Question

Определить, как изменится константа равновесия реакции 4Р + 3О2 ↔ 2Р2О3 (О2 и Р2О3), если увеличить концентрацию кислорода и фосфора в 2 раза? Сформулировать принцип, используемый при решении данной задачи. 3

Answer 1

Kp=[P2O3]^2/([P]^4*[O2]^3) =>  таким образом, если увеличить к-ции исходных веществ в 2 раза, то принимая во внимания степени, стоящие при той или иной к-циии, получится, что константа равновесия уменьшится в (2^4)*(2^3)=16*9=144 раза

Answer 2

Changes in Equilibrium Constant and the Principle Used

When the concentrations of reactants or products in a chemical reaction are changed, it can affect the equilibrium position and the value of the equilibrium constant. In this case, we have the reaction:

4P + 3O2 ↔ 2P2O3 (O2 and P2O3)

If the concentrations of oxygen (O2) and phosphorus (P) are both increased by a factor of 2, we need to determine how this change will affect the equilibrium constant.

The principle used to solve this problem is Le Chatelier's principle. According to this principle, when a system at equilibrium is subjected to a change in concentration, pressure, or temperature, it will respond in a way that tends to counteract the change and restore equilibrium.

Applying Le Chatelier's Principle

In this case, increasing the concentrations of oxygen and phosphorus by a factor of 2 will disturb the equilibrium of the reaction. Let's analyze the effect of this change on the equilibrium position and the equilibrium constant.

1. Effect on the Equilibrium Position: - Increasing the concentration of oxygen (O2) will shift the equilibrium to the right, favoring the formation of products (P2O3). - Increasing the concentration of phosphorus (P) will also shift the equilibrium to the right, favoring the formation of products (P2O3). - Therefore, the equilibrium position will shift to the right, resulting in an increase in the concentration of P2O3.

2. Effect on the Equilibrium Constant: - The equilibrium constant (K) is a measure of the ratio of product concentrations to reactant concentrations at equilibrium. - When the concentrations of reactants or products change, the equilibrium constant remains constant as long as the temperature is constant. - Therefore, increasing the concentrations of oxygen and phosphorus will not change the value of the equilibrium constant (K).

Conclusion

In summary, if the concentrations of oxygen and phosphorus in the reaction 4P + 3O2 ↔ 2P2O3 are increased by a factor of 2, the equilibrium position will shift to the right, favoring the formation of products (P2O3). However, the equilibrium constant (K) will remain unchanged.

The principle used to solve this problem is Le Chatelier's principle, which states that a system at equilibrium will respond to a change in concentration by shifting the equilibrium position in a way that tends to counteract the change and restore equilibrium.