New concepts in the scale-up of chlorine-caustic mercury cells

Gallone, P.

doi:10.1007/bf00613502

J Appl Electrochem

1973

DOI: 10.1007/bf00613502

|View full text |Cite

New concepts in the scale-up of chlorine-caustic mercury cells

P. Gallone

Help me understand this report

Search citation statements

Order By: Relevance

Paper Sections

Select...

Citation Types

Supporting

Mentioning

Contrasting

Year Published

1980

2005

Publication Types

Select...

Article3

Relationship

Self Cite0

Independent3

Authors

Journals

Cited by 3 publications

(2 citation statements)

References 6 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…Since the recovery of chlorine is often the best way from the viewpoints of economy and the environment, several chlorine recovery processes have been reported. [2][3][4][5] On the other hand, the fixation of nitrogen as ammonia is also an important process because ammonia is an essential ingredient of fertilizer, chemicals, and so on. 6 The authors have proposed an electrolytic ammonia synthesis method from nitrogen and various hydrogen sources, such as hydrogen, 7 methane, 8 hydrogen sulfide, 9 and water, 10 in molten salts under atmospheric pressure.…”

mentioning

confidence: 99%

Electrolytic Ammonia Synthesis from Hydrogen Chloride and Nitrogen Gases with Simultaneous Recovery of Chlorine under Atmospheric Pressure

Murakami

Nishikiori

Ito

2005

Electrochem. Solid-State Lett.

View full text Add to dashboard Cite

It was confirmed that ammonia was synthesized by bubbling hydrogen chloride gas into a LiCl-KCl-CsCl melt containing nitride ions at 573 K. Then, anodic galvanostatic electrolysis was conducted at 20 mA cm −2 using a glassy carbon working electrode and a nitrogen gas counter electrode, which showed that chlorine evolved at the anode by the oxidation of chloride ions, and that nitrogen was reduced to nitride ions at the cathode. The obtained results confirmed that ammonia and chlorine were produced from hydrogen chloride and nitrogen as the overall reaction.Hydrogen chloride is produced as a by-product in various industrial chlorination processes. 1 Approximately half of the chlorine produced in the world, which amounts to tens of millions of metric tons per year, is wasted as hydrogen chloride or chloride salts in the current world chlorination processes. Therefore, effective utilization of the hydrogen chloride by-product is required. Since the recovery of chlorine is often the best way from the viewpoints of economy and the environment, several chlorine recovery processes have been reported. 2-5 On the other hand, the fixation of nitrogen as ammonia is also an important process because ammonia is an essential ingredient of fertilizer, chemicals, and so on. 6 The authors have proposed an electrolytic ammonia synthesis method from nitrogen and various hydrogen sources, such as hydrogen, 7 methane, 8 hydrogen sulfide, 9 and water, 10 in molten salts under atmospheric pressure. Here, the authors propose a novel electrochemical method that utilizes hydrogen chloride as a hydrogen source for ammonia synthesis and simultaneously recovers chlorine from hydrogen chloride. The principle is shown in Fig. 1. The electrolyte is molten alkali metal halides. Nitrogen gas is reduced to nitride ion ͑N 3− ͒ at the cathode 11Hydrogen chloride gas is introduced into the melt between the anode and the cathode, preferably in the vicinity of the cathode. Then, the nitride ions formed at the cathode react with hydrogen chloride in the melt to form ammoniaAt the anode, chlorine gas is produced by the oxidation of chloride ionsIn total, ammonia and chlorine are produced from hydrogen chloride and nitrogen gases under atmospheric pressureThe theoretical standard electrolysis voltage is calculated to be 1.06 V at 573 K from the standard Gibbs energy change of Reaction 4 306 kJ mol −1 . 12 Since the standard electrode potential of N 2 /N 3− couple was reported to be 0.281 V ͑vs. Li + /Li͒ 13 in LiClKCl-CsCl melt at 573 K, the standard Gibbs energy of formation of Li 3 N in the melt can be evaluated as −81.3 kJ mol −1 . The standard Gibbs energies of formation of NH 3 ͑g͒, HCl͑g͒, and LiCl͑l͒ at 573 K are reported as 13.1, −97.8, and −345.0 kJ mol −1 , respectively. 12 Then, the equilibrium constant of Reaction 5 is calculated to be 1.0 ϫ 10 59 3HCl + Li 3 N → NH 3 + 3LiCl ͓5͔

show abstract

mentioning

confidence: 99%

Electrolytic Ammonia Synthesis from Hydrogen Chloride and Nitrogen Gases with Simultaneous Recovery of Chlorine under Atmospheric Pressure

Murakami

Nishikiori

Ito

2005

Electrochem. Solid-State Lett.

View full text Add to dashboard Cite

show abstract

“…Alternatively, HCl may be decomposed electrochemically. In the Uhde, or DeNora, electrolysis cell, hydrochloric acid is fed to both the anode and the cathode, and direct current is used to decompose HCl 4,5 2HCl ͑ aq͒ → H 2 ϩ Cl 2 ͓2͔…”

mentioning

confidence: 99%

Chlorine Recovery from Anhydrous Hydrogen Chloride in a Molten Salt Electrolyte Membrane Cell

Bartling¹,

Winnick²

2003

J. Electrochem. Soc.

View full text Add to dashboard Cite

A novel electrochemical membrane process has been developed to recover chlorine from anhydrous HCl waste. The proposed method produces a pure chlorine product stream and a hydrogen-enriched stream from HCl waste in a single step. The electrochemical method requires only an external electric potential and no concentration gradient, and it produces chlorine with exceptional selectivity. The electrolyzer can be operated at high current densities and current efficiencies. Downstream separation is not necessary, and no exotic electrode materials are required. A single experimental cell was constructed and tested for HCl removal and chlorine production from concentrated HCl reactant streams at variable flow rate. Applied current densities exceeded 400 mA/cm 2 , and conversions over 94% were achieved. Ohmic resistance dominated cell potentials due to the formation of hydrogen and chlorine bubbles. The proposed process is found to be a viable option for the treatment of anhydrous HCl waste.

show abstract

Electrochemical reaction engineering

Jansson¹

1980

Chemical Engineering Science

View full text Add to dashboard Cite

scite is a Brooklyn-based organization that helps researchers better discover and understand research articles through Smart Citations–citations that display the context of the citation and describe whether the article provides supporting or contrasting evidence. scite is used by students and researchers from around the world and is funded in part by the National Science Foundation and the National Institute on Drug Abuse of the National Institutes of Health.

Contact Info

customersupport@researchsolutions.com

10624 S. Eastern Ave., Ste. A-614

Henderson, NV 89052, USA

This site is protected by reCAPTCHA and the Google Privacy Policy and Terms of Service apply.

Blog Terms and Conditions API Terms Privacy Policy Contact Cookie Preferences Do Not Sell or Share My Personal Information

Made with 💙 for researchers

Part of the Research Solutions Family.

New concepts in the scale-up of chlorine-caustic mercury cells

Cited by 3 publications

References 6 publications

Electrolytic Ammonia Synthesis from Hydrogen Chloride and Nitrogen Gases with Simultaneous Recovery of Chlorine under Atmospheric Pressure

Electrolytic Ammonia Synthesis from Hydrogen Chloride and Nitrogen Gases with Simultaneous Recovery of Chlorine under Atmospheric Pressure

Chlorine Recovery from Anhydrous Hydrogen Chloride in a Molten Salt Electrolyte Membrane Cell

Electrochemical reaction engineering

Contact Info

Product

Resources

About