Predict the effect of decreasing the temperature on the position of the

following equilibria.

(a) H2(g) + Cl2(g) ↔ 2HCl(g) + 49.7 kJ

My answer: shifts to the right


(b) 2NH3(g) ↔ N2(g) + 3H2(g) ∆ H = 37.2 kJ

My answer: shifts to the left

(c) CO(g) + H2O(g) ↔ CO2(g) + H2(g) ∆ H = -27.6 kJ

My answer: shifts to the right

youre bald

Angus fr spitting

shut it

angus chill

(a) Well, it's getting colder in here, so H2 and Cl2 might want to cuddle up more. So, the equilibrium would shift to the right. They'll be making more HCl than a reality TV show makes drama.

(b) Oh boy, it's chilly out here! So, the ammonia molecules might start feeling a bit lazy and prefer to stick together as NH3. That means the equilibrium would shift to the left. Looks like N2 and H2 will have to find another party to crash.

(c) Brrr, it's freezing! In this icy weather, CO and H2O decide to get cozy and form CO2 and H2. So, the equilibrium would shift to the right. It's like they're doubling up to stay warm, just like penguins in tuxedos!

To predict the effect of decreasing temperature on the position of the equilibria, we need to consider Le Chatelier's principle. According to this principle, changes in temperature will cause the system to shift in a direction that minimizes the effects of the change.

For each of the given equilibria, let's analyze the effects of decreasing temperature:

(a) H2(g) + Cl2(g) ↔ 2HCl(g) + 49.7 kJ
In this reaction, heat is released (exothermic) since the reaction has a positive enthalpy (∆H) value. Decreasing the temperature would shift the equilibrium towards the exothermic side to counteract the decrease. Hence, the reaction would shift to the right to produce more heat. Your answer is correct.

(b) 2NH3(g) ↔ N2(g) + 3H2(g) ∆H = 37.2 kJ
This reaction is also exothermic since the reaction has a positive ∆H value. Decreasing the temperature would shift the equilibrium to the side that produces more heat. In this case, it would shift to the left to decrease the amount of heat produced. Therefore, your answer of shifting to the left is correct.

(c) CO(g) + H2O(g) ↔ CO2(g) + H2(g) ∆H = -27.6 kJ
Unlike the previous reactions, this reaction is endothermic since the reaction has a negative ∆H value. Decreasing the temperature would shift the equilibrium to the side that produces more heat. In this case, the reaction would shift to the right to increase the heat generation. Hence, your answer of shifting to the right is correct.

In summary, decreasing the temperature would cause the reactions to shift in the following directions:
(a) to the right
(b) to the left
(c) to the right

correct on them all.