IB Chemistry Topic R3.2.14 Gibbs Free Energy and Cell Potential Revision Notes (HL)

IB Chemistry Topic R3.2.14 Gibbs Free Energy and Cell Potential Revision Notes (HL) | RevisionDojo

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The Equation: $ΔG^\circ = −nFE^\circ_{\text{cell}}$

The equation $$ΔG^\circ = −nFE^\circ_{\text{cell}}$$ links two fundamental concepts in chemistry: Gibbs free energy change ($ΔG^\circ$) and standard cell potential ($E^\circ_{\text{cell}}$).
Let’s break it down step by step to understand how it works.

$ΔG^\circ$ (Standard Gibbs Free Energy Change):

$ΔG^\circ$ represents the maximum amount of energy available to do useful work from a chemical reaction under standard conditions (298 K, 1 bar, and 1 M concentrations for all solutions).
The sign of $ΔG^\circ$ determines spontaneity:
1. Negative $ΔG^\circ$: The reaction is spontaneous under standard conditions.
2. Positive $ΔG^\circ$: The reaction is non-spontaneous under standard conditions.
3. $ΔG^\circ=0$: The system is at equilibrium.

$E^\circ_{\text{cell}}$ (Standard Cell Potential):

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The Equation: $ΔG^\circ = −nFE^\circ_{\text{cell}}$

The equation $$ΔG^\circ = −nFE^\circ_{\text{cell}}$$ links two fundamental concepts in chemistry: Gibbs free energy change ($ΔG^\circ$) and standard cell potential ($E^\circ_{\text{cell}}$).
Let’s break it down step by step to understand how it works.

$ΔG^\circ$ (Standard Gibbs Free Energy Change):

$ΔG^\circ$ represents the maximum amount of energy available to do useful work from a chemical reaction under standard conditions (298 K, 1 bar, and 1 M concentrations for all solutions).
The sign of $ΔG^\circ$ determines spontaneity:
1. Negative $ΔG^\circ$: The reaction is spontaneous under standard conditions.
2. Positive $ΔG^\circ$: The reaction is non-spontaneous under standard conditions.
3. $ΔG^\circ=0$: The system is at equilibrium.

$E^\circ_{\text{cell}}$ (Standard Cell Potential):

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Structure 1. Models of the particulate nature of matter5 subtopics

Structure 2. Models of bonding and structure4 subtopics

Structure 3. Classification of matter2 subtopics

Reactivity 1. What drives chemical reactions?4 subtopics

Reactivity 2. How much, how fast and how far?3 subtopics

Reactivity 3. What are the mechanisms of chemical change?4 subtopics

IB Chemistry R3.2.14 Gibbs Free Energy and Cell Potential Notes

Structure 1. Models of the particulate nature of matter5 subtopics

Structure 2. Models of bonding and structure4 subtopics

Structure 3. Classification of matter2 subtopics

Reactivity 1. What drives chemical reactions?4 subtopics

Reactivity 2. How much, how fast and how far?3 subtopics

Reactivity 3. What are the mechanisms of chemical change?4 subtopics

The Equation: $ΔG^\circ = −nFE^\circ_{\text{cell}}$

$ΔG^\circ$ (Standard Gibbs Free Energy Change):

$E^\circ_{\text{cell}}$ (Standard Cell Potential):

anim nostrud sit dolore minim proident quis fugiat velit et eiusmod nulla quis nulla mollit dolor sunt culpa aliqua

Duis aute irure dolor in reprehenderit

Excepteur sint occaecat cupidatat non proident

Unlock the rest of this chapter with a free account

The Equation: $ΔG^\circ = −nFE^\circ_{\text{cell}}$

$ΔG^\circ$ (Standard Gibbs Free Energy Change):

$E^\circ_{\text{cell}}$ (Standard Cell Potential):

anim nostrud sit dolore minim proident quis fugiat velit et eiusmod nulla quis nulla mollit dolor sunt culpa aliqua

Duis aute irure dolor in reprehenderit

Excepteur sint occaecat cupidatat non proident

Unlock the rest of this chapter with a free account