Name: equilibrium concentrations from an ice table
Uploaded: 2020-09-24T15:06:50.000Z
Duration: 2 min 5 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.5.2

Calculating Equilibrium Concentrations

Bilinmeyen denge konsantrasyonları, reaktanların başlangıç konsantrasyonundan ve reaksiyon için denge sabiti K'den belirlenebilir. 0, 30 molar nitrojen gazı ve 0, 40 molar oksijen gazının nitrik oksit gazı üretmek için reaksiyona girdiği ve K'nin 0, 10 olduğu reaksiyonu düşünün. Denge konsantrasyonlarını hesaplamak için bilinen değerler bir ICE tablosunda tablo halinde verilmiştir.Konsantrasyondaki değişiklik için, sırasıyla her ürün veya reaktan için artış veya azalma, stokiyometrik katsayısının x katı ile gösterilir. Toplam veya fark, daha sonra denge ifadesine yerleştirilen denge konsantrasyonlarını bulmak için kullanılır. X'i bulmak için, ifade genişletilir ve tüm terimler bir kenara konarak onu şu forma dönüştürür:ax kare artı bx artı c.Bu denklem ikinci dereceden formül kullanılarak çözülebilir. Çözme, x için iki değerle sonuçlanır:0, 047 ve negatif 0, 065. Bir maddenin negatif konsantrasyonu imkansız olduğundan, değer reddedilebilir.X için 0, 047 kullanıldığında, nitrojen, oksijen ve nitrik oksidin denge konsantrasyonları sırasıyla 0, 25, 0, 35 ve 0, 094 molara eşittir. Tam kare koşulu, ikinci dereceden formülden kaçınmak için bir kısayolun kullanılabileceği bir durumdur. Örneğin, yukarıdaki reaksiyondaki ilk nitrojen ve oksijen konsantrasyonlarının her biri 0, 30 molar idi, ve denklem tam bir kare haline geldi.Bu gibi durumlarda, denklem, x'i bulmak için her iki tarafın karekökü alınarak basitleştirilebilir.

<ol>
	<li>Lim, Kieran F. "Kimyada grafik hesap makinelerini ve elektronik tabloları kullanma: Denge problemlerini çözme." Kimya Eğitimi Dergisi 85, no. 10 (2008): 1347. <a href="https://pubs.acs.org/doi/pdf/10.1021/ed085p1347">https://pubs.acs.org/doi/pdf/10.1021/ed085p1347</a></li>
</ol>

denge konsanstrasyonlarını hesaplama

Denge konsantrasyonlarını hesaplayabilmek, bilim ve teknolojinin birçok alanı — örneğin farmasötik ürünlerin formülasyonu ve dozajında— için gereklidir. Bir ilaç yutulduktan veya enjekte edildikten sonra, tipik olarak, ilgilenilen vücut sistemindeki nihai konsantrasyonunu etkileyen birkaç kimyasal dengeye dahil olur. İstenen terapötik etkiyi sağlayacak bir dozaj miktarını hesaplamak için bu dengelerin nicel yönleri hakkında bilgi sahibi olunması gerekir.
 
 Denge konsantrasyonlarının, başlangıç konsantrasyonlarından ve denge sabitinden türetildiği bir hesap daha zorlu bir denge hesaplama türü olabilir. Bu hesaplamalar için genellikle dört adımlı bir yaklaşım kullanışlı olmaktadır:
 <ol>
 <li>Reaksiyonun dengeye ulaşmak için ilerleyeceği yönü belirleyin.</li>
 <li>Bir ICE tablosu geliştirin.</li>
 <li>Konsantrasyon değişikliklerini ve daha sonra denge konsantrasyonlarını hesaplayın.</li>
 <li>Hesaplanan denge konsantrasyonlarını doğrulayın.</li>
 </ol>
 
 Denge Konsantrasyonlarının Hesaplanması
 
 Belirli koşullar altında, PCl 5(g) 'nin PCl3(g) ve Cl2(g)'ye ayrışması için denge sabitiKc 0,0211'dir. Yukarıdaki prosedür, başlangıçta 1,00 m'lik bir konsantrasyonda sadece PCl5 içeren bir karışımda PCl5, PCl3 ve Cl2 denge konsantrasyonlarını belirlemek için kullanılabilir.
 
 1. Adım Reaksiyonun hangi yönde ilerlediğini belirleyin.
 
 PCl5 ayrışması için dengeli denklem şu şekildedir:
 
 <img alt=""Eq1"" src=""/files/ftp_upload/11390/11390_Equation 1.png"" style=""text-align: center; height: 50px;"" />
 
 Başlangıçta sadece reaktan mevcut olduğundan, Qc = 0 ve reaksiyon sağa doğru ilerleyecektir.
 
 2. Adım Bir ICE tablosu geliştirin.
 <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;"">     PCl5 (g)     </td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">  PCl3 (g)   </td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">  Cl2 (g)  </td>
 </tr>
 <tr>
 <td style=""color: black; border: 1px solid black; text-align: center;"">Başlangıç Konsantrasyonu (M)</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">1,00</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">0</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;"">Değişim (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;"">Denge Konsantrasyonu (M)</td>
 <td style=""color: black; border: 1px solid black; text-align: center;"">1,00 − 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>
 </tbody>
 </table>
 
 3. Adım Değişim ve denge konsantrasyonları için çözün.
 
 Denge konsantrasyonlarının denge sabiti denklemi yerine geçmesi şunu verir:
 
 <img alt=""Eq2"" src=""/files/ftp_upload/11390/11390_Equation 2.png"" style=""text-align: center; height: 170px;"" />
 
 ax2 + bx + c = 0 formun bir denklemi, x’i çözmek için yeniden düzenlenebilir:
 
 <img alt=""Eq3"" src=""/files/ftp_upload/11390/11390_Equation 3.png"" style=""text-align: center; height: 90px;"" />
 
 Bu durumda, a = 1, b = 0,0211, and c = −0,0211. a, b ve c için uygun değerlerin değiştirilmesi şunu verir:
 
 <img alt=""Eq4"" src=""/files/ftp_upload/11390/11390_Equation 4.png"" style=""text-align: center; height: 90px;"" />
 
 Bu yüzden ikinci dereceden iki kök,
 
 <img alt=""Eq5"" src=""/files/ftp_upload/11390/11390_Equation 5.png"" style=""text-align: center; height: 50px;"" />
 
 Bu senaryo için, sadece pozitif kök fiziksel olarak anlamlıdır( konsantrasyonlar sıfır veya pozitiftir) ve bu nedenle x = 0,135 M. Denge konsantrasyonları:
 
 <img alt=""Eq6"" src=""/files/ftp_upload/11390/11390_Equation 6.png"" style=""text-align: center; height: 130px;"" />
 
 4. Adım Hesaplanan denge konsantrasyonlarını doğrulayın.
 
 Kc için tanımı değiştirme (hesaplamayı kontrol etmek için) şunu verir:
 
 <img alt=""Eq7"" src=""/files/ftp_upload/11390/11390_Equation 7.png"" style=""text-align: center; height: 90px;"" />
 
 Denge konsantrasyonlarından hesaplanan denge sabiti, (uygun sayıda anlamlı rakamlara yuvarlandığında) problemde verilen Kc değerine eşittir.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href=""https://openstax.org/books/chemistry-2e/pages/13-4-equilibrium-calculations"">Openstax, Chemistry 2e, Section 13.4 Equilibrium Calculations</a><a href=""https://openstax.org/books/chemistry-2e/pages/13-4-equilibrium-calculations"">.</a>

Denge Konsanstrasyonlarını Hesaplama

Denge konsantrasyonlarını hesaplayabilmek, bilim ve teknolojinin birçok alanı için esastır - örneğin, formülasyon ve dozajlamada ...

Education

JoVE Core

Kimya

Chemical Equilibrium

Kimyasal Denge

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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 effect.

A common approach is needed when equilibrium concentrations must be derived from starting values and a known Kc. The first step is to decide which way the reaction will move to reach equilibrium. Next, an ICE table is set up. ICE stands for initial, change, and equilibrium. After that, the concentration changes are solved and used to find the equilibrium concentrations. The final step is to check the answer.

The decomposition of PCl5(g) into PCl3(g) and Cl2(g) shows how this works. In the example, Kc is 0.0211, and the mixture starts with only PCl5 at 1.00 M. Because only the reactant is present at the start, Qc equals 0, so the reaction moves to the right. The ICE table gives an initial concentration of 1.00 M for PCl5 and 0 for the products, with changes of -x, +x, and +x.

Substituting the equilibrium values into the Kc expression leads to a quadratic equation. Solving it gives two roots, but only the positive root is physically meaningful because concentrations cannot be negative. In this case, x = 0.135 M. The equilibrium concentrations are then found for PCl5, PCl3, and Cl2. A final substitution into the Kc expression confirms that the calculated value matches the given equilibrium constant when rounded correctly.

Equilibrium Concentrations from an ICE Table

equilibrium-concentrations-from-an-ice-table

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

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Relating Kc and Kp in Gas Equilibria

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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

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...

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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 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)

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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

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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

Learn how to find equilibrium concentrations with an ICE table, use Kc, and check answers with a PCl5 decomposition example for high school chemistry.

Equilibrium Concentrations from an ICE Table | JoVE K12

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Physical Science

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Equilibrium Concentrations from an ICE Table

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