Question

Balancing of Redox Reactions MnO, +so; Mn" +so; (Acidic)​

Answer 1

Answer:

okk hope this helps you

mark me as brainliest

Explanation:

logo.png

Adopted a LibreTexts for your class? Click here to let us know!

Search

How can we help you?

Search

Remixer

Downloads

Sign in

Contents Home Bookshelves Analytical Chemistry Supplemental Modules (Analytical Chemistry) Electrochemistry Expand/collapse global location

Balancing Redox Reactions - Examples

Last updatedApr 1, 2021

Balancing Redox Reactions

Comparing Strengths of Oxidants and Reductants

picture_as_pdf

Readability

Cite this page

Donate

Oxidation-Reduction or "redox" reactions occur when elements in a chemical reaction gain or lose electrons, causing an increase or decrease in oxidation numbers. The Half Equation Method is used to balance these reactions.

In a redox reaction, one or more element becomes oxidized, and one or more element becomes reduced. Oxidation is the loss of electrons whereas reduction is the gain of electrons. An easy way to remember this is to think of the charges: an element's charge is reduced if it gains electrons (an acronym to remember the difference is LEO = Lose Electron Oxidation & GER = Gain Electron Reduction). Redox reactions usually occur in one of two environments: acidic or basic. In order to balance redox equations, understanding oxidation states is necessary.

Some points to remember when balancing redox reactions:

The equation is separated into two half-equations, one for oxidation, and one for reduction.

The equation is balanced by adjusting coefficients and adding H2O, H+, and e- in this order:

1) Balance the atoms in the equation, apart from O and H.

2) To balance the Oxygen atoms, add the appropriate number of water (H2O) molecules to the other side.

3) To balance the Hydrogen atoms (including those added in step 2), add H+ ions.

4) Add up the charges on each side. They must be made equal by adding enough electrons (e-) to the more positive side.

The e- on each side must be made equal; if they are not equal, they must be multiplied by appropriate integers to be made the same.

The half-equations are added together, cancelling out the electrons to form one balanced equation. Cancel out as much as possible.

(If the equation is being balanced in a basic solution, the appropriate number of OH- must be added to turn the remaining H+ into water molecules)

The equation can now be checked to make sure it is balanced