[PDF] Chapter 20 Concepts and Formulas Electrochemistry is the PDF chapter%2020%20notes.pdf

When we balance redox (oxidation-reduction) equations, we look at the change each of the species has undergone We look at half-reactions We apply this basic

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Electrochemical Cells are of two types: It may be defined as the conducting power of all the ions formula unit of the electrolyte on complete dissociation 5

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Electrochemistry all formulas pdf Continue All important notes chemistry neet, JEE There are a total of 21 chapters in chemistry that are important to NEE and

[PDF] Chapter 20 Concepts and Formulas Electrochemistry is the

When we balance redox (oxidation-reduction) equations, we look at the change each of the species has undergone We look at half-reactions We apply this basic

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When the concentrations of all the species involved in a half-cell is unity then the electrode potential is known as standard electrode potential According to IUPAC

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Analysis shows that a metal oxide has the empirical formula M 0 98 O 1 00 (b ) Atoms B occupy all the octahedral voids and half of the tetrahedral voids Electrochemistry may be defined as the branch of chemistry which deals with the

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If all three conditions are not met, then it is nonstandard conditions Formulas Definitions E°cell = E°red + E°ox E°cell = cell potential at standard conditions,

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(3) v+ and v- are the numbers of cations and anions per formula unit of an difference for zero current through the cell, all local charage transfer equilibria and

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between them By 1812, the Swedish chemist Berzelius could propose that all Electrochemistry is the study of reactions in which charged particles (ions or electrons) to the next on the right is written in between the formulas (Note that the

Chapter 20 Concepts and Formulas

Electrochemistry is the relationship between electricity and chemical re actions. Remember LEO goes GER! (Losing electrons is oxidation, gaining electro ns is reduction) When we balance redox (oxidation-reduction) equations, we look at the change each of the species has undergone. We look at half-reactions. We apply this basic method:

1) Balance each half-reaction, leaving H and O for last, unless H

and H2 are involved.

2) Balance the O by adding H

O to one side and H

to the other, then add e as needed.

If done in basic solution, OH

ions are to be added afterwards. 3) Multiply each half-reaction by an integer so that the number of e

are the same and cancel out when the two half-reactions are added together.

4) Simplify by cancelling, if possible, and check to see everything is

balanced.

Voltaic cells --->

Anode -- where oxidation occurs -- "a negative electrode" Cathode -- where reductions occursTwo metals can pass electrons via a conducting salt "bridge." Voltage, or electromotive force, the electrical potential, sometimes call ed the potential difference between two points in a circuit. It is analagous to gravitation al potential; that One volt (V) is the potential difference required to impart one joule (J) of energy to one coulomb (C) of electrons. That is

1 V = -----

One coulomb is 6.25 x 10

18 electrons....one electron's charge is 1.6 x 10 -19 C. Unless noted, all electrochemical reactions are considered at 25°C (

298 K).

The standard cell potential is given as E

o cell = E o (cathode) - E o (anode). The little o represents standard state conditions.

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