EXTRACTION OF BROMINE FROM SEA WATER

Slides:

Advertisements

Similar presentations

12 Chemistry 2.2 quantitative chemistry CR 07 Halogens: F 2, Cl 2, Br 2, I 2 Halogens as oxidants: Halogens attract electrons from other substances – they.

Advertisements

Oxidation-Reduction Oxidation literally means to react with oxygen. Oxidation literally means to react with oxygen. Example:2Mg + O 2 2MgO Example:2Mg.

None of these react with bare copper. Oxidized here FeCl 3 Pb(NO 3 ) 2 Mg(NO 3 ) 2.

Blast Furnace Reactions

CHEMISTRY DEPARTMENT WAID ACADEMY Redox and Faraday.

11.0 The Halogens Text book p166 to AQA AS Specification LessonsTopics 1 How and why does the atomic radius and electronegativity change in Gp.

Unit 33 Bleach. Types of Bleaches Household chlorine bleach – a solution of chlorine in sodium hydroxide solution Cl 2(aq) + 2NaOH (aq)  NaCl (aq) +

Bromobutane. Halogenoalkanes Halogenoalkanes are hydrocarbon chains that have one or more hydrogen atom(s) exchanged for halogen atom(s).

Third Nine Weeks- 9 weeks review

Sea water BLOWING OUT TOWER STEAMING OUT TOWER CONDENSER SEPARATOR DRYER.

Bleach 21 What is a bleach? What has caused this colour change?

Unit 20 Oxidation and reduction Activity 20.2 Investigating redox reactions of aqueous chlorine Reference in textbook: Section S.

Zn  Zn2+ + 2e- (oxidation) Cu e-  Cu (reduction)

Redox Reactions What is oxidation? What is reduction?

The Preparation and Collection Of Non-Metals.

All toxic All form Diatomic molecules All form ionic salts

Electrolysis. –A redox reaction that is made to occur by passing a direct electric current through an electrolyte Electrolyte –is a liquid that conducts.

When bleach is treated with an acid, evolution of chlorine gas ensues Preparation of Chlorine Gas from Bleach.

“Redox” REVIEW GAME.

Redox Reactions and Oxidation States. The Basics...  ‘Redox’ is used to describe reactions where oxidation and reduction take place.  If one reactant.

Displacement Reactions. Lets look at the reaction between chlorine and potassium bromide When chlorine is bubbled through potassium bromide solution (colourless),

Halogens AS. F Cl Br I (At) Generally: Oxidising agents Germicides Note: Atoms are halogens Ions are halides Ions have 8 electrons by borrowing one, so.

Chemistry Revision 3. Electronic configurations State which block in the periodic table you find the following elements: Sulphur Vanadium Strontium.

Redox Reactions. Oxidation Reduction Oxidation and Reduction Oxidation: Gain of oxygen Loss of electrons Reduction: Loss of oxygen Gain of electrons.

Bell Work Write down these equations, then answer the following: __BiCl 5 + __Zn  __ZnCl 2 + __Bi and __Mg(NO 3 ) 2 + __Na 2 SO 4  __NaNO 3 + __MgSO.

Studio 13b: Activity Series. Redox Reactions 2 Fe (s) + 3 Cl 2(g)  2 FeCl 3(s) Fe 0  Fe +3 Cl 0  Cl - A species is said to undergo REDUCTION if it.

Applications of Redox Electrochemistry. Review Oxidation reduction reactions involve a transfer of electrons. OIL-RIG Oxidation Involves Loss Reduction.

Choose Your Category Oxidation Numbers Redox Reactions Balancing Chemical Reactions Reaction Types Note Type Questions Organic Questions

Na & K, Mg & Br Zephan and Tae. Alkali Metals Most reactive elements – Ionic in nature (solid or aqueous) – Kept under special conditions to prevent contact.

Redox equations.

Permanganate reactions. Manganese exists in many different oxidation states, each with a characteristic colour including: Mn VII: MnO 4 – purple Mn VI:

Redox reactions of the halogens

COMMON REDOX REACTIONS

Choose Your Category Will It Happen Oxidation Numbers Redox Reactions Balancing Chemical Reactions Reaction Types Note Type Questions Organic Questions.

Unit: Electrochemistry

Redox Reactions – Examples(1 – Synthesis) The following is one type of oxidation/ reduction reaction. 1.Balance the equation. 2.Indicate the species that.

IGCSE CHEMISTRY SECTION 2 LESSON 2. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.

IGCSE CHEMISTRY SECTION 2 LESSON 4. Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3.

Analysing Oxidants and Reductants. What is a redox reaction? The reactant that loses electrons is oxidised Mnemonic devices OIL RIG O(xidation) I(s) L(oss.

The Periodic Table Chapter 12. The modern periodic table  Arranged by atomic number NOT atomic mass. Atomic number: Number of protons  New elements.

3.2.3 Group 7, the Halogens.

Alcohols – nomenclature and reactions

Starter Write the word equation for the following reactions.

HALOGENS PRECIOUS.

Redox reactions ?.

Redox Reactions and Electrolysis

sea water BLOWING OUT TOWER CONDENSER SEPARATOR STEAMING OUT TOWER

Reactions of the halogens and halide ions

Double-Replacement Reactions

Do Now How many possible reactions are there when Group 1 and 2 elements react with Group 7? Which reaction would be the most reactive of them all? Which.

Types of Chemical Reactions

Group 2 and 7 revision.

Knowledge Organiser – Chemical Changes

2.6.3 Redox Reactions of the Halogens

Group 7 Members General comment Elements Symbols

Oxidation-Reduction Reactions “Redox”

Redox reactions.

Double-Replacement Reactions

EXTRACTION OF BROMINE FROM SEA WATER

2.6.3 Redox Reactions of the Halogens

Chemistry 4: Chemical Changes

Oxidation and Reduction, Displacement and Rusting.

1.5 b Learning Outcomes apply knowledge of oxidation and reduction to explain the rusting of iron give an example of an oxidising and a reducing bleach.

Presentation transcript:

EXTRACTION OF BROMINE FROM SEA WATER 1. Oxidation of Bromide ions to Bromine. Removal of Bromine Vapour. Reduction of Bromine to Hydrobromic acid. 4. Oxidation of Hydrobromic acid to Bromine

1:Oxidation Of Bromide to Bromine Seawater is acidified using H2SO4. ( pH8-3.5). Why? At High pH Chlorine and Bromine react with Water. Br2(aq) + H2O(aq)HBr(aq) + HBrO(aq) Cl2(aq) + H2O(aq)HCl(aq) + HClO(aq)

What is Redox? Iron is OXIDISED – It is Losing Electrons Fe  Fe2+ + 2e- O + 2e-  O2- Oxygen is being Reduced- It is Gaining Electrons

A Small Excess of Chlorine is added to the acidified Water, to displace Bromine by a redox reaction. Cl2(aq) + 2Br-(aq)2Cl-(aq) + Br2(aq) 2Br-(aq) Br2(aq) +2e- : Cl2(aq)+2e-  2Cl- Chlorine is the Oxidising agent and Bromine the Reducing agent

2: Removal of Bromine Vapour Treated Sea water then passes into a Blowing out tower: Bromine being very volatile is removed from the air along with some chlorine. The Bromine Vapour Concentration is TOO LOW to produce liquid Bromine

Blowing out tower

3: Reduction of Bromine to Hydrobromic acid Sulphur dioxide is injected into the blowing out tower. The Bromine is reduced to hydrobromic acid by the sulphur dioxide Br2(aq) + SO2(g) + 2H2O0(l)  2HBr(aq) + H2SO4(aq) A fine mist of acids is produced when fresh water is injected into the tower. This is then condensed in the absorber stage of the tower. The mixture now contains 13% by mass of bromine.

4: Oxidation of Hydrobromic acid to Bromine The Acid passes into a steaming out tower. Chlorine regenerates the bromine using a redox reaction 2HBr(aq) + Cl2(g)  Br2(g) + 2HCl(aq) Chlorine oxidises the Bromide in HBr to bromine. Hot vapour is condensed to form an aqueous layer and a lower layer of bromine

4: Oxidation of Hydrobromic acid to Bromine Spent seawater is discharged. Remaining Br2 and Cl2 are destroyed using sulphur dioxide before any water leaves the blowing out tower. On discharge the pH s 3.5 but rapidly rises to ph8.

Dense Dark and Beautiful Extraction is a continuous process. Bromine is transported in lead –lined steel Tanks.