When an aqueous solution of CuCl2 is electrolysed using Pt inert electrodes, the reaction at cathode and anode respectively are

Question

When an aqueous solution of CuCl2 is electrolysed using Pt inert electrodes, the reaction at cathode and anode respectively are (A) 4 H 2 O (l) stackrel+4 e- longrightarrow 2 H 2( g )+ 4 overline O H 2( aq ); 2 H 2 O (l) stackrel-4 e- longrightarrow O 2(g)+4 H +(a q) (B) 2 Cu 2+( aq ) stackrel+4 e- longrightarrow 2 Cu ( s ); 2 H 2 O (l) stackrel-4 e- longrightarrow O 2(g)+4 H +( aq ) (C) Cu 2+( aq ) stackrel+2 e - longrightarrow Cu ( s ) ; 2 Cl -( aq ) stackrel-2 e - longrightarrow Cl 2(g) (D) 2 H 2 O (l) stackrel+2 e- longrightarrow H 2(g)+2 overline O H ( aq ); 2 Cl -( aq ) stackrel-2 e - longrightarrow Cl 2( g )

Tardigrade Admin · Accepted Answer

CuCl 2 longrightarrow Cu 2+(a q)+2 Cl -(a q) Cl - show oxidation at anode and form Cl 2 gas. 2 Cl - stackrel-2 e- longrightarrow Cl 2(g) Due to less reactivity, Cu 2+ gain electrons and deposited at cathode electrode. Cu 2++2 e- longrightarrow Cu

Q. When an aqueous solution of $CuCl X_{2}$ is electrolysed using Pt inert electrodes, the reaction at cathode and anode respectively are

$4 H_{2} O (l) ⟶ + 4 e^{-} 2 H_{2} (g) + 4 \overline{O} H_{2} (a q); 2 H_{2} O (l) ⟶ - 4 e^{-} O_{2} (g) + 4 H^{+} (a q)$

$2 C u^{2 +} (a q) ⟶ + 4 e^{-} 2 C u (s); 2 H_{2} O (l) ⟶ - 4 e^{-} O_{2} (g) + 4 H^{+} (a q)$

$C u^{2 +} (a q) ⟶ + 2 e^{-} C u (s); 2 C l^{-} (a q) ⟶ - 2 e^{-} C l_{2} (g)$

$2 H_{2} O (l) ⟶ + 2 e^{-} H_{2} (g) + 2 \overline{O} H (a q);$ $2 C l^{-} (a q) ⟶ - 2 e^{-} C l_{2} (g)$

$C u C l_{2} ⟶ C u^{2 +} (a q) + 2 C l^{-} (a q)$

$C l^{-}$ show oxidation at anode and form $C l_{2}$ gas.

$2 C l^{-} ⟶ - 2 e^{-} C l_{2} (g)$

Due to less reactivity, $C u^{2 +}$ gain electrons and deposited at cathode electrode.

$C u^{2 +} + 2 e^{-} ⟶ C u$

Q. When an aqueous solution of CuClX2​ is electrolysed using Pt inert electrodes, the reaction at cathode and anode respectively are

4H2​O(l)⟶+4e−​2H2​(g)+4OH2​(aq);2H2​O(l)⟶−4e−​O2​(g)+4H+(aq)

2Cu2+(aq)⟶+4e−​2Cu(s);2H2​O(l)⟶−4e−​O2​(g)+4H+(aq)

Cu2+(aq)⟶+2e−​Cu(s);2Cl−(aq)⟶−2e−​Cl2​(g)

2H2​O(l)⟶+2e−​H2​(g)+2OH(aq); 2Cl−(aq)⟶−2e−​Cl2​(g)