Question

Укажите факторы, способствующие смещению вправо равновесия реакции СО(Г) + Н2O(Г) ⇄ СО2(Г) + Н2(Г); Н < 0,

Answer 1

1) понижение температуры, т.к. экзотермическая реакция
2) увеличение концентрации CO или H2O
изменение давления не влияет 

Answer 2

Factors contributing to the rightward shift of the equilibrium reaction CO(G) + H2O(G) ⇄ CO2(G) + H2(G); ΔN < 0

The rightward shift of the equilibrium reaction CO(G) + H2O(G) ⇄ CO2(G) + H2(G) occurs when certain factors are present. Here are some factors that can contribute to this shift:

1. Changes in concentration: Increasing the concentration of CO or H2O or decreasing the concentration of CO2 or H2 can shift the equilibrium to the right. This is based on Le Chatelier's principle, which states that if the concentration of a reactant is increased or the concentration of a product is decreased, the equilibrium will shift in the direction that reduces the change in concentration.

2. Changes in pressure: If the reaction involves gases, changes in pressure can also affect the equilibrium position. Increasing the pressure can shift the equilibrium to the side with fewer moles of gas, while decreasing the pressure can shift the equilibrium to the side with more moles of gas. In the given reaction, there is no change in the number of moles of gas, so pressure changes would not have a significant effect on the equilibrium position.

3. Changes in temperature: Altering the temperature can also influence the equilibrium position. In an exothermic reaction (releases heat), increasing the temperature will shift the equilibrium to the left, while decreasing the temperature will shift it to the right. In an endothermic reaction (absorbs heat), the opposite is true. Without information about the enthalpy change of the reaction, it is not possible to determine the effect of temperature on the equilibrium position.

4. Catalysts: The presence of a catalyst does not affect the equilibrium position but can increase the rate at which the equilibrium is reached. A catalyst provides an alternative reaction pathway with lower activation energy, allowing the reaction to proceed more quickly. However, it does not change the position of the equilibrium.

Please note that the specific conditions and context of the reaction can also influence the equilibrium position. Without additional information, it is challenging to provide a more detailed analysis.