Question

Электролиз растворов 1)NH4OH 2)FeBr2 3)Co(NO3)3 4)AgSO4

Answer 1

1)Нет
2)FeBr2:
2FeBr2+2H2O---эл. ток-->Fe+H2+2Br2+Fe(OH)2
(-)K: 2H2O+2e=H2+2OH(-)
Fe(+2)+2e=Fe(0)
(+)A: 2Br(-)-2e=Br2
3)2Со (2+) + 2Н2О = 2Со↓ + 4Н (+) + О2↑ (либо 2Co(NO3)2 + 2H2O = 2Со↓ + 4НNO3 + О2↑ (1)
4)MgSO4 + H2O = H2 +O2 + Mg(OH)2 + H2SO4
MgSO4 = Mg2+ + SO4-

Answer 2

Electrolysis of NH4OH (Ammonium Hydroxide) Solution

Electrolysis is the process of using an electric current to drive a non-spontaneous chemical reaction. When an aqueous solution of NH4OH (ammonium hydroxide) is electrolyzed, it undergoes various reactions at the electrodes.

At the anode (positive electrode), water molecules are oxidized to produce oxygen gas and protons (H+ ions). The protons can then react with the ammonium ions (NH4+) present in the solution to form ammonia gas (NH3) and water.

At the cathode (negative electrode), water molecules are reduced to produce hydrogen gas and hydroxide ions (OH-). The hydroxide ions can then react with the ammonium ions (NH4+) present in the solution to form water and ammonia gas.

The overall reaction can be represented as follows:

Anode: 2H2O(l) -> O2(g) + 4H+(aq) + 4e-

Cathode: 4H2O(l) + 4e- -> 2H2(g) + 4OH-(aq)

Overall reaction: 2NH4OH(l) -> NH3(g) + H2O(l)

Electrolysis of FeBr2 (Iron(II) Bromide) Solution

When an aqueous solution of FeBr2 (iron(II) bromide) is electrolyzed, it undergoes various reactions at the electrodes.

At the anode (positive electrode), bromide ions (Br-) are oxidized to produce bromine gas (Br2). The iron(II) ions (Fe2+) present in the solution can also be oxidized to form iron(III) ions (Fe3+).

At the cathode (negative electrode), water molecules are reduced to produce hydrogen gas and hydroxide ions (OH-). The iron(II) ions (Fe2+) present in the solution can also be reduced to form iron metal (Fe).

The overall reaction can be represented as follows:

Anode: 2Br-(aq) -> Br2(g) + 2e-

Cathode: 2H2O(l) + 2e- -> H2(g) + 2OH-(aq)

Overall reaction: 2FeBr2(l) -> 2Fe(s) + Br2(g)

Electrolysis of Co(NO3)3 (Cobalt(III) Nitrate) Solution

When an aqueous solution of Co(NO3)3 (cobalt(III) nitrate) is electrolyzed, it undergoes various reactions at the electrodes.

At the anode (positive electrode), nitrate ions (NO3-) are oxidized to produce oxygen gas and nitrogen dioxide gas (NO2). The cobalt(III) ions (Co3+) present in the solution can also be oxidized to form cobalt(IV) ions (Co4+).

At the cathode (negative electrode), water molecules are reduced to produce hydrogen gas and hydroxide ions (OH-). The cobalt(III) ions (Co3+) present in the solution can also be reduced to form cobalt metal (Co).

The overall reaction can be represented as follows:

Anode: 2NO3-(aq) -> O2(g) + 2NO2(g) + 2e-

Cathode: 2H2O(l) + 2e- -> H2(g) + 2OH-(aq)

Overall reaction: 2Co(NO3)3(l) -> 2Co(s) + 6NO2(g) + O2(g)

Electrolysis of AgSO4 (Silver Sulfate) Solution

When an aqueous solution of AgSO4 (silver sulfate) is electrolyzed, it undergoes various reactions at the electrodes.

At the anode (positive electrode), sulfate ions (SO4^2-) are oxidized to produce oxygen gas and sulfur dioxide gas (SO2). The silver ions (Ag+) present in the solution can also be oxidized to form silver metal (Ag).

At the cathode (negative electrode), water molecules are reduced to produce hydrogen gas and hydroxide ions (OH-). The silver ions (Ag+) present in the solution can also be reduced to form silver metal (Ag).

The overall reaction can be represented as follows:

Anode: 2SO4^2-(aq) -> O2(g) + 2SO2(g) + 4e-

Cathode: 2H2O(l) + 4e- -> 2H2(g) + 4OH-(aq)

Overall reaction: 2AgSO4(l) -> 2Ag(s) + O2(g) + 2SO2(g)

Please note that the reactions mentioned above are simplified representations of the electrolysis process and may not take into account all possible side reactions or variations in experimental conditions.