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Preparation of Sodium Hydroxide

Consider the ...

Question

Consider the following reactions:
I. $2 N a + 2 H_{2} O \to 2 N a O H + H_{2}$
II. $2 N a O H + C l_{2} \to N a C l + N a O C l + H_{2} O$
III. $4 O H^{-} \to O_{2} + 2 H_{2} O + 4 e^{-}$
IV. $2 C l^{-} \to C l_{2} + 2 e^{-}$
In the diaphragm cell used for the electrolysis of brine, the reactions that occur would include :

A

2,3,4

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B

1,3,4

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C

1,2,3

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D

1,2,4

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Solution

The correct option is A 1,3,4
In the diaphragm cell process, there are two compartments separated by a permeable diaphragm, often made of asbestos fibres. Brine is introduced into the anode compartment and flows into the cathode compartment. Similar to the membrane cell, chloride ions are oxidized at the anode to produce chlorine, and at the cathode, water is split into caustic soda and hydrogen. The diaphragm prevents the reaction of the caustic soda with the chlorine. Reactions involved in the electrolysis are:
$2 N a + 2 H_{2} O \to 2 N a O H + H_{2}$
$2 N a O H + C l_{2} \to N a C l + N a O C l + H_{2} O$
$2 C l^{-} \to C l_{2} + 2 e^{-}$

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Similar questions

Q. In the electrolysis of aqueous

N a C l

solution, side reactions taking place are :

2 O H^{-} + C l_{2} \to 2 O C l^{-} + H_{2} O

2 N a + 2 H_{2} O \to 2 N a O H + H_{2}

4 O H^{-} \to O_{2} + 2 H_{2} + 4 e^{-}

Select the correct alternate :

Q. Consider the table of standard reduction potentials shown below.

Half-reaction	$E^{\circ}$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36 V$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23 V$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83$
$R b^{+} + e^{-} \to R b$	$- 2.93 V$

Use the following from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when a molten rubidium chloride undergoes electrolysis.

Q. Consider the table of standard reduction potentials shown below.

Half-reaction	$E^{\circ}$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36 V$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23 V$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83 V$
$R b^{+} + e^{-} \to R b$	$- 2.93 V$

Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis.

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

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

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

N a O H

can be prepared by two methods each with two steps having

100 %

I

2 N a + 2 H_{2} O ⟶ 2 N a O H + H_{2}

2 H_{2} + O_{2} ⟶ 2 H_{2} O

I I

2 N a + \frac{1}{2} O_{2} ⟶ N a_{2} O

N a_{2} O + H_{2} O ⟶ 2 N a O H

Which gives better yield?

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