passed through two cells, one containing

H C l

and the other

A g {N O}_{3}

solution. What volume of

H_{2}

will be liberated at NTP, if

1.08 \times 10^{- 4} k g

of Ag got deposited at the other electrode?
(Molar mass of

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

H = 1 g {m o l}^{- 1}

)

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