Question

На примере заданного уравнения определите, как температура, концентрация и давление влияют на химическое равновесие в уравнении: 3Н2 + N2 + 2NH3 + 91,84кДж.. Заполните таблицу: Влияние факторов на Химическое равновесие при воздействии следующих факторов химическое Температура Концентрация Давление равновесие При увеличении При уменьшении Помогитеее срочноо дам 100балоов​

Answer 1

The Influence of Temperature, Concentration, and Pressure on Chemical Equilibrium

Chemical equilibrium is a state in a chemical reaction where the forward and reverse reactions occur at equal rates. The equilibrium position of a reaction can be influenced by various factors, including temperature, concentration, and pressure. Let's examine how these factors affect the chemical equilibrium using the given equation:

3H2 + N2 ⇌ 2NH3 + 91.84 kJ

Temperature:

Temperature plays a crucial role in determining the direction in which a chemical reaction proceeds. According to Le Chatelier's principle, an increase in temperature favors an endothermic reaction (absorbs heat), while a decrease in temperature favors an exothermic reaction (releases heat).

In the given equation, the forward reaction is exothermic because it releases energy in the form of 91.84 kJ. Therefore, increasing the temperature will shift the equilibrium in the reverse direction (towards the reactants) to counteract the added heat. Conversely, decreasing the temperature will favor the forward reaction (towards the products) to generate more heat.

Concentration:

Concentration refers to the amount of reactants or products present in a given volume. Changes in concentration can affect the equilibrium position by altering the ratio of reactants to products.

In the given equation, increasing the concentration of any of the reactants (H2 or N2) will shift the equilibrium towards the products (NH3) to consume the excess reactants. Conversely, increasing the concentration of the products will favor the reverse reaction (towards the reactants) to restore equilibrium.

Similarly, decreasing the concentration of any reactant or product will cause the equilibrium to shift in the opposite direction to compensate for the deficiency.

Pressure:

Pressure primarily affects the equilibrium position in reactions involving gases. According to Le Chatelier's principle, an increase in pressure will favor the side of the reaction with fewer moles of gas, while a decrease in pressure will favor the side with more moles of gas.

In the given equation, the stoichiometry shows that the number of moles of gas is the same on both sides. Therefore, changes in pressure will not significantly affect the equilibrium position.

Summary:

To summarize the effects of temperature, concentration, and pressure on the given chemical equilibrium:

- Temperature: Increasing the temperature will favor the reverse reaction (towards the reactants), while decreasing the temperature will favor the forward reaction (towards the products). - Concentration: Increasing the concentration of reactants will shift the equilibrium towards the products, while increasing the concentration of products will favor the reverse reaction. Decreasing the concentration of reactants or products will cause the equilibrium to shift in the opposite direction. - Pressure: Changes in pressure will not significantly affect the equilibrium position in the given equation since the number of moles of gas is the same on both sides.

Please note that the effects of these factors on chemical equilibrium can vary depending on the specific reaction and its stoichiometry.