CHEM 30: Electrochemistry

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36 Terms

1

Oxidize

When a substance LOSES its electrons.

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2

Reduced

When a substance GAINS its electrons.

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3

Redox Reaction

The net reaction of oxidation and reduction.

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4

Oxidation and Reduction

Occur together in ONE reaction.

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5

Oxidizing Agent

A substance that gets reduced causes another substance to be oxidized.

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6

Reducing Agent

A substance that gets oxidized cause another substance to be reduced.

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7

Disproportionation

A reaction in which the same substance functions as both the oxidizing agent and a reducing agent; it is both reduced and oxidized.

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8

Oxidation Number

A positive or negative number that allows you to determine what is happening to the electron in the reaction.

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9

Oxidation Number Increaese

The substance is being OXIDIZED.

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10

Oxidation Number Decrease

The substance is being REDUCED.

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11

Oxidization States Constants

All atoms: 0

Hydrogen: +1, except in hydrides then -1

Oxygen: -2, except in peroxides then -1

Monatomic inons: charge on ion

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12

Spontaneity Rule

If the OA is above the RA pn the redox half reaction table.

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13

5 Step Methode

Step 1: list all entities present and classify as OA and RA and SOA and SRA.

Step 2: Write down the half reactions for the SOA.

Step 3: Write down the half reactions for the SRA.

Step 4: Balance the electrons in both half reactions and put the two half reactions together.

Step 5: Perdict spontinaity.

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14

Voltaic Cell

An electrochemical cell that spontaneously reacts to PRODUCE electricity.

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15

Electrolytic Cell

An electrochemical cell that USES electricity to cause a non-spontanious chemical change.

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16

Electrode

The solid in the half-cell where the wires attach.

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17

Anode

The electrode where oxidization occurs, where the strongest RA reacts.

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18

Cathode

The eletrode where reduction occurs, where the strongest OA reacts.

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19

Anion

A negative ion, moves toward the anode.

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20

Cation

A postive ion, moves toward the cathode.

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21

Salt Bridge

A barrier the keeps the solutions in a voltaic cell apart, but allows the flow of ions between the solutions to prevent an electrical charge build up. Required by Voltaic Cells

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22

Electrolyte

A substance the conducts electricity when dissolved in water.

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23

Power Supply

An electronic device that replaces a battery.

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24

External Circuit

The wires that are used to connect the anode to the cathode.

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25

Electron Flow

Anode to Cathode.

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26

Ion FLow

Anions to Anode; Cations to Cathade.

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27

Cell Spontanaity

Voltaic: yes

Electrolytic: no

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28

Net Electrode Potencial of Cells (E°net )

Voltaic: positve

Electrolytic: negative

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29

Line Notion of Cells

anode / anode electrolyte // cathode electrolyte / cathode

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30

Chloride Anomaly

When chloride acts as the reducing agent when with water in a reaction.

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31

Standard Hydrogen Half-Cell

What is used to measure the standard reduction potentials. It contains 1.00 mol/L of the hydrogen ion.

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32

Standard Cell Difference Equation

E°net= E°r(cathode) - E°r(anode)

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33

Calculating Cell Potential Difference

Step 1: List all entities present

Step 2: Determine OAs and RAs

Step 3: Determine SOAs and SRAs

Step 4: Write down anode and cathode half reactions (redox half reactions)

Step 5: Calculate the cell potential difference

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34

Spontaneity in Electrochemical Cells

If OA is above the RA, it is spontaneous.

If the cell potential is positive, the reactions is spontaneous.

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35

Faraday's Constant

9.65 x 10^4 C/mol → it represents the number of coulombs per mole of electrons.

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36

Moles of an Electron Equation

(I x t)/F

I = amps

t = time in seconds

F = Faraday's constant in C/s

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