Understanding Electrolysis: Moles of Chlorine Gas from Faradays

How Does Electrolysis Work? Let's Get Nerdy!

So, you’re preparing for the IGCSE Chemistry exam and want to tackle the electrifying world of electrolysis, specifically with sodium chloride (NaCl). To ignite our learning, let’s break down how we arrive at the number of moles of chlorine gas produced when electricity zaps its way through this salty solution.

What’s the Story with Sodium Chloride?

Sodium chloride, that's table salt for those of us just thinking about our next meal, dissolves in water and breaks apart into sodium ions (Na⁺) and chloride ions (Cl⁻). When we start to pass electricity through this solution, things get a bit zappy!

At the anode—where oxidation happens—we’re interested in our good friend, chlorine. The half-reaction responsible for creating chlorine gas (Cl₂) looks like this:

[ 2Cl^- \rightarrow Cl_2 + 2e^- ]

What does this little equation mean? Well, it tells us that two chloride ions are needed to create one mole of chlorine gas. But wait, we're just getting warmed up!

What's a Faraday Anyway?

Now, let’s talk about Faradays. A Faraday is a unit of electric charge that amounts to about 96485 coulombs (that’s a mouthful, isn’t it?). In our chemical playground, one Faraday is also equivalent to the amount of charge needed to produce one mole of monovalent ions at an electrode. So, in this scenario, it's like we’re assembling building blocks with the energy provided by our electricity!

Quick Fact: Why do we care about the moles of chlorine gas produced? Understanding this helps students calculate yields in chemical reactions and become more proficient in various electrochemical processes.

Putting It All Together: The Calculation

Now, back to our main equation. We know it requires 2 Faradays to produce 1 mole of Cl₂. So, if we hoist out 10 Faradays (thank you, science!), it’s easy to calculate how much chlorine we’re cooking up:

• Using our handy relationship: 2 Faradays = 1 mole of Cl₂
• For 10 Faradays, it looks like this:
  ➡️ 10 Faradays ÷ 2 Faradays/mole = 5 moles of Cl₂ formed.

That’s right—5 moles of chlorine gas form from our spirited little conversation of electricity through sodium chloride!

So, What's the Final Answer?

Given that you know everything from the charges to the proportions, the answer to the question posed is 5 mol of chlorine gas. If you ever asked yourself how electricity and chemistry play together, this is how they dance!

A Quick Recap: Why It Matters

Understanding this relationship isn't just about memorizing; it’s foundational for grasping more complex chemical processes down the line. As you are preparing for your IGCSE Chemistry exam, keeping these concepts sharp will help you tackle electrochemical reactions with confidence.

In summary, whether you’re about to shock a friend with your newfound knowledge or just trying to ace that exam, understanding how electricity interacts with chemical compounds will make you a superstar student. So, next time you see sodium chloride, think of it not just as a seasoning, but as a vital link in the study of chemistry!

And remember, even when the periodic table seems daunting, it's all about connecting the dots—just like how electricity connects ions to gas production, right? 🎉 Happy studying!