Reducing Nature (Group 2)

Q.

During the electrolysis of cupric chloride, the reactions occurring at electrodes are

1. At the anode:
   $C{u}^{2+}+2e^{-}\to Cu\left(s\right)$

2. At the cathode:
   $2C{l}^{-}\to C{l}_2\left(g\right)+2e^{-}$

3. At the cathode:
   $C{u}^{2+}+2e^{-}\to Cu\left(s\right)$

4. At the anode:
   $2C{l}^{-}\to C{l}_2\left(g\right)+2e^{-}$

Q.

Is lithium metal dangerous?

Q.

Given are the reactions occuring during the electrolysis of sodium chloride solution:

$2C{l}^{-}\to C{l}_2+2e^{-}$
$2H_{2}O+2e^{-}\to H_2+2O{H}^{-}$

Which of the following is correct regarding liberation of electrolytic products?

1. Cathode : $Na$ and $H_2$
2. Cathode : $Na$ and $O_2$
3. Anode: $O_2$
4. Anode : $C{l}_2$

Q. When the electrolysis of acidified water is carried out, the equation for the discharge of ions at the cathode is:

1. $2H_{2}O\to O_2+4H^{+}+4e^{-}$
2. $4H_{2}O+4e^{-}\to 2H_2+4O{H}^{-}$
3. $4H_{2}O+4e^{-}\to 4H_2+O_2$
4. $2H_{2}O\to O_2+2H_2$

Q. $Be$ is placed above $Mg$ in the second group. $Be$ dust, therefore when added to $MgC{l}_2$ solution will

1. precipitate Mg metal
2. have no effect
3. lead to dissolution of Be
   
4. precipitate MgO

Q. Mg burns in $C{O}_2$ to form

1. MgO + CO
2. Mgo
3. MgO +C
4. 

Q.

Why are alkali metals kept in kerosene oil?

Q. Which of the following statements is not true regarding alkali metals

1. The alkali metals exhibit only +1 oxidation state
2. The alkali metals have high chemical reactivity
3. The alkali metals die slove in liquid ammonia to give blue coloured solutions
4. Since the alkali metals have good tendency to lose s – electron, they behave as strong oxidizing agents
   

Q. A solution of sodium sulphate in water is electrolysed using inert electrodes. The products at the cathode and anode are respectively
(IIT-JEE, 1987)

1. $H_2,O_2$
2. $O_2,H_2$
3. $O_2,S{O}_3$
4. $O_2,Na$