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Free Equilibrium Constant Lesson

Practice Equilibrium Constant concepts in Chemistry. Step-by-step lessons to reinforce learning and understanding.

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Lesson 1: Equilibrium Constant

Equilibrium Constant

In chemistry, the equilibrium constant, denoted as ${K}_c$ , quantifies the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. It is a crucial concept in understanding chemical equilibria.

Definition

For a general reaction: $aA + bB \rightleftharpoons cC + dD$ The equilibrium constant is expressed as: where:

Keywords: Equilibrium, Equilibrium Constant, Chemical Reaction, Concentration

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{K}_c = \frac{[C]^c [D]^d}{[A]^a [B]^b}

$[C]$ , $[D]$ , $[A]$ , and $[B]$ are the equilibrium concentrations of the species.
$a$ , $b$ , $c$ , and $d$ are the coefficients from the balanced chemical equation.

Example

Consider the reaction: $2H_{2}(g) + O_{2}(g) \rightleftharpoons 2H_{2}O(g)$ The equilibrium constant expression is: $K_c = \frac{[H_{2}O]^{2}}{[H_{2}]^{2} [O_{2}]}$

Steps to Calculate ${K}_c$ :

Write the balanced equation.
Identify the concentrations at equilibrium.
Substitute the values into the equilibrium expression.
Calculate $K_c$ .

Key Questions

What factors can affect the value of the equilibrium constant?
How do you interpret the value of $K_c$ ?
What is the difference between $K_c$ and $K_p$ ?

Summary

The equilibrium constant is a fundamental concept in chemical equilibrium that allows chemists to predict the direction of a reaction and the concentrations of reactants and products at equilibrium.

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