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

Stałą równowagi, Kc, można wyznaczyć, podstawiając odpowiednie wartości do wyrażenia stałej równowagi, jeśli znane są stężenia wszystkich reagentów i produktów w stanie równowagi.
Gazową mieszaninę dwutlenku siarki i tlenu w temperaturze 530 °C dopuszcza się do reakcji zgodnie z przedstawioną reakcją. W stanie równowagi mieszanina zawiera 0,10 mola dwutlenku siarki, 0,15 mola tlenu i 10,88 mola trójtlenku siarki. 
Podstawiając wartości do wyrażenia równowagi, Kc wynosi 7,9 × 104. 
Kc można również obliczyć, o ile znane jest początkowe stężenie wszystkich składników i stężenie równowagowe co najmniej jednego związku.
Nieznane stężenia równowagowe można następnie obliczyć za pomocą stechiometrii reakcji. Tabela ICE służy do organizowania informacji o stężeniach początkowych, zmianowych i równowagowych reakcji.
Gdy mieszanina reakcyjna zawierająca 0,11 molowego azotu i 0,36 molowego wodoru osiągnie równowagę w temperaturze 500 °C, w stanie równowagi wytwarza 0,020 molowego amoniaku. Aby obliczyć Kc, należy określić stężenia równowagowe azotu i wodoru.
Stechiometria reakcji pokazuje, że do wytworzenia 2 moli gazowego amoniaku potrzeba 1 mola gazowego azotu i 3 moli gazowego wodoru.
Zmiana x, pomnożona przez współczynniki reagentów i produktów, oznacza stężenie zużytych reagentów i stężenie produktu wytworzonego w celu osiągnięcia równowagi. 
Ponieważ 2x równa się 0,020, x równa się 0,010. Stężenie równowagowe azotu i wodoru można następnie określić, odejmując odpowiednią zmianę stężenia od ich stężenia początkowego, które wynosi odpowiednio 0,10 i 0,33 mola.
Podstawiając stężenia równowagowe w wyrażeniu Kc, Kc wynosi 0,11.
Kp dla reakcji z udziałem gazów można obliczyć za pomocą tabeli ICE, a wyrażenie równowagi zapisać za pomocą ciśnień cząstkowych.

obliczanie stałej równowagi

Stałą równowagi reakcji oblicza się na podstawie stężeń równowagowych (lub ciśnień) jej reagentów i produktów. Jeśli te stężenia są znane, obliczenia obejmują po prostu ich podstawienie do wyrażenia Kc.

Na przykład gazowy dwutlenek azotu tworzy czterotlenek diazotu zgodnie z następującym równaniem:

<img alt="Eq1" src="/files/ftp_upload/11388/11388_Equation_1.png" style="text-align: center; height: 50px;" />

Po dodaniu 0,10 mola NO2 do 1,0-litrowej kolby w temperaturze 25°C stężenie zmienia się tak, że w stanie równowagi [NO2] = 0,016 M i [N2O4] = 0,042 M. Wartość stałej równowagi reakcji może wynosić obliczone w następujący sposób:

<img alt="Eq2" src="/files/ftp_upload/11388/11388_Equation_2.png" style="text-align: center; height: 90px;" />

Następny przykład jest nieco bardziej wymagający. Stechiometrię reakcji wykorzystuje się tutaj do obliczenia stężeń równowagowych na podstawie dostarczonych informacji. Podstawowa strategia tych obliczeń jest pomocna w wielu typach obliczeń równowagi i opiera się na użyciu terminów określających początkowo obecne stężenia reagentów i produktów, ich zmiany w miarę postępu reakcji oraz tego, jak zachowują się, gdy układ osiąga równowagę. W odniesieniu do tego podejścia matematycznego powszechnie używa się akronimu ICE, a terminy dotyczące koncentracji są zwykle gromadzone w formie tabelarycznej zwanej tabelą ICE.

Obliczanie stałej równowagi

Cząsteczki jodu reagują odwracalnie z jonami jodkowymi, tworząc jony trójjodkowe.

<img alt="Eq3" src="/files/ftp_upload/11388/11388_Equation_3.png" style="text-align: center; height: 50px;" />

Jeśli roztwór o stężeniach I2 i I− obu równych 1,000 × 10-3 M przed reakcją daje równowagowe stężenie I2 równe 6,61 × 10-4 M, jaka jest stała równowagi dla tej reakcji?

Aby obliczyć stałe równowagi, potrzebne są stężenia równowagowe dla wszystkich reagentów i produktów:

<img alt="Eq4" src="/files/ftp_upload/11388/11388_Equation_4.png" style="text-align: center; height: 90px;" />

Podano początkowe stężenia reagentów i stężenie równowagowe produktu. Informacje te można wykorzystać do wyprowadzenia warunków dla stężeń równowagowych reagentów, przedstawiając wszystkie informacje w tabeli ICE.

<div class="overflow">
<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;">Stężenie początkowe (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;">Zmień (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;">Stężenie równowagowe (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>
</div>

<img alt="Eq5" src="/files/ftp_upload/11388/11388_Equation_5.png" style="text-align: center; height: 90px;" />

Tabela ICE może być teraz aktualizowana o wartości liczbowe dla wszystkich jej stężeń:

<div class="overflow">
<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;">Stężenie początkowe (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;">Zmiana (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;">Stężenie równowagowe (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>
</div>

<img alt="Eq6" src="/files/ftp_upload/11388/11388_Equation_6.png" style="text-align: center; height: 90px;" />

Obliczanie stałej równowagi

Stałą równowagi dla reakcji oblicza się na podstawie stężeń (lub ciśnień) równowagi jej reagentów i produktów. Jeśli te ...

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Chemical Equilibrium

Równowaga chemiczna

KEY TERMS AND CONCEPTS

Kluczowe terminy i pojęcia

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

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Shifting Equilibrium by Changing Concentration

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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...

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

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calculating equilibrium concentrations

Equilibrium Concentrations from an ICE Table

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Gas Equilibrium Under Volume Changes

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Le Chatelier's Principle in Heating and Cooling

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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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