badge image

Enroll For Free Now & Improve Your Performance.

×
User Icon
User Icon
User Icon
User Icon
User Icon

Thank you for registering.

One of our academic counsellors will contact you within 1 working day.

Please check your email for login details.
MY CART (5)

Use Coupon: CART20 and get 20% off on all online Study Material

ITEM
DETAILS
MRP
DISCOUNT
FINAL PRICE
Total Price: Rs.

There are no items in this cart.
Continue Shopping
Menu
Grade: 9

                        

explain how rusting of iron is envisaged as setting of an electrochemical series

6 years ago

Answers : (2)

Vasantha Kumari
askIITians Faculty
38 Points
							

The term corrosion refers to degradation of metals in their chemical interaction with the environment and usually we refer to steel in this process. Metals that are in a metastable state will lose energy as they have little mechanical strength. These corrosion reactions are electrochemical in nature and a mixed anodic and cathodic reaction happens at its surface. This mixed electrode is a complete electrochemical cell on a single metal.

Metals of differing electrochemical properties come in contact a galvanic couple is formed.
We can predict these galvanic effects by studying the galvanic series comprising metals and alloys in order of their potentials in the corrosive environment.

Thanks & Regards,

Vasantha Sivaraj,

askIITians faculty.

6 years ago
K RAJESH
37 Points
							Rusting of iron form an electrochemical cell.The reaction is take place in presence of water. An electrochemical cell is created on an iron object that has a distinct anode and cathode.

    * At one spot  iron loses electrons (is oxidized) to form iron (II) ions.

 Fe (s)?Fe2+ (aq) + 2e- (the anodic site of our electrochemical cell)

    * At another spot oxygen in the air combines with water and forms hydroxide ions.

Ā½O2 (g) + H2O (l) + 2e-? 2OH- (aq)(the cathodic site of our electrochemical cell)

    * In the presence of oxygen  iron further oxidizes at the anode (loses electrons) to become iron (III) ions.

Fe 2+ (aq)? Fe3+ (aq) + e-

    * The iron (III) ions and the hydroxide combine to form rust.

2Fe 3+ (aq) + 6OH- (aq)? Fe2O3 (s) + 3 H2O (l) 
Hence, rusting of iron act as electrochemical cell.
						
6 years ago
Think You Can Provide A Better Answer ?
Answer & Earn Cool Goodies


Course Features

  • 731 Video Lectures
  • Revision Notes
  • Previous Year Papers
  • Mind Map
  • Study Planner
  • NCERT Solutions
  • Discussion Forum
  • Test paper with Video Solution


Course Features

  • 54 Video Lectures
  • Revision Notes
  • Test paper with Video Solution
  • Mind Map
  • Study Planner
  • NCERT Solutions
  • Discussion Forum
  • Previous Year Exam Questions


Ask Experts

Have any Question? Ask Experts

Post Question

 
 
Answer ā€˜nā€™ Earn
Attractive Gift
Vouchers
To Win!!! Click Here for details