Equilibrium occurs when the rate of the forward reaction is equal to the rate of the reverse reaction, resulting in constant concentrations of reactants.

Chemical equilibrium is a form of dynamic equilibrium where the reaction is still occurring but the concentrations of reactants no longer change.

In a concentration profile graph, the concentrations of reactants reach a point of dynamic equilibrium where they no longer change over time.

The equilibrium constant K represents the ratio of the products to the reactants and is equal to the forward rate constant divided by the reverse rate constant.

The coefficients in the balanced chemical equation become exponents in the equilibrium expression.

To calculate the equilibrium constant Kc, the concentrations of the products and reactants at equilibrium are used.

⚖️ The video discusses the concept of chemical equilibrium and the equilibrium constant Kp and Kc.

📊 To calculate the equilibrium constant Kp, the partial pressures of the products and reactants are used in an expression.

🔢 The video also explains how to convert between Kp and Kc using the ideal gas law equation and the concentrations of the substances involved.

🔑 The equilibrium expression for Kp can be written as the ratio of the product of concentration terms to the product of reactant concentration terms.

🔢 The exponents in Kp can be obtained by adding the exponents of the concentration terms and the exponents of the rt terms.

⚖️ The relationship between Kp and Kc can be defined as Kp = Kc times rt raised to the power of delta n, where delta n is the sum of product coefficients minus reactant coefficients.

The equilibrium constant, K, is affected by adjusting the coefficients of a reaction.

Doubling the coefficients of a reaction results in K being squared.

Dividing the coefficients of a reaction by half results in K being raised to the power of one-half.

Reversing a reaction leads to K being equal to 1 divided by the original K value.

Multiplying the coefficients of a reversed reaction by a certain factor results in K being raised to the power of that factor.

The video explains how to calculate the equilibrium constant (K) for a chemical reaction using ice tables.

An example is presented where the equilibrium concentrations for reactants and products are determined using an ice table, and the value of Kc is calculated.

A second example demonstrates how to find the equilibrium concentration of a reactant (CO) using the given value of Kc and the concentrations of other substances at equilibrium.

🔑 At a certain temperature, ammonia partially decomposes into nitrogen gas and hydrogen gas at equilibrium.

📝 Using an ICE table, we can determine the partial pressures of the reactants and products at equilibrium.

💡 By solving for 'x' in the equation, we can calculate the equilibrium partial pressure of NH3.

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