Faraday's Second Law

Q.

A certain current liberated 0.504 gm of hydrogen in 2 hours. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution

1. 12.7 gm

2. 15.9 gm

3. 31.8 gm

4. 63.5 gm

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 $Ag(At.wt.=108),Ni(At.wt.=59)andCr(At.wt.=52)$ is

$\begin{array}{cccc}& Ag\left(ingm\right)& Ni\left(ingm\right)& Cr\left(ingm\right)\\ a)& 108& 59& 52\\ b)& 108& 29.5& 17.3\\ c)& 36& 19.6& 17.3\\ d)& 108& 108& 108\end{array}$

1. d
2. a
3. b
4. c

Q.

A lead storage battery containing 5.0L of $H_{2}S{O}_4$ solution is operated for $9.65\times {10}^{5}s$ with a steady current of 100 mA. Assuming volume of the solution remains constant, normality of $H_{2}S{O}_4$ will :

1. increase by unity

2. increase by 0.20

3. decrease by 0.40

4. remain unchanged

Q. When 0.1 mol $Mn{O}_4^{2-}$ is oxidised, quantity of electricity required to completely oxidise $Mn{O}_4^{2-}$ to $Mn{O}_4^{-}$ is

1. 9650 C
2. 96.50 C
3. 96500 C
4. 2 $\times$ 96500 C

Q. $4.5g$ of aluminum (at. mass 27amu) is deposited at cathode from $A{l}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $H+$ ions in solution by the same quantity of electric charge will be

1. 22.4 L
2. 5.6 L
3. 11.2 L
4. 44.8 L

Q.

In a fuel cell, H2& O2 react to produce electricity. In the process, H2 gas is oxidized at the anode & O2 at the cathode . If 67.2 litre of H2 at STP react in 15 minutes, If the entire current is used for electrode deposition of Cu from Cu (II) solution, how many grams of Cu will be deposited?

1. 190.5 g

2. 160 g

3. 280 g

4. 320 g

Q. The weight of silver (at.wt. = 108) displaced by a quantity of electricity which displaces 5600 mL of $O_2$ at STP will be

1. 10.8 g
2. 54.0 g
3. 108.0 g
4. 5.4 g

Q. Three ampere current was passed through an aqueous solution of an unknown salt of metal M for 1 hour. 2.997 gm of $M^{n+}$ was deposited at cathode. The value of n is (Atomic weight of M = 106.4)

1. 1
2. 2
3. 3
4. 4

Q. $4.5g$ of aluminum (at. mass 27amu) is deposited at cathode from $A{l}^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from $H+$ ions in solution by the same quantity of electric charge will be

1. 11.2 L
2. 5.6 L
3. 22.4 L
4. 44.8 L

Q. When 0.1 mol $Mn{O}_4^{2-}$ is oxidised, quantity of electricity required to completely oxidise $Mn{O}_4^{2-}$ to $Mn{O}_4^{-}$ is

1. 96500 C
2. 2 $\times$ 96500 C
3. 9650 C
4. 96.50 C

Q.

By passing a certain amount of charge through NaCl solution, 9.2 litre of Cl2 were liberated at S.T.P. When the same charge is passed through a nitrate solution of metal M, 7.467 g of the metal was deposited. If the specific heat of metal is 0.216 cal/g, what is formula of metal nitrate ?

1. MNO₃

2. M(NO₃)₂

3. M(NO₃)₃

4. M(NO₃)₄