Name: finding kc from equilibrium data
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 2 min 46 s
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Chemistry

Matter and its Interactions

PS.Chm.5.2

Calculating the Equilibrium Constant

O equilíbrio constante, Kc, pode ser determinado através da substituição dos valores correspondentes para a expressão de equilíbrio constante se as concentrações de todos os reagentes e produtos em equilíbrio forem conhecidas. Uma mistura gasosa de dióxido de enxofre e oxigénio a 530 graus Celsius é permitida para reagir de acordo com a reação demonstrada. Em equilíbrio, a mistura contém 0, 10 molar de dióxido de enxofre, 0, 15 molar de oxigénio, e 10, 88 molar de trióxido de enxofre.Ao substituir os valores na expressão de equilíbrio, o Kc é igual a 7, 9 10⁴. O Kc também pode ser calculado desde que a concentração inicial de todos os componentes e a concentração de concentração de pelo menos um composto seja conhecida. As concentrações de equilíbrio desconhecidas podem ser calculadas utilizando a estequiometria de reação.É utilizada uma tabela ICE para organizar a informação para as concentrações inicial, de mudança e de equilíbrio da reação. Quando é permitido uma mistura de reação que contém 0, 11 molar de nitrogénio e 0, 36 molar de hidrogénio alcançar o equilíbrio a 500 graus Celsius, ela produz 0, 020 molar de amoníaco em equilíbrio. Para calcular o Kc, as concentrações de equilíbrio do nitrogénio e hidrogénio precisam de ser determinadas.A estequiometria da reação mostra que 1 mol de gás de nitrogénio e 3 mols de gás de hidrogénio são obrigados a produzir 2 mols de gás de amoníaco. A mudança, x, quando multiplicada pelos coeficientes dos reagentes e produtos, denota a concentração dos reagentes consumidos e a concentração do produto produzido para alcançar o equilíbrio. Se 2x é igual a 0, 020, x é igual a 0, 010.A concentração de equilíbrio do nitrogénio e hidrogénio pode então ser determinada pela subtração da respectiva alteração da concentração desde que a sua concentração inicial equivale a 0, 10 e 0, 33 molar, respetivamente. Ao substituir as concentrações de equilíbrio na expressão Kc Kc, o Kc é igual a 0, 11. O Kp para reações que envolvam gases pode ser calculado utilizando uma tabela ICE e a expressão de equilíbrio escrita com pressões parciais.

cálculo da constante de equilíbrio

A constante de equilíbrio para uma reação é calculada a partir das concentrações de equilíbrio (ou pressões) dos seus reagentes e produtos. Se estas concentrações forem conhecidas, o cálculo envolve simplesmente a sua substituição na expressão Kc.
Por exemplo, o dióxido de nitrogénio gasoso forma tetróxido de dinitrogénio de acordo com esta equação:
<img alt="Eq1" src="/files/ftp_upload/11388/11388_Equation_1.png" style="text-align: center; height: 50px;" />
Quando se adiciona 0,10 mol de NO2 a um frasco de 1,0 L a 25 °C, a concentração muda de modo a que, em equilíbrio, [NO2] = 0,016 M e [N2O4] = 0,042 M. O valor da constante de equilíbrio para a reação pode ser calculado da seguinte forma:
<img alt="Eq2" src="/files/ftp_upload/11388/11388_Equation_2.png" style="text-align: center; height: 90px;" />
Um exemplo um pouco mais desafiante é mostrado a seguir, no qual a estequiometria da reação é usada para derivar concentrações de equilíbrio a partir da informação fornecida. A estratégia básica desta computação é útil para muitos tipos de cálculos de equilíbrio e depende do uso de termos para as concentrações de reagentes e produtos inicialmente presentes, para como elas mudam à medida que a reação prossegue, e para o que elas são quando o sistema atinge o equilíbrio. O acrónimo ICE é comumente usado para referir essa abordagem matemática, e os termos de concentração são geralmente reunidos em um formato tabular chamado de tabela ICE.
Cálculo de uma Constante de Equilíbrio
As moléculas de iodo reagem reversivelmente com iões iodeto para produzir iões triiodeto.
<img alt="Eq3" src="/files/ftp_upload/11388/11388_Equation_3.png" style="text-align: center; height: 50px;" />
Se uma solução com concentrações de I2 e I− ambas iguais a 1,000 × 10−3 M antes da reação der uma concentração de equilíbrio de I2 de 6,61 × 10−4 M, qual é a constante de equilíbrio para a reação?
Para calcular as constantes de equilíbrio, são necessárias concentrações de equilíbrio para todos os reagentes e produtos:
<img alt="Eq4" src="/files/ftp_upload/11388/11388_Equation_4.png" style="text-align: center; height: 90px;" />
São fornecidas as concentrações iniciais dos reagentes e a concentração de equilíbrio do produto. Esta informação pode ser usada para derivar termos para as concentrações de equilíbrio dos reagentes, apresentando todas as informações em uma tabela ICE.
<table style="margin-left: auto; margin-right: auto;">
<tbody>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;"></td>
<td style="color: black; border: 1px solid black; text-align: center;">      I2 (aq)        </td>
<td style="color: black; border: 1px solid black; text-align: center;">I− (aq) </td>
<td style="color: black; border: 1px solid black; text-align: center;">   I3− (aq)     </td>
</tr>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Concentração Inicial (M)</td>
<td style="color: black; border: 1px solid black; text-align: center;">1,000 × 10−3</td>
<td style="color: black; border: 1px solid black; text-align: center;">1,000 × 10−3</td>
<td style="color: black; border: 1px solid black; text-align: center;">0</td>
</tr>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Alteração (M)</td>
<td style="color: black; border: 1px solid black; text-align: center;">−x</td>
<td style="color: black; border: 1px solid black; text-align: center;">−x</td>
<td style="color: black; border: 1px solid black; text-align: center;">+x</td>
</tr>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Concentração em Equilíbrio (M)</td>
<td style="color: black; border: 1px solid black; text-align: center;">  1,000 × 10−3 − x  </td>
<td style="color: black; border: 1px solid black; text-align: center;">    1,000 × 10-3 − x  </td>
<td style="color: black; border: 1px solid black; text-align: center;">x</td>
</tr>
</tbody>
</table>
Em equilíbrio a concentração de I2 é 6,61 × 10−4 M por isso
<img alt="Eq5" src="/files/ftp_upload/11388/11388_Equation_5.png" style="text-align: center; height: 90px;" />
A tabela ICE pode agora ser atualizada com valores numéricos para todas as suas concentrações:
<table style="margin-left: auto; margin-right: auto;">
<tbody>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;"></td>
<td style="color: black; border: 1px solid black; text-align: center;">I2 (aq) </td>
<td style="color: black; border: 1px solid black; text-align: center;">I− (aq) </td>
<td style="color: black; border: 1px solid black; text-align: center;">I3− (aq)</td>
</tr>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Concentration Inicial (M)</td>
<td style="color: black; border: 1px solid black; text-align: center;"> 1,000 × 10−3 </td>
<td style="color: black; border: 1px solid black; text-align: center;">  1,000 × 10−3  </td>
<td style="color: black; border: 1px solid black; text-align: center;">0</td>
</tr>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Alteração (M)</td>
<td style="color: black; border: 1px solid black; text-align: center;"> −3,39 × 10−4 </td>
<td style="color: black; border: 1px solid black; text-align: center;">  −3,39 × 10−4  </td>
<td style="color: black; border: 1px solid black; text-align: center;">  +3,39 × 10-4  </td>
</tr>
<tr>
<td style="color: black; border: 1px solid black; text-align: center;">Concentração em Equilíbrio (M)</td>
<td style="color: black; border: 1px solid black; text-align: center;"> 6,61 × 10−4 </td>
<td style="color: black; border: 1px solid black; text-align: center;">  6,61 × 10−4  </td>
<td style="color: black; border: 1px solid black; text-align: center;"> 3,39 × 10−4 </td>
</tr>
</tbody>
</table>
Por fim, as concentrações de equilíbrio podem ser substituídas na expressão Kc e resolvidas:
<img alt="Eq6" src="/files/ftp_upload/11388/11388_Equation_6.png" style="text-align: center; height: 90px;" />
Este texto foi adaptado de <a href="https://openstax.org/books/chemistry-2e/pages/13-4-equilibrium-calculations">Openstax, Chemistry 2e, Section 13.4 Equilibrium Calculations</a>.

Cálculo da Constante de Equilíbrio

A constante de equilíbrio para uma reação é calculada a partir das concentrações de equilíbrio (ou pressões) de seus reagentes e produtos. Se estes ...

Education

JoVE Core

Química

Chemical Equilibrium

Equilíbrio Químico

KEY TERMS AND CONCEPTS

TERMOS-CHAVE E CONCEITOS

finding kc from equilibrium data

The equilibrium constant, Kc, can be found from the equilibrium concentrations of reactants and products. When those concentrations are known, the calculation is straightforward. The values are placed into the Kc expression for the reaction.

One example uses nitrogen dioxide and dinitrogen tetroxide. When 0.10 mol NO2 is added to a 1.0-L flask at 25 °C, the concentrations change until equilibrium is reached. At equilibrium, [NO2] is 0.016 M and [N2O4] is 0.042 M, and these values are used to calculate the equilibrium constant for the reaction.

A more advanced example uses reaction stoichiometry to find equilibrium concentrations from the information given. This method is useful for many equilibrium calculations. It tracks the amount present at the start, how it changes as the reaction proceeds, and the amount present at equilibrium. The acronym ICE is used for this approach, and the values are often organized in an ICE table.

The iodine example shows how this works. I2 reacts reversibly with iodide ions to form triiodide ions. If a solution starts with 1.000 × 10^-3 M I2 and 1.000 × 10^-3 M I−, and the equilibrium concentration of I2 is 6.61 × 10^-4 M, the equilibrium constant can be found for the reaction.

To do this, the initial concentrations of the reactants and the equilibrium concentration of the product are used to build an ICE table. The table shows I2, I−, and I3− with initial, change, and equilibrium entries. From the given equilibrium value for I2, the other concentrations can be calculated, including 6.61 × 10^-4 M for I2 and I− and 3.39 × 10^-4 M for I3−.

Once the equilibrium concentrations are known, they are substituted into the Kc expression and solved. This same strategy links the ICE table to the final equilibrium constant. It is a practical way to handle equilibrium problems in chemistry.

Finding Kc from Equilibrium Data

the equilibrium constant

Chemical Equilibrium and Kc Rules

Chemical equilibrium and the equilibrium constant Kc describe how reactants and products are balanced in a reaction. In the oxidation of sulfur dioxide, a mixture that starts with reactants only has no product at first. As the reaction moves forward toward equilibrium, reactant concentrations decrease and product concentration increases. When equilibrium is reached, the concentrations of both stay constant. A reaction can also begin with only products present. In that case, the reaction moves...

homogeneous equilibria for gaseous reactions

homogeneous-equilibria-for-gaseous-reactions

Relating Kc and Kp in Gas Equilibria

Gas-phase equilibrium can be written using either concentration or pressure. The equilibrium constant may be shown as Kc, which uses molar concentration, or as Kp, which uses partial pressure of the reactants and products. The link between Kc and Kp comes from the ideal gas equation and the definition of molarity. Molarity is the number of moles divided by volume. In the ideal gas equation, P stands for partial pressure, V for volume, n for number of moles, R for the gas constant, and T for...

le chatelier's principle: changing concentration

le-chatelier-s-principle-changing-concentration

Shifting Equilibrium by Changing Concentration

Chemical equilibrium is a dynamic balance. At equilibrium, the forward and reverse reactions happen at equal rates. If the system is stressed in a way that changes one rate more than the other, it is no longer at equilibrium and will shift until balance is restored. This behavior is described by Le Châtelier’s principle. Changes in concentration are a major stress on an equilibrium system. Reaction rates depend mainly on concentration and temperature. For that reason, changing the amount of a...

calculating the equilibrium constant

The equilibrium constant, Kc, can be found from the equilibrium concentrations of reactants and products. When those concentrations are known, the calculation is straightforward. The values are placed into the Kc expression for the reaction. One example uses nitrogen dioxide and dinitrogen tetroxide. When 0.10 mol NO2 is added to a 1.0-L flask at 25 °C, the concentrations change until equilibrium is reached. At equilibrium, [NO2] is 0.016 M and [N2O4] is 0.042 M, and these values are used to...

reaction quotient

Using Q to Track Equilibrium Changes

Reaction quotient Q helps track how far a reversible reaction has moved toward equilibrium. For a balanced reaction such as m A + n B ⇌ x C + y D, Q comes directly from the stoichiometric coefficients in the equation. When concentrations are used, the expression is written as Qc. For gases, a similar form uses partial pressures. These expressions use relative concentration and pressure values, not absolute values. That means reaction quotients are dimensionless and have no units. As a reaction...

dynamic equilibrium

Chemical Equilibrium in Reversible Reactions

Chemical equilibrium in reversible reactions happens when a reaction moves in both directions at the same time. A reversible reaction uses a double arrow to show that products can turn back into reactants. At equilibrium, the concentrations of reactants and products stay constant over time because the forward and reverse reaction rates are equal. The video uses the reversible decomposition of colorless dinitrogen tetroxide to brown nitrogen dioxide as an example. At time zero, there is finite...

calculating equilibrium concentrations

Equilibrium Concentrations from an ICE Table

Equilibrium concentrations can be found from initial concentrations and an equilibrium constant. This skill matters in many areas of science and technology, including pharmaceutical product formulation and dosing. After a drug is ingested or injected, it may take part in several chemical equilibria that change its final concentration in the body system of interest. Scientists use these quantitative equilibrium relationships to help calculate a dosage that will produce the desired therapeutic...

le chatelier's principle: changing volume (pressure)

le-chatelier-s-principle-changing-volume-pressure

Gas Equilibrium Under Volume Changes

Gas-phase equilibrium can shift when the volume of the system changes. In these reactions, a change in pressure changes concentration because the partial pressure of an ideal gas is proportional to its molar concentration. That means pressure changes affect equilibrium in the same way as concentration changes. When the volume of a gas mixture changes, the concentrations of reactants and products change together. Since every gas in the equilibrium occupies the same space, the same volume change...

le chatelier's principle: changing temperature

le-chatelier-s-principle-changing-temperature

Le Chatelier's Principle in Heating and Cooling

Le Chatelier's principle helps explain how chemical equilibrium responds to heating and cooling. A system at equilibrium will shift to restore balance after a temperature change, but the equilibrium constant, K, will not stay the same. Instead, the mixture reaches a new equilibrium with a different composition. This temperature effect is different from a concentration change, which shifts equilibrium without changing K. To understand why temperature matters, the reaction can be written with...

the small x assumption

Estimating Equilibrium with Small Changes

A small equilibrium constant can make equilibrium calculations easier. In these reactions, the equilibrium position favors the reactants. When the initial reactant concentration is high and the Kc value is small, the change in concentration may be negligible. In that case, the equilibrium concentration is close to the initial concentration. This idea helps simplify weak acid and weak base problems. Chemists can assume that some equilibrium concentrations are equal to the initial concentrations.

key terms and concepts

Use equilibrium concentrations and ICE tables to find Kc in chemistry. See how nitrogen dioxide and iodine examples connect data to the equilibrium constant.

Finding Kc from Equilibrium Data | JoVE K12

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Finding Kc from Equilibrium Data

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