Question

Действием каких факторов можно сместить равновесие в сторону пря-мой химической реакции Fe(т) +2HCl(ж) FeCl2(ж) + Н2(г)? ∆Н > 0

Answer 1

Если ∆Н > 0, то -Q. Соответственно, при повышении температуры равновесие смещается в сторону прямой реакции. При прямой реакции образуется газ, значит, надо уменьшить давление. Можно увеличить концентрацию исходных веществ или уменьшить концентрацию продуктов.

Answer 2

Factors that can shift the equilibrium towards the forward reaction Fe(s) + 2HCl(l) → FeCl2(l) + H2(g) when ΔH > 0

There are several factors that can shift the equilibrium of a chemical reaction towards the forward reaction Fe(s) + 2HCl(l) → FeCl2(l) + H2(g) when ΔH > 0. These factors include:

1. Increasing the concentration of reactants: According to Le Chatelier's principle, increasing the concentration of reactants can shift the equilibrium towards the products. In this case, increasing the concentration of Fe(s) and HCl(l) can favor the formation of FeCl2(l) and H2(g) [[1]].

2. Decreasing the concentration of products: Similarly, decreasing the concentration of products (FeCl2(l) and H2(g)) can also shift the equilibrium towards the products. This can be achieved by removing some of the FeCl2(l) and H2(g) from the reaction mixture [[1]].

3. Increasing the pressure: If the reaction involves gases, increasing the pressure can shift the equilibrium towards the side with fewer moles of gas. In this case, increasing the pressure can favor the formation of FeCl2(l) and H2(g) since there are fewer moles of gas on the product side [[1]].

4. Increasing the temperature: Increasing the temperature can favor the endothermic reaction, which is the forward reaction in this case. Since the forward reaction is endothermic (ΔH > 0), increasing the temperature can shift the equilibrium towards the formation of FeCl2(l) and H2(g) [[1]].

5. Using a catalyst: A catalyst can increase the rate of the reaction without being consumed in the process. By increasing the rate of the forward reaction, a catalyst can help shift the equilibrium towards the products [[1]].

It's important to note that these factors can shift the equilibrium but do not change the value of ΔH for the reaction. ΔH represents the heat change associated with the reaction and is independent of the factors that can shift the equilibrium.

I hope this helps! Let me know if you have any further questions.