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Rocket

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

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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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Test Tube

Chapter 6 - What Are The Mechanisms Of Chemical Change?

🌟 Key Concept: When a chemical reaction reaches equilibrium, the ratio of the concentrations of reactants and products is constant at a constant temperature. This constant is known as the equilibrium constant, K.

For a general reaction: aA + bB ⇌ xX + yY The equilibrium constant, K, is given by - K= [A] a [B] b [X] x [Y] y​

Here, the square brackets denote the concentrations of the substances, typically in moldm&minus;3&minus;3.

N2​(g) + 3H2​(g) ⇌ 2NH3(g)&nbsp;\(\frac{[NH_3]^2}{[N_2][H_2]^3}\)

<ul>
	<li>Concentration of Solvents: Not included in the K expression when the reaction takes place in a solution.</li>
	<li>Unitless Quantities: K values are treated as unitless to focus our attention on the crucial information about the system at equilibrium.</li>
	<li>Temperature Dependency: The value of K depends on temperature but not on other reaction conditions like pressure or concentration.</li>
</ul>

<ul>
	<li>If &gt;1K&gt;1: Products are favored. 📈</li>
	<li>If &lt;1K&lt;1: Reactants are favored. 📉</li>
	<li>If =1K=1: Approximately equal concentrations of reactants and products.</li>
</ul>

<ul>
	<li>&gt;&gt;1K&gt;&gt;1: Practically irreversible reaction. The forward reaction is favored strongly.</li>
	<li>&lt;&lt;1K&lt;&lt;1: Only the reverse reaction will be observed predominantly.</li>
</ul>

<ul>
	<li>If all stoichiometric coefficients are halved, the new K will be the square root of the original constant.</li>
	<li>If coefficients are doubled, the K will be squared.</li>
	<li>If the equation is reversed, the new K will be reciprocal to the original constant.</li>
</ul>

Worked Example

<ul>
	<li>For the reversed reaction of Ammonia Synthesis at 475K: 2NH3​(g) ⇌ N2​(g) + 3H2​(g) Given, K = 0.59 For the reversed reaction, &asymp;10.59&asymp;1.7K&prime;=K1​&asymp;0.591​&asymp;1.7</li>
	<li>And when the stoichiometric coefficients are halved K&prime;&asymp;&radic;1.7&asymp;1.3</li>
</ul>

Imagine the equilibrium constant like the perfect temperature for baking cookies. 🍪 Too high and the cookies will burn (favoring products). Too low, and they&#39;ll never bake (favoring reactants). Just right, and you have a delicious treat!

Understanding the equilibrium constant is like finding the perfect balance in a chemical reaction, just like having the right amount of toppings on your pizza or the right temperature for baking cookies. Keep practicing to master this concept!

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

Mastering Chemical Equilibrium!

Table of content

Equation & Definition ✍️

Real-World Example: Ammonia Synthesis 🌍

Important Points 🧠

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

Mastering Chemical Equilibrium!

Table of content

Equation & Definition ✍️

Real-World Example: Ammonia Synthesis 🌍

Important Points 🧠

Unlock the Full Content!