A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic masses: Na = 23, Hg = 200, 1 Faraday = 96500 coulombs). The total number of moles of chlorine gas evolved is

Question

A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic masses: Na = 23, Hg = 200, 1 Faraday = 96500 coulombs). The total number of moles of chlorine gas evolved is (A) 0.5 (B) 1.0 (C) 2.0 (D) 3.0

Tardigrade Admin · Accepted Answer

NaCl arrow Na++Cl- At anode: 2Cl- arrow Cl2 Moles of Cl-=2 in 500 ml. Therefore 1 mole of Cl2 evolves.

Q. A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic masses: Na $=$ 23, Hg $=$ 200, 1 Faraday $=$ 96500 coulombs). The total number of moles of chlorine gas evolved is

0.5

1.0

2.0

3.0

$N a Cl \to N a^{+} + C l^{-}$

At anode: $2 C l^{-} \to C l_{2}$

Moles of $C l^{-} = 2$ in 500 ml.

Therefore 1 mole of $C l_{2}$ evolves.

Q. A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic masses: Na = 23, Hg = 200, 1 Faraday = 96500 coulombs). The total number of moles of chlorine gas evolved is

0.5

1.0

2.0

3.0

NaCl→Na++Cl− At anode: 2Cl−→Cl2​ Moles of Cl−=2 in 500 ml. Therefore 1 mole of Cl2​ evolves.

Q. A 4.0 molar aqueous solution of NaCl is prepared and 500 mL of this solution is electrolysed. This leads to the evolution of chlorine gas at one of the electrodes (atomic masses: Na $=$ 23, Hg $=$ 200, 1 Faraday $=$ 96500 coulombs). The total number of moles of chlorine gas evolved is

$N a Cl \to N a^{+} + C l^{-}$

At anode: $2 C l^{-} \to C l_{2}$

Moles of $C l^{-} = 2$ in 500 ml.

Therefore 1 mole of $C l_{2}$ evolves.