Chemical Industry Titanium Electrolyzer for Producing Sodium Chlorate NaClO3

Product Overview

Description

Mono-polar Electrolyzer

 

Model	FG-II20-B	FG-II25-B		FG-II30-B		FG-II60-B	FG-II80-B	FG-II120-B
Electrolytic Area	10M2	12.5M2		15M2		30M2	40M2	60 M2
Anode Material	Noble Metal Oxide Coating+ High Purity Titanium
Cathode Material	Extreme Low Carbon Steel
Design Current Density	2200-2500A/M2
Inter-electrode Distance	2.5mm~3mm
Anode Material	Quintuple Noble Metal Nano-structured Coating
Anode Service Life	>6 Years	>6Years		>6Years		>6Years	>6Years	>6Years
Oxygen Content	<3%	<3%		<3%		<3%	<3%	<3%
Current Efficiency	>92%(Secondary Refined Brine)
Shell Material	Carbon Steel, Titanium
Chlorates Output	110MT/Year		130MT/Year		160MT/Year	300MT/Year	400MT/Year	600MT/Year
DC Power Consumption	<5000KW/MT
Working Temperature	80°C~85°C

 

Name: Chemical Industry Titanium Sodium Chlorate Electrolytic Cell

Item No.: EL-001

 

Specifications:

Technical parameters:

Anode coating for chlorates:

Electrolyte: NaCl 100-130g/L+HCL+NaCLO3

Current density: 2000-2500A/M2

Temperature: 80-90°C

Service life: >6years

Ph value: 5.5-6.5

Main components: RuO2+IrO2+TiO2+SnO2+X

 

Features:

1. Electrolyzers for producing sodium chlorate and potassium chlorate.

2. Low consumption power.

3. High working efficiency.

 

Application:

Electrochemistry.

1. Effluent treatment

2. Organic electrosynthesis

3. Oxidant production and regeneration such as perchloride, iodate, chromic anhydride and persulphate etc.

4. Industrial electroplating such as Zn and Cr plating etc.

 

Introduction:

An electrolytic cell decomposes chemical compounds by means of electrical energy, in a process called electrolysis; the Greek word lysis means to break up. The result is that the chemical energy is increased. Important examples of electrolysis are the decomposition of water into hydrogen and oxygen, and bauxite into aluminum and other chemicals.

An electrolytic cell has three component parts: an electrolyte and two electrodes (a cathode and an anode). The electrolyte is usually a solution of water or other solvents in which ions are dissolved. Molten salts such as sodium chloride are also electrolytes. When driven by an external voltage applied to the electrodes, the electrolyte provides ions that flow to and from the electrodes, where charge-transferring, or faradaic, or redox, reactions can take place. Only for an external electrical potential (i.e. voltage) of the correct polarity and large enough magnitude can an electrolytic cell decompose a normally stable or inert chemical compound in the solution. The electrical energy provided undoes the effect of spontaneous chemical reactions.

 

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