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Test Tube

Chapter 6 - What Are The Mechanisms Of Chemical Change?

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Atom Symbol

Chapter 1 - Models Of The Particulate Nature Of Matter

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Chapter 2 - Models Of Bonding & Structure

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 Globe with Meridians

Chapter 3 - Classification Of Matter

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Fire

Chapter 4 - What Drives Chemical Reactions?

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Rocket

Chapter 5 - How Much, How Fast & How Far?

Hey budding chemist! Ever wondered how batteries work or why some reactions just seem to &quot;go&quot; on their own? Let&#39;s dive into the exciting world of electrochemical cells to unravel the magic! 🎩✨

<ul>
	<li>Electrochemical Cells: These are the nifty devices where chemical energy transforms into electrical energy. They&#39;re what&#39;s powering your phone right now!</li>
	<li>Electrodes: The two metals (or other materials) involved in the reaction. Each half-cell has one! 🥇🥈</li>
	<li>Standard Cell Potential (E⦵ cell): Fancy name for the voltage or &quot;push&quot; in a battery. It&#39;s determined by the difference in &quot;want&quot; (or potential) of two electrodes to gain or lose electrons.</li>
</ul>

<ul>
	<li>The greater the difference in reactivity between two species, the higher the voltage.</li>
	<li>Fun Fact: If E⦵ cell is positive, the reaction happens on its own (spontaneous)! 🎉</li>
</ul>

Formula Time 📏: E⦵ cell = E⦵(cathode) &minus; E⦵(anode)

<ul>
	<li>Cathode: Where reduction happens (gains electrons). Think of it like a &quot;Cat&quot; receiving a treat (electron)! 🐱</li>
	<li>Anode: Where oxidation happens (loses electrons). Think &quot;A-no-de&quot; as in, &quot;Ah, no! I lost an electron!&quot; 😱</li>
</ul>

🌍 Real-World Example: Imagine two soccer teams, Team Fe (iron) and Team Cu (copper). Based on the data -&nbsp;Fe2+ (aq) + 2e&minus; ⇌ Fe(s) E⦵ = &minus;0.45V Cu2+ (aq) + 2e&minus; ⇌ Cu(s) E⦵ = +0.34V

&nbsp;

Team Cu is &quot;stronger&quot; (more positive E⦵) and wants to win (or get reduced). Meanwhile, Team Fe, being the &quot;weaker&quot; team (more negative E⦵), loses (or gets oxidized). The overall difference in their strengths is 0.79V (like a score difference in a match!).

&nbsp;

Overall equation: Fe(s) + Cu2+ (aq) ⇌ Fe2+ (aq) + Cu(s)

<ul>
	<li>For an electrochemical cell of Zn2+ |Zn and a standard hydrogen electrode: a. Anode: Zinc (Zn) 🥉 b. Spontaneous Reaction Direction: Forward! c. E⦵ cell = 0.76V 🎉</li>
	<li>For a cell with Cu2+ |Cu and Ag+ |Ag: a. Anode -&nbsp;Copper (Cu) b. Spontaneous Reaction -&nbsp;2Ag+(aq) + Cu(s) &rarr; 2Ag(s) + Cu2+ (aq) c. E⦵ cell = 0.46V 🥳</li>
</ul>

💡 Remember: The number of electrons lost and gained should balance. But the cell potential? It only cares about the nature of the species, not how we balance them. So, no doubling the voltage!

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Happy Chemistry-ing! 🧪🔍📚

Unlocking Standard Cell Potentials: Decoding Electrochemical Reactivity

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Standard Level

Chemistry SL

Chapter 6 - What Are The Mechanisms Of Chemical Change?

Unlocking Standard Cell Potentials: Decoding Electrochemical Reactivity

Table of content

What's in a battery? The Basics 🔋

The Connection 🔗

Unlock the Full Content!

Chapter 6 - What Are The Mechanisms Of Chemical Change?

Unlocking Standard Cell Potentials: Decoding Electrochemical Reactivity

Table of content

What's in a battery? The Basics 🔋

The Connection 🔗

Unlock the Full Content!